Explanation The dissociation of S O 2 ( g ) into gaseous sulfur and oxygen atoms can be represented as: S O 2 ( g ) → S ( g ) + 2 O ( g ) S t a n d a r d h e a t s o f f o r m a t i o n o f : Δ H f , O ( g ) ° = 249.2 k J / m o l ; Δ H f , S ( g , rhombic ) ° = 277.2 k J / m o l a n d Δ H f , S O 2 ( g ) ° = − 296.8 k J / m o l The enthalpy of the reaction is calculated as: Δ H r x n = ∑ Δ H f ° ( p r o d u c t s ) − ∑ Δ H f ° ( reactants ) =

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Chapter 9, Problem 125E

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To find: The average bond energy of S=O in SO2 using the standard heat of formation.

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Chapter 9, Problem 124E

Chapter 9, Problem 126E

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The average bond energy of S = O i n S O 2 using the standard heat of formation.

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To find: The average bond energy of S=O in SO2 using the standard heat of formation.

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Chapter 9 Solutions