Exploring Chemical Analysis
Exploring Chemical Analysis
5th Edition
ISBN: 9781429275033
Author: Daniel C. Harris
Publisher: Macmillan Higher Education
Question
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Chapter 16, Problem 16.15P

(a)

Interpretation Introduction

Interpretation:

Equilibrium constant for the reaction has to be determined.

  I2(aq)+2e2I

Concept Introduction:

For any spontaneous redox reaction the relation between ECell0 and ΔGo is as follows:

    ΔG0=nFEcell0

Here, ΔGo is the standard Gibbs free energy change of the reaction.

ECell0 is cell potential of overall reaction.

n is number of electron transfered.

F is Faraday constant.

The relation between equilibrium constant (K) and ΔGo is as follows:

    ΔG0=RTlnK

Here, ΔGo is standard Gibbs free energy change of the reaction.

K is equilibrium constant of the reaction.

R is gas constant.

T is temperature in Kelvin scale.

Hence the relation between ECell0 and equilibrium constant (K) is as follows:

    K=enFEcell0RT

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant of the reaction has to be determined.

  I2(s)+2e2I

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Solubility of I2 in water has to be determined.

Concept Introduction:

For any spontaneous redox reaction the relation between ECell0 and ΔGo is as follows:

    ΔGo=nFEcell0

Here, ΔGo is the Gibbs free energy change of the reaction.

ECell0 is cell potential of overall reaction.

n is number of electron transferred.

F is Faraday constant.

The relation between equilibrium constant (K) and ΔGo is as follows:

    ΔGo=RTlnK

Here, ΔGo is the Gibbs free energy change of the reaction.

K is equilibrium constant of overall reaction.

R is universal gas constant.

T is temperature in Kelvin scale.

Hence the relation between ECell0 and equilibrium constant (K) is as follows:

    K=enFEcell0RT

For solubility of any element, equilibrium constant (K) of solubility reaction is equal to the solubility of that element.

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