   Chapter 17, Problem 98CWP

Chapter
Section
Textbook Problem

# Consider the reaction: H 2 S ( g ) + SO 2 ( g ) → 3 S ( g ) + 2 H 2 O ( l ) for which ∆H is −233 kJ and ∆S is −424 J/K.a. Calculate the free energy change for the reaction (∆G) at 393 K.b. Assuming ∆H and ∆S do not depend on temperature, at what temperatures is this reaction spontaneous?

(a)

Interpretation Introduction

Interpretation: The free energy change of the given reaction and the temperature at which the reaction becomes spontaneous is to be calculated.

Concept Interpretation: The free energy change of the given reaction is calculated by using the formula,

ΔG=ΔHTΔS

To determine: The free energy change of the given reaction.

Explanation

Explanation

Given

The balanced chemical equation for the given reaction is,

H2S(g)+SO2(g)3S(g)+2H2O(l)

The enthalpy change of the reaction is 233kJ(=233×103J) .

The entropy change of the reaction is 424J/K .

The temperature of the reaction is 373K .

The free energy change of the given reaction is calculated by using the formula,

ΔG=ΔHTΔS

Where,

• ΔS is the entropy change of the process

(b)

Interpretation Introduction

Interpretation: The free energy change of the given reaction and the temperature at which the reaction becomes spontaneous is to be calculated.

Concept Interpretation: The free energy change of the given reaction is calculated by using the formula,

ΔG=ΔHTΔS

To determine: The temperature at which the given reaction is spontaneous.

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