Problem: Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g):2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJΔH°f (kJ/mol)SO2(g) -297

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We’re being asked to determine the standard enthalpy change of formation (ΔH˚f) for SO3(g). Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved


H°rxn = H°f, products - H°f, reactants


We’re given the ΔH˚rxn for the combustion of 2 moles of SO2. The balanced chemical equation for that reaction is:

2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ



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Problem Details

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g):
2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ
ΔH°f (kJ/mol)
SO2(g) -297

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