The standard cell potential of the HCO 3 − / CO 3 2 − , H 2 couple has to be predicted. Concept introduction: The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by Δ r G ° whereas Δ r G depends on the reaction condition and extent of reaction.

Question

Want to see the full answer?

Answer 1

Question

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Indicate the order of basicity of primary, secondary and tertiary amines.

> Classify each of the following molecules as aromatic, antiaromatic, or nonaromatic. Cl Z- N O aromatic O antiaromatic O nonaromatic O aromatic O antiaromatic O nonaromatic O aromatic ○ antiaromatic nonaromatic

Please help me answer this question. I don't understand how or even if this can happen in a single transformation. Please provide a detailed explanation and a drawing showing how it can happen in a single transformation. Add the necessary reagents and reaction conditions above and below the arrow in this organic reaction. If the products can't be made from the reactant with a single transformation, check the box under the drawing area instead.

Answer 2

Question

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Answer 6

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

Answer 7

Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the $HCO3−/CO32−,H2$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by $ΔrG°$ whereas $ΔrG$ depends on the reaction condition and extent of reaction.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction $Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $pH$ is changed to $7.0$ at $298 K$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,

$Ecell=Ecellο−RTvFlnQ$

Where,

$Ecell$ is the electrode potential of the cell.

$Ecellο$ is the standard electrode potential of the cell.

$R$ is the gas constant.

$T$ is the temperature.

$v$ is the number of electrons.

$F$ is the Faraday’s constant.

$Q$ is the reaction quotient.

Answer 14

Expert Solution & Answer

Answer 15

Expert Solution & Answer

Answer 16

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 17

Ch. 6 - Prob. 6A.1ST Ch. 6 - Prob. 6A.2ST Ch. 6 - Prob. 6B.1ST Ch. 6 - Prob. 6C.1ST Ch. 6 - Prob. 6D.2ST Ch. 6 - Prob. 6A.1DQ Ch. 6 - Prob. 6A.2DQ Ch. 6 - Prob. 6A.1AE Ch. 6 - Prob. 6A.1BE Ch. 6 - Prob. 6A.2AE

Videos

Want to see the full answer?

Chapter 6 Solutions