Given the following $\Delta$H° values, H₂(g)+ O₂(g)$\rarr$ H₂O(l)$\Delta$H°_f = -285.8 kJ/mol H₂O₂(l)$\rarr$ H₂(g)+ O₂(g)$\Delta$H°_rxn = 187.6 kJ/mol calculate $\Delta$H°_rxn for the reaction H₂O₂(l)$\rarr$H₂O(l)+ O₂(g),

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The Answer of Given the following $\Delta$H° values, H₂(g)+ O₂(g)$\rarr$ H₂O(l)$\Delta$H°_f = -285.8 kJ/mol H₂O₂(l)$\rarr$ H₂(g)+ O₂(g)$\Delta$H°_rxn = 187.6 kJ/mol calculate $\Delta$H°_rxn for the reaction H₂O₂(l)$\rarr$H₂O(l)+ O₂(g),

Given the Following Δ\DeltaΔ H° Values, H2(g)+ O2(g) →\rarr→ H2O(l) Δ\DeltaΔ H°f = -285

Given the Following $\Delta$ H° Values,
H₂(g)+ O₂(g) $\rarr$ H₂O(l) $\Delta$ H°_f = -285