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wariber [46]
3 years ago
8

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
Chemistry
1 answer:
BaLLatris [955]3 years ago
3 0
Answer is: -267 kJ/mol.
Chemical reaction: Ag₂O(s) + H₂S(g) → Ag₂S(s) + H₂O<span>(l).
</span>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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