   # Calculate equilibrium constants for the following reactions at 298 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. (a) 2 Cl − (aq) + Br 2 ( ℓ ) ⇄ Cl 2 (aq) + 2 Br − (aq) (b) Fe 2+ (aq) + Ag + (aq) ⇄ Fe 3+ (aq) + Ag(s) ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 19, Problem 85GQ
Textbook Problem
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## Calculate equilibrium constants for the following reactions at 298 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. (a) 2 Cl−(aq) + Br2(ℓ) ⇄ Cl2(aq) + 2 Br−(aq) (b) Fe2+(aq) + Ag+(aq) ⇄ Fe3+(aq) + Ag(s)

(a)

Interpretation Introduction

Interpretation:

The equilibrium constants for the following reactions at 298 K have to be determined and also determine the equilibrium is a reactant or product favoured at equilibrium.

(a) 2Cl-(aq) + Br2(l) Cl2(g) + 2Br-(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 of Solution

The given chemical reaction is as follows.

2Cl-(aq) + Br2(l) Cl2(g) + 2Br-(aq)

Let’s write an each half cell reaction.

At anode:Oxiation : Cl2(aq) + 2e  2Cl(aq)At cathode:Reduction : Br2(l) + 2e2Br-(aq)

Let’s calculate the Ecello of the reaction.

Ecello= ECathode0- EAnode0= 1.08 V-(1.36 V)= -0.28 V

Let’s calculate the ΔG0 for the reaction.

ΔG0= -nFE0n = 2F = 96485C/mol  E0= -0

(b)

Interpretation Introduction

Interpretation:

The equilibrium constants for the following reactions at 298 K have to be determined and also determine the equilibrium is a reactant or product favoured at equilibrium.

(b) Fe2+(aq) + Ag+(aq) Fe3+(aq) + Ag(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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