Consider an electrochemical cell based on the half-reactions Ni 2+ (aq) + 2 e − → Ni(s) and Cd 2+ (aq) + 2 e − → Cd(s). (a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge). (b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction. (c) What is the polarity of each electrode? (d) What is the value of E ° cell ? (e) In which direction do electrons flow in the external circuit? (f) Assume that a salt bridge containing NaNO 3 connects the two half-cells. In which direction do the Na + (aq) ions move? In which direction do the NO 3 − (aq) ions move? (g) Calculate the equilibrium constant for the reaction. (h) If the concentration of Cd 2+ is reduced to 0.010 M and [Ni 2+ ] = 1.0 M, what is the value of E cell ? Is the net reaction still the reaction given in part (b)? (i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

Question

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Answer 1

Textbook Question

Chapter 19, Problem 99IL

Consider an electrochemical cell based on the half-reactions Ni²⁺(aq) + 2 e⁻ → Ni(s) and Cd²⁺(aq) + 2e⁻ → Cd(s).

(a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge).
(b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction.
(c) What is the polarity of each electrode?
(d) What is the value of E°_cell?
(e) In which direction do electrons flow in the external circuit?
(f) Assume that a salt bridge containing NaNO₃ connects the two half-cells. In which direction do the Na⁺(aq) ions move? In which direction do the NO₃⁻ (aq) ions move?
(g) Calculate the equilibrium constant for the reaction.
(h) If the concentration of Cd²⁺ is reduced to 0.010 M and [Ni²⁺] = 1.0 M, what is the value of E_cell? Is the net reaction still the reaction given in part (b)?
(i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

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Answer 2

Textbook Question

Chapter 19, Problem 99IL

Consider an electrochemical cell based on the half-reactions Ni²⁺(aq) + 2 e⁻ → Ni(s) and Cd²⁺(aq) + 2e⁻ → Cd(s).

(a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge).
(b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction.
(c) What is the polarity of each electrode?
(d) What is the value of E°_cell?
(e) In which direction do electrons flow in the external circuit?
(f) Assume that a salt bridge containing NaNO₃ connects the two half-cells. In which direction do the Na⁺(aq) ions move? In which direction do the NO₃⁻ (aq) ions move?
(g) Calculate the equilibrium constant for the reaction.
(h) If the concentration of Cd²⁺ is reduced to 0.010 M and [Ni²⁺] = 1.0 M, what is the value of E_cell? Is the net reaction still the reaction given in part (b)?
(i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

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Answer 3

Textbook Question

Chapter 19, Problem 99IL

Consider an electrochemical cell based on the half-reactions Ni²⁺(aq) + 2 e⁻ → Ni(s) and Cd²⁺(aq) + 2e⁻ → Cd(s).

(a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge).
(b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction.
(c) What is the polarity of each electrode?
(d) What is the value of E°_cell?
(e) In which direction do electrons flow in the external circuit?
(f) Assume that a salt bridge containing NaNO₃ connects the two half-cells. In which direction do the Na⁺(aq) ions move? In which direction do the NO₃⁻ (aq) ions move?
(g) Calculate the equilibrium constant for the reaction.
(h) If the concentration of Cd²⁺ is reduced to 0.010 M and [Ni²⁺] = 1.0 M, what is the value of E_cell? Is the net reaction still the reaction given in part (b)?
(i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

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Answer 4

Textbook Question

Chapter 19, Problem 99IL

Consider an electrochemical cell based on the half-reactions Ni²⁺(aq) + 2 e⁻ → Ni(s) and Cd²⁺(aq) + 2e⁻ → Cd(s).

(a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge).
(b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction.
(c) What is the polarity of each electrode?
(d) What is the value of E°_cell?
(e) In which direction do electrons flow in the external circuit?
(f) Assume that a salt bridge containing NaNO₃ connects the two half-cells. In which direction do the Na⁺(aq) ions move? In which direction do the NO₃⁻ (aq) ions move?
(g) Calculate the equilibrium constant for the reaction.
(h) If the concentration of Cd²⁺ is reduced to 0.010 M and [Ni²⁺] = 1.0 M, what is the value of E_cell? Is the net reaction still the reaction given in part (b)?
(i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

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Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

Answer 8

(a)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The cell has to be drawn and label each of the component.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 13

Answer to Problem 99IL

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 1

Answer 14

Explanation of Solution

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The voltaic cell are as follows:

Chemistry & Chemical Reactivity, Chapter 19, Problem 99IL , additional homework tip 2

Answer 15

(b)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The balance equation has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 20

Answer to Problem 99IL

Balanced reaction: $Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Answer 21

Explanation of Solution

Let’s write the half reactions occur at anode and cathode:

$At anode:Cd(s) →Cd2+(aq) + 2e-At cathode:Ni2+(aq)+2e- →Ni(s)$

By adding these two half reactions we get balanced reaction.

$Cd(s) →Cd2+(aq) + 2e-Ni2+(aq)+2e- →Ni(s)________________________Cd(s) + Ni2+(aq) →Cd2+(aq) + Ni(s)$

Answer 22

(c)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Anode is negative cathode is positive.

