# 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) + Br 2 (l) → Cl 2 (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 - W ΔU = Change in internal energy Q = Heat added to the system W=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. ΔG 0 = -nFE 0 n = Number of moles transferred per mole of reactant and products F = Faradayconstant=96485C/mol E 0 = Volts = Work(J)/Charge(C) The relation between standard cell potential and equilibrium constant is as follows. lnK = nE 0 0 .0257 at 298K

### Chemistry & Chemical Reactivity

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

### Chemistry & Chemical Reactivity

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

#### Solutions

Chapter 19, Problem 89GQ

(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 systemIn 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

(b)

Interpretation Introduction

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