Given the following $\Delta$H^$\circ$ values, H₂(g) + (1/2)O₂(g) $\rarr$ H₂O(l) $\Delta$H^$\circ$_f = -285.8 kJ/mol H₂O₂(l) $\rarr$ H₂(g) + O₂(g) $\Delta$H^$\circ$_rxn = 187.6 kJ/mol Calculate $\Delta$H ^$\circ$_rxn for the reaction H₂O₂(l) $\rarr$ H₂O(l) + (1/2)O₂(g). A) -98.2 kJ/mol B) -88.2 kJ/mol C) -78.2 kJ/mol D) -68.2 kJ/mol E) None of the above

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The Answer of Given the following $\Delta$H^$\circ$ values, H₂(g) + (1/2)O₂(g) $\rarr$ H₂O(l) $\Delta$H^$\circ$_f = -285.8 kJ/mol H₂O₂(l) $\rarr$ H₂(g) + O₂(g) $\Delta$H^$\circ$_rxn = 187.6 kJ/mol Calculate $\Delta$H ^$\circ$_rxn for the reaction H₂O₂(l) $\rarr$ H₂O(l) + (1/2)O₂(g). A) -98.2 kJ/mol B) -88.2 kJ/mol C) -78.2 kJ/mol D) -68.2 kJ/mol E) None of the above

Given the Following Δ\DeltaΔ H ∘\circ∘ Values, H2(g) + (1/2)O2(g) →\rarr→ H2O(l) Δ\DeltaΔ

Given the Following $\Delta$ H^$\circ$ Values, H₂(g) + (1/2)O₂(g) $\rarr$ H₂O(l) $\Delta$