Sulfur reacts with oxygen to form sulfur dioxide SO sub 2 times g , Δ⁢H_f=−296.8kJ/mol ) according to the equation. cap s times s plus cap o sub 2 times g rightarrow SO sub 2 times g What is the enthalpy change for the reaction? Use Δ⁢H_rxn=∑(Δ⁢H_f_1p⁢r⁢o⁢d⁢u⁢c⁢t⁢s)−∑(Δ⁢H_f_1r⁢e⁢a⁢c⁢tan⁡t⁢s)

Use ΔH_rxn = ΣΔH_f(products) − ΣΔH_f(reactants). SO₂(g) has ΔH_f = −296.8 kJ/mol, while S(s) and O₂(g) are elements in their standard states, so each has ΔH_f = 0. Thus ΔH_rxn = −296.8 − (0 + 0) = −296.8 kJ, matching the choice “negative 296.8 kJ.”

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