Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 21, Problem 21.151P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential for the given cell has to be calculated.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Redox reaction: Redox reaction is a type of chemical reaction, where both the oxidation and reduction occur at the same time. In a redox reaction, one of the reactant is oxidized and the other is reduced simultaneously.

Eocell-the cell potential measured at specified temperature conditions which is used to compare the potentials of different cells since, the Ecell is affected by concentration changes as reaction proceeds and due to energy loss from heating of the cell and external circuit.

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G=-nFE°cell

n - Number of electrons involved per equivalent of the net redox reaction in the cell

F - Faraday’s Constant (96500 C)

E°cell - Standard cell potential.

(a)

Expert Solution
Check Mark

Explanation of Solution

The given information says that two voltaic cells are combined. The half reactions are depicted as follows,

  Au3+(aq)+3eAu(s) E=1.50VCr3+(aq)+3eCr(s) E=0.74VCo2+(aq)+2eCo(s) E=0.28VZn2+(aq)+2eZn(s) E=0.76V

Applying, the formula Ecell=EcathodeEanode, cell potential is determined as follows,

  Ecell=EcathodeEanodeFor cell Au/CrEcell=1.50V(0.74V)                                    =2.24 VFor cell Co/ZnEcell=0.28V(0.76V)                                    =0.48 V.

(b)

Interpretation Introduction

Interpretation:

The total cell potential when two given cells are connected in series has to be calculated.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Redox reaction: Redox reaction is a type of chemical reaction, where both the oxidation and reduction occur at the same time. In a redox reaction, one of the reactant is oxidized and the other is reduced simultaneously.

Eocell-the cell potential measured at specified temperature conditions which is used to compare the potentials of different cells since, the Ecell is affected by concentration changes as reaction proceeds and due to energy loss from heating of the cell and external circuit.

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G=-nFE°cell

n - Number of electrons involved per equivalent of the net redox reaction in the cell

F - Faraday’s Constant (96500 C)

E°cell - Standard cell potential.

(b)

Expert Solution
Check Mark

Explanation of Solution

The given information says that two voltaic cells are combined. The half reactions are depicted as follows,

  Au3+(aq)+3eAu(s) E=1.50VCr3+(aq)+3eCr(s) E=0.74VCo2+(aq)+2eCo(s) E=0.28VZn2+(aq)+2eZn(s) E=0.76V

Applying, the formula Ecell=EcathodeEanode, cell potential is determined as follows,

  Ecell=EcathodeEanodeFor cell Au/CrEcell=1.50V(0.74V)                                    =2.24 VFor cell Co/ZnEcell=0.28V(0.76V)                                    =0.48 V

When two cells are connected in series the total cell potential is obtained by adding the potentials of individual cells present.

    Eseries=EAu/Cr+ECo/Zn= 2.24 V + 0.48V= 2.72 V.

(c)

Interpretation Introduction

Interpretation:

The cell that acts as voltaic cell and the one that act as electrolytic cell present in the given cell has to be identified when the given condition is applied.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Redox reaction: Redox reaction is a type of chemical reaction, where both the oxidation and reduction occur at the same time. In a redox reaction, one of the reactant is oxidized and the other is reduced simultaneously.

Eocell-the cell potential measured at specified temperature conditions which is used to compare the potentials of different cells since, the Ecell is affected by concentration changes as reaction proceeds and due to energy loss from heating of the cell and external circuit.

The Standard Gibb’s free energy change and the standard cell potential are related as followed:

Δ°G=-nFE°cell

n - Number of electrons involved per equivalent of the net redox reaction in the cell

F - Faraday’s Constant (96500 C)

E°cell - Standard cell potential.

(c)

Expert Solution
Check Mark

Explanation of Solution

The difference in voltages occurs when the given cells are connected in series that is connecting (Au/Cr) as voltaic and (Co/Zn) as electrolytic cell. The difference in voltages that is as follows,

    Eseries=EAu/CrECo/Zn= 2.24 V - 0.48V= 1.76 V.

(d)

Interpretation Introduction

Interpretation:

The metal ion that gets reduced in each cell has to be identified.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Redox reaction: Redox reaction is a type of chemical reaction, where both the oxidation and reduction occur at the same time. In a redox reaction, one of the reactant is oxidized and the other is reduced simultaneously.

