   # Given the thermodynamic data below, calculate ∆S and ∆ S surr for the following reaction at 25°C and 1 atm: XeF 6 ( g ) → XeF 4 ( s ) + F 2 ( g ) Δ H f o (KJ/mol) S °(J/K mol) XeF 6 ( g ) -294 300. XeF 4 ( s ) -251 146 F 2 ( g ) 0 203 ### 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 97CWP
Textbook Problem
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## Given the thermodynamic data below, calculate ∆S and ∆Ssurr for the following reaction at 25°C and 1 atm: XeF 6 ( g ) → XeF 4 ( s ) + F 2 ( g )   Δ H f o (KJ/mol) S°(J/K mol) XeF6(g) -294 300. XeF4(s) -251 146 F2(g) 0 203

Interpretation Introduction

Interpretation: The entropy change of system and surroundings for the given reaction at 25°C and 1atm is to be calculated.

Concept Introduction: The entropy change of the system is the difference of sum of entropy change of products and reactants.

The entropy change of the surroundings is calculated by using the formula,

ΔSsurr=ΔHrxnT

To determine: The entropy change of system and surroundings for the given reaction.

### Explanation of Solution

Given

The balanced chemical equation for the given reaction is,

XeF6(g)XeF4(s)+F2(g)

The temperature of the reaction is 25°C .

The pressure of the reaction is 1atm .

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

T(K)=T(°C)+273.15

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

T(K)=(25+273.15)K=298.15K

The standard entropy change of system for the given reaction is calculated by the formula,

ΔS=nS(products)mS(reactants)=(SXeF4(s)+SF2(g))SXeF6(g)

Substitute the values of SXeF4(s) , SF2(g) and SXeF6(g) from appendix C in equation

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