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The polarity of each electrode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 27

Answer to Problem 99IL

Anode is negative cathode is positive.

Answer 28

Explanation of Solution

In the voltaic cell has two voltaic cells. One electrode has positive charge called cathode and another electrode has negative called anode.

Answer 29

(d)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The $Ecello$ has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 34

Answer to Problem 99IL

$Ecello$ of the reaction is $0.15 V$

Answer 35

Explanation of Solution

The reactions occur at anode and cathode is as follows.

$At anode:Cd(s) →Cd2+(aq) + 2e- ; E0= -0.40 VAt cathode:Ni2+(aq)+2e- →Ni(s) ; E0= -0.25 V$

Let’s calculate the $Ecello$ of the reaction

$Ecello=Ecathodeo-Eanodeo= -0.25 V-(-0.40) V= 0.15 V$

Answer 36

(e)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The direction in which electrons flow in the external circuit has to be given.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 41

Answer to Problem 99IL

Electrons are flow from anode to cathode.

Answer 42

Explanation of Solution

In the voltaic cell electrons are move anode to cathode.

Answer 43

(f)

Expert Solution

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Answer 44

(f)

Expert Solution

Answer 45

(f)

Expert Solution

Answer 46

Expert Solution

Answer 47

Interpretation Introduction

Interpretation:

To determine the following.

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

Assume that a salt bride containing $NaNO3$ connect the two half cells. It has to be identified in which direction do $Na+$ (aq) ions and $NO3- (aq)$ move.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 48

Answer to Problem 99IL

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Answer 49

Explanation of Solution

Salt bridge contains $NaNO3$ solution and it is dissociates into $Na+ and NO3-$ ions.

$Na+$ ions moves from anode to cathode

$NO3-$ ions move from cathode to anode

Answer 50

(g)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

Answer 51

(g)

Expert Solution

Answer 52

(g)

Expert Solution

Answer 53

Expert Solution

Answer 54

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The equilibrium constant has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 55

Answer to Problem 99IL

The equilibrium constant of the reaction is $1.1×105$ .

Answer 56

Explanation of Solution

$lnK=nE00.0257=(2)(0.15 V)0.0257=11.673K=1.1 ×105$

Answer 57

(h)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

Answer 58

(h)

Expert Solution

Answer 59

(h)

Expert Solution

Answer 60

Expert Solution

Answer 61

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

If the concentration of $Cd2+(aq)$ is reduced to $0.010 M$ and $[Ni2+]=1.0 M$ . The $Ecello$ of the reaction has to be calculated.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 62

Answer to Problem 99IL

$Ecell$ of the reaction is $0.21 V$ .

Answer 63

Explanation of Solution

$Ecell= Ecello-0.02572lnQ=Ecello-0.02572ln[Cd2+][Ni2+]=0.15 V-0.02572ln(0.010 M)(1.0 M)=0.21 V$

Net reaction will be still given in part (b)

Answer 64

(i)

Expert Solution

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

Answer 65

(i)

Expert Solution

Answer 66

(i)

Expert Solution

Answer 67

Expert Solution

Answer 68

Interpretation Introduction

Interpretation:

The half reactions are as follows.

$Ni2+(aq) + 2e- →Ni(s) and Cd2+(aq)+2e- →Cd(s)$

The time the battery will last if $0.050 M$ is drawn from the battery has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

$Salt bridge ↓Cu(s)|Cu2+(aq) || Ag+(aq)|Ag(s)____________ ___________ ↓ ↓ Half cell Half cell$

Answer 69

Answer to Problem 99IL

The time required for the electrolysis is $4800 h$

Answer 70

Explanation of Solution

$Moles of electrons required:Mole e-= (50 g Cd)(1 mol112.4 mol e-)(2 mol e-1 mol Cd)=0.88896 mol e-$

Let’s calculate the charge of the cell:

$Charge (C) = (0.8896 mol e-)(96500 C1 mol e-)= 8.58 u ×104 C$

Therefore, the time can be calculated as follows.

$Charge = Current (A) × time (s)8.584×104 C= 0.05 A ×time (s)time (s)=1.7×106 S=4800 h$

Answer 71

Ch. 19.1 - Prob. 2CYU Ch. 19.1 - Prob. 3CYU Ch. 19.1 - 1. Copper(II) sulfide reacts with nitric acid...Ch. 19.1 - Prob. 2RC Ch. 19.1 - The balanced half-reaction for Br2 BrO3 in basic...Ch. 19.2 - Describe how to set up a voltaic cell using the...Ch. 19.2 - The following overall chemical reaction occurs in...Ch. 19.2 - Prob. 1RC Ch. 19.2 - Prob. 2RC Ch. 19.2 - Prob. 3RC

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Answer to Problem 99IL

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Answer to Problem 99IL

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Answer to Problem 99IL

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Answer to Problem 99IL

Explanation of Solution

Answer to Problem 99IL

Explanation of Solution

Answer to Problem 99IL

Explanation of Solution

Answer to Problem 99IL

Explanation of Solution

Answer to Problem 99IL

Explanation of Solution

Answer to Problem 99IL

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