Chapter 19, Problem 36PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Calculate ΔrG° and the equilibrium constant for the following reactions. (a) Zn2+(aq) + Ni(s) ⇄ Zn(s) + Ni2+(aq) (b) Cu(s) + 2 Ag+(aq) ⇄ Cu2+(aq) + 2 Ag(s)

a)

Interpretation Introduction

Interpretation:

The ΔrGo value and the equilibrium constant for the following reaction has to be determined.

1. a) Zn2+(aq) + Ni(s)Zn(s) + Ni2+(aq)

Concept introduction:

According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system.

The equation is as follows.

ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol  E0= Volts = Work(J)/Charge(C)

The relation between standard cell potential and equilibrium constant is as follows.

lnK = nE00.0257 at 298K

Explanation

The given chemical reaction is as follows.

Zn2+(aq)Â +Â Ni(s)â‡ŒZn(s)Â +Â Ni2+(aq)

Letâ€™s write an each half cell reaction.

AtÂ anode:OxiationÂ :Â Ni(s)Â Â â†’Â Ni2+(aq)Â +Â 2eâˆ’AtÂ cathode:ReductionÂ :Â Zn2+(aq)Â +Â 2eâˆ’â†’Zn(s)

Letâ€™s calculate the Ecello value of the reaction.

Ecello=Â ECathode0-Â EAnode0=Â -0.736Â V-(-0.25Â V)=Â -0.513Â V

Letâ€™s calculate the Î”G0 value for the reaction.

Î”G0=Â -nFE0nÂ =Â 2FÂ =Â 96485C/molÂ Â E0=Â -0

(b)

Interpretation Introduction

Interpretation:

The ΔrGo value and the equilibrium constant for the following reaction has to be determined.

1. a) Cu(s) + 2Ag+(aq)Cu2+(aq) + 2Ag(s)

Concept introduction:

According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system.

The equation is as follows.

ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol  E0= Volts = Work(J)/Charge(C)

The relation between standard cell potential and equilibrium constant is as follows.

lnK = nE00.0257 at 298K

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