Chapter 19, Problem 90GQ

### 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

# Use the table of standard reduction potentials (Appendix M) to calculate ΔrG° for the following reactions at 298 K. (a) ClO3−(aq) + 5 Cl−(aq) + 6 H+(aq) → 3 Cl2(g) + 3 H2O(ℓ) (b) AgCI(s) + Br−(aq) → AgBr(s) + Cl−(aq)

(a)

Interpretation Introduction

Interpretation:

The ΔrG0 for the following reaction has to be determined.

(a) ClO3-(aq) + 5Cl-(aq) + 6H+ (aq) 3Cl2(g) + 3H2O(l)

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.

ClO3-(aq)Â +Â 5Cl-(aq)Â +Â 6H+Â (aq)Â â†’3Cl2(g)Â +Â 3H2O(l)

First, we have to find the oxidized and reduced elements.

Oxidation state:

ClO3-xÂ +Â 3(-2)=Â -1xÂ =Â +5

Cl-Â andÂ ClO3- are being oxidized into Cl2 and H2O.

Letâ€™s write an each half cell reaction.

AtÂ anode:OxiationÂ :Â 5Clâˆ’(aq)Â +Â 5eâˆ’Â â†’Â 52Cl2(g)AtÂ cathode:ReductionÂ :Â ClO3âˆ’(aq)Â +Â 6H++5e-â†’12Cl2(g)Â +Â 3H2O

Letâ€™s calculate the Ecello of the reaction

(b)

Interpretation Introduction

Interpretation:

The ΔrG0 for the following reactions has to be determined.

(b) AgCl(s) + Br-(aq) AgBr (s) + Cl-(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

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