(d)

Expert Solution
Check Mark

Explanation of Solution

The given information says that two voltaic cells are combined. The half reactions are depicted as follows,

  Au3+(aq)+3eAu(s) E=1.50VCr3+(aq)+3eCr(s) E=0.74VCo2+(aq)+2eCo(s) E=0.28VZn2+(aq)+2eZn(s) E=0.76V

Analyzing the reduction potentials of Au3+ and Cr3+ it is clear that Au3+ gets easily reduced since its reduction potential is higher than Cr3+.

Similarly, analyzing the reduction potentials of Co2+ and Zn2+ it is clear that Co2+ gets easily reduced since its reduction potential is higher than Zn2+.

(e)

Interpretation Introduction

Interpretation:

The amount of metal obtained from electrolytic cell when 2 grams of metal plates out from voltaic cell has to be identified.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Redox reaction: Redox reaction is a type of chemical reaction, where both the oxidation and reduction occur at the same time. In a redox reaction, one of the reactant is oxidized and the other is reduced simultaneously.

(e)

Expert Solution
Check Mark

Explanation of Solution

The difference in voltages occurs when the given cells are connected in series that is connecting (Au/Cr) as voltaic and (Co/Zn) as electrolytic cell. The difference in voltages that is as follows,

    Eseries=EAu/CrECo/Zn= 2.24 V - 0.48V= 1.76 V.

As per above connection, Co/Zn is forced to operate in reverse direction which results in reduction of Zn2+.

Therefore, the mass of zinc produced is calculated as follows,

    ZnMass=2 g Au(1molAu197 g Au)(3mole1molAu)(1molZn2mole)(65.41 g Zn1molZn)=0.996 g Zn.

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Chapter 21 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 21.4 - Prob. 21.6AFPCh. 21.4 - Prob. 21.6BFPCh. 21.4 - Prob. 21.7AFPCh. 21.4 - Prob. 21.7BFPCh. 21.4 - Prob. 21.8AFPCh. 21.4 - Prob. 21.8BFPCh. 21.7 - The most ionic and least ionic of the common...Ch. 21.7 - Prob. 21.9BFPCh. 21.7 - Prob. 21.10AFPCh. 21.7 - Prob. 21.10BFPCh. 21.7 - Prob. 21.11AFPCh. 21.7 - Prob. 21.11BFPCh. 21.7 - In the final steps of the ETC, iron and copper...Ch. 21.7 - Prob. B21.2PCh. 21 - Prob. 21.1PCh. 21 - Prob. 21.2PCh. 21 - Prob. 21.3PCh. 21 - Water is used to balance O atoms in the...Ch. 21 - Prob. 21.5PCh. 21 - Prob. 21.6PCh. 21 - Prob. 21.7PCh. 21 - Prob. 21.8PCh. 21 - Prob. 21.9PCh. 21 - Prob. 21.10PCh. 21 - Prob. 21.11PCh. 21 - Prob. 21.12PCh. 21 - Prob. 21.13PCh. 21 - Prob. 21.14PCh. 21 - Prob. 21.15PCh. 21 - Prob. 21.16PCh. 21 - Prob. 21.17PCh. 21 - Prob. 21.18PCh. 21 - Prob. 21.19PCh. 21 - Prob. 21.20PCh. 21 - Aqua regia, a mixture of concentrated HNO3 and...Ch. 21 - Consider the following general voltaic...Ch. 21 - Why does a voltaic cell not operate unless the two...Ch. 21 - Prob. 21.24PCh. 21 - Prob. 21.25PCh. 21 - Prob. 21.26PCh. 21 - Consider the following voltaic cell: In which...Ch. 21 - Consider the following voltaic cell: In which...Ch. 21 - Prob. 21.29PCh. 21 - Prob. 21.30PCh. 21 - A voltaic cell is constructed with an Fe/Fe2+...Ch. 21 - Prob. 21.32PCh. 21 - Prob. 21.33PCh. 21 - Prob. 21.34PCh. 21 - Prob. 21.35PCh. 21 - What does a negative indicate about a redox...Ch. 21 - Prob. 21.37PCh. 21 - In basic solution, Se2− and ions react...Ch. 21 - Prob. 21.39PCh. 21 - Prob. 21.40PCh. 21 - Use the emf series (Appendix D) to arrange each...Ch. 21 - Prob. 21.42PCh. 21 - Prob. 21.43PCh. 21 - Prob. 21.44PCh. 21 - Prob. 21.45PCh. 21 - Prob. 21.46PCh. 21 - Prob. 21.47PCh. 21 - Prob. 21.48PCh. 21 - Prob. 21.49PCh. 21 - Prob. 21.50PCh. 21 - Prob. 21.51PCh. 21 - Prob. 21.52PCh. 21 - Prob. 21.53PCh. 21 - Prob. 21.54PCh. 21 - Prob. 21.55PCh. 21 - Prob. 21.56PCh. 21 - Prob. 21.57PCh. 21 - Prob. 21.58PCh. 21 - Prob. 21.59PCh. 21 - Prob. 21.60PCh. 21 - Prob. 21.61PCh. 21 - Prob. 21.62PCh. 21 - Prob. 21.63PCh. 21 - Prob. 21.64PCh. 21 - Prob. 21.65PCh. 21 - Prob. 21.66PCh. 21 - Prob. 21.67PCh. 21 - Prob. 21.68PCh. 21 - Prob. 21.69PCh. 21 - Prob. 21.70PCh. 21 - Prob. 21.71PCh. 21 - Prob. 21.72PCh. 21 - Prob. 21.73PCh. 21 - Prob. 21.74PCh. 21 - Prob. 21.75PCh. 21 - Prob. 21.76PCh. 21 - Prob. 21.77PCh. 21 - Prob. 21.78PCh. 21 - Prob. 21.79PCh. 21 - Prob. 21.80PCh. 21 - Prob. 21.81PCh. 21 - Consider the following general electrolytic...Ch. 21 - Prob. 21.83PCh. 21 - Prob. 21.84PCh. 21 - Prob. 21.85PCh. 21 - Prob. 21.86PCh. 21 - In the electrolysis of molten NaBr: What product...Ch. 21 - Prob. 21.88PCh. 21 - Prob. 21.89PCh. 21 - Prob. 21.90PCh. 21 - Prob. 21.91PCh. 21 - Prob. 21.92PCh. 21 - Prob. 21.93PCh. 21 - Prob. 21.94PCh. 21 - Prob. 21.95PCh. 21 - Prob. 21.96PCh. 21 - Prob. 21.97PCh. 21 - Write a balanced half-reaction for the product...Ch. 21 - Prob. 21.99PCh. 21 - Prob. 21.100PCh. 21 - Prob. 21.101PCh. 21 - Prob. 21.102PCh. 21 - Prob. 21.103PCh. 21 - Prob. 21.104PCh. 21 - Prob. 21.105PCh. 21 - Prob. 21.106PCh. 21 - Prob. 21.107PCh. 21 - Prob. 21.108PCh. 21 - Prob. 21.109PCh. 21 - Prob. 21.110PCh. 21 - Prob. 21.111PCh. 21 - Prob. 21.112PCh. 21 - Prob. 21.113PCh. 21 - Prob. 21.114PCh. 21 - Prob. 21.115PCh. 21 - Prob. 21.116PCh. 21 - Prob. 21.117PCh. 21 - Prob. 21.118PCh. 21 - Prob. 21.119PCh. 21 - Prob. 21.120PCh. 21 - To examine the effect of ion removal on cell...Ch. 21 - Prob. 21.122PCh. 21 - Prob. 21.123PCh. 21 - Prob. 21.124PCh. 21 - Prob. 21.125PCh. 21 - Prob. 21.126PCh. 21 - Commercial electrolytic cells for producing...Ch. 21 - Prob. 21.129PCh. 21 - Prob. 21.130PCh. 21 - The following reactions are used in...Ch. 21 - Prob. 21.132PCh. 21 - Prob. 21.133PCh. 21 - Prob. 21.134PCh. 21 - Prob. 21.135PCh. 21 - If the Ecell of the following cell is 0.915 V,...Ch. 21 - Prob. 21.137PCh. 21 - Prob. 21.138PCh. 21 - Prob. 21.139PCh. 21 - Prob. 21.140PCh. 21 - Prob. 21.141PCh. 21 - Prob. 21.142PCh. 21 - Prob. 21.143PCh. 21 - Prob. 21.144PCh. 21 - Prob. 21.145PCh. 21 - Prob. 21.146PCh. 21 - Prob. 21.147PCh. 21 - Both Ti and V are reactive enough to displace H2...Ch. 21 - For the reaction ∆G° = 87.8 kJ/mol Identity the...Ch. 21 - Two voltaic cells are to be joined so that one...Ch. 21 - Prob. 21.152PCh. 21 - Prob. 21.153P
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