   # The following reaction occurs in pure water: H 2 O ( l ) + H 2 O ( l ) → H 3 O + ( a q ) + OH - ( a q ) which is often abbreviated as H 2 O ( l ) → H + ( a q ) + OH - ( a q ) For this reaction, ∆ G ° = 79.9 kJ/mol at 25°C. Calculate the value of ∆ G for this reaction at 25°C when [OH − ] = 0.15 M and [H + ] = 0.71 M. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 16, Problem 99CWP
Textbook Problem
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## The following reaction occurs in pure water: H 2 O ( l ) + H 2 O ( l ) → H 3 O + ( a q ) + OH - ( a q ) which is often abbreviated as H 2 O ( l ) → H + ( a q ) + OH - ( a q ) For this reaction, ∆G° = 79.9 kJ/mol at 25°C. Calculate the value of ∆G for this reaction at 25°C when [OH−] = 0.15 M and [H+] = 0.71 M.

Interpretation Introduction

Interpretation: The free energy change of the given reaction with the given values of standard free energy change, temperature and concentrations is to be calculated.

Concept Introduction: The free energy change of the given process is calculated by the formula,

ΔG=ΔG+RTlnK

To determine: The value of ΔG for the given reaction.

### Explanation of Solution

Given

The chemical equation for the given reaction is,

H2O(l)H+(aq)+OH(aq)

The concentration of H+ ions is 0.15M .

The concentration of OH ions is 2.4×103M .

The temperature of the reaction is 25°C .

The standard free energy change of the process is 79.9kJ/mol .

The conversion of temperature from °C into Kelvin is done as,

T(K)=T(°C)+273

Hence, the conversion of temperature from 25°C into Kelvin is,

T(K)=(25+273)K=298K

The free energy change per mole for the given process is calculated by the formula,

ΔG=ΔG+RTln([H+][OH])

Where,

• ΔG is the free energy change of the reaction

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