Compute ΔH°rxn for the following reaction. The value of ΔH°f in kJ/mol is given below each species:
2 CaO(s) + 2 SO₂(g) + O₂(g) → 2 CaSO₄(s)
-635.5 -296.9 0.0 -1432.7

Question

Compute ΔH°rxn for the following reaction. The value of ΔH°f in kJ/mol is given below each species: 2 CaO(s) + 2 SO₂(g) + O₂(g) → 2 CaSO₄(s) -635.5 -296.9 0.0 -1432.7

Quizplus · Accepted Answer

The correct answer is A.The enthalpy change of a reaction is equal to the difference between the enthalpy of the products and the enthalpy of the reactants. In this case, the enthalpy of the products is -1432.7 kJ/mol and the enthalpy of the reactants is -635.5 kJ/mol - 296.9 kJ/mol + 0.0 kJ/mol = -932.4 kJ/mol. Therefore, the enthalpy change of the reaction is -1432.7 kJ/mol - (-932.4 kJ/mol) = -1000.6 kJ/mol.

Compute ΔH°rxn for the Following Reaction