Find $\Delta$H^$\circ$_rxn for the reaction 2Ag₂S(s) + 2H₂O(l) $\rarr$ 4Ag(s) + 2H₂S(g) + O₂(g).[$\Delta$H^$\circ$_f (Ag₂S(s)) = -32.6 kJ/mol; $\Delta$H^$\circ$_f (H₂S(g)) = -20.5 kJ/mol; $\Delta$H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol] A) 595.2 kJ/mol B) 585.2 kJ/mol C) 575.2 kJ/mol D) 565.2 kJ/mol E) None of the above

Question

Quizplus · Accepted Answer

To find $\Delta$H^$\circ$_rxn, use the formula: $\Delta$H^$\circ$_rxn = $\sum\Delta$H^$\circ$_f (products) - $\sum\Delta$H^$\circ$_f (reactants). For the given reaction: $\Delta$H^$\circ$_rxn = [4(0) + 2(-20.5) + 0] - [2(-32.6) + 2(-285.5)] = 595.2 kJ/mol.

Find Δ\DeltaΔ H ∘\circ∘ rxn for the Reaction 2Ag2S(s) + 2H2O(l) →\rarr→

Find $\Delta$ H^$\circ$_rxn for the Reaction
2Ag₂S(s) + 2H₂O(l) $\rarr$