The standard enthalpy change, and entropy change for the given reaction. Solution: The standard enthalpy change for the given reaction is − 196.6 kJ and the standard entropy change for the reaction is 189.6 J/K . Explanation: Given The balanced chemical reaction is, 2 SO 2 ( g ) + O 2 ( g ) → 2 SO 3 ( g ) The standard entropy change of the reaction is calculated by the formula, Δ H 0 = ∑ n Δ H 0 ( products ) − ∑ m Δ H 0 ( reactants ) = 2 Δ H SO 3 ( g ) 0 − ( 2 Δ H SO 2 ( g ) 0 + Δ H O 2 ( g ) 0 ) Substitute the standard values of Δ H SO 2 ( g ) 0 , Δ H O 2 ( g ) 0 and Δ H SO 3 ( g ) 0 from appendix C in above equation. Δ H 0 = 2 × ( − 395.2 kJ/mol ) − ( 2 mol × ( − 296.9 kJ/mol ) + 1 mol × 0.0 kJ/mol ) = − 196.6 kJ Thus, the standard enthalpy change for the given reaction is − 196.6 kJ . Now, calculate the standard entropy change for the given reaction. The balanced chemical reaction is, 2 SO 2 ( g ) + O 2 ( g ) → 2 SO 3 ( g ) The standard entropy change of the reaction is calculated by the formula, Δ S 0 = ∑ n Δ S 0 ( products ) − ∑ m Δ S 0 ( reactants ) = 2 Δ S SO 3 ( g ) 0 − ( 2 Δ S SO 2 ( g ) 0 + Δ S O 2 ( g ) 0 ) Substitute the standard values of Δ S SO 2 ( g ) 0 , Δ S O 2 ( g ) 0 and Δ S SO 3 ( g ) 0 from appendix C in the above equation. Δ S 0 = 2 × 256.2 J/mol ⋅ K − ( 2 mol × 248.5 J/mol ⋅ K + 1 mol × 205.0 J/mol ⋅ K ) = − 189.6 J/K Thus, the standard entropy change for the given reaction is − 189.6 J/K . Conclusion: The standard enthalpy change for the given reaction is − 196.6 kJ and the standard entropy change for the reaction is 189.6 J/K .

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Chapter 4, Problem 69E

(a)

Interpretation Introduction

To determine: The standard enthalpy change, and entropy change for the given reaction.

Solution: The standard enthalpy change for the given reaction is $−196.6 kJ$ and the standard entropy change for the reaction is $189.6 J/K$ .

Explanation:

Given

The balanced chemical reaction is,
$2SO2(g)+O2(g)→2SO3(g)$

The standard entropy change of the reaction is calculated by the formula,
$ΔH0=∑nΔH0( products)−∑mΔH0( reactants)=2ΔH SO3(g)0−(2ΔH SO 2 ( g )0+ΔH O 2 ( g )0)$

Substitute the standard values of $ΔHSO2(g)0$ , $ΔHO2(g)0$ and $ΔHSO3(g)0$ from appendix C in above equation.
$ΔH0=2×(−395.2 kJ/mol)−(2 mol×( −296.9 kJ/mol)+1 mol×0.0 kJ/mol)=−196.6 kJ$

Thus, the standard enthalpy change for the given reaction is $−196.6 kJ$ .

Now, calculate the standard entropy change for the given reaction.

The balanced chemical reaction is,
$2SO2(g)+O2(g)→2SO3(g)$

The standard entropy change of the reaction is calculated by the formula,
$ΔS0=∑nΔS0( products)−∑mΔS0( reactants)=2ΔS SO3(g)0−(2ΔS SO 2 ( g )0+ΔS O 2 ( g )0)$

Substitute the standard values of $ΔSSO2(g)0$ , $ΔSO2(g)0$ and $ΔSSO3(g)0$ from appendix C in the above equation.
$ΔS0=2×256.2 J/mol⋅K−(2 mol×248.5 J/mol⋅K+1 mol×205.0 J/mol⋅K)=−189.6 J/K$

Thus, the standard entropy change for the given reaction is $−189.6 J/K$ .

Conclusion:

The standard enthalpy change for the given reaction is $−196.6 kJ$ and the standard entropy change for the reaction is $189.6 J/K$ .

(b)

Interpretation Introduction

To determine: The standard free energy change for the given reaction.

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