Given H₂(g) + (1/2)O₂(g) $\rarr$ H₂O(l), $\Delta$H^$\circ$ = -286 kJ/mol, determine the standard enthalpