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Given the data in the table below, δh°rxn for the reaction ag2o (s) + h2s (g) → ag2s (s) + h2o (l) is ________ kj. substance δh∘f(kj/mol) ag2o (s) -31.0 ag2s (s) -32.6 h2s (g) -20.6 h2o (l) -286

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Answer is: -267 kJ/mol.
Chemical reaction: Ag₂O(s) + H₂S(g) → Ag₂S(s) + H₂O(l).
ΔHrxn = ∑ΔH(products of reaction) - ∑ΔH(reactants).
ΔHrxn = (ΔHf(Ag₂S) + ΔHf(H₂O)) - (ΔHf(H₂S) + ΔHf(Ag₂O)).
ΔHrxn = (-32,6 kJ/mol - 286 kJ/mol) - (-20,6 kJ/mol - 31 kJ/mol).
ΔHrxn = -318,6 kJ/mol + 51,6 kJ/mol.
ΔHrxn = -267 kJ/mol.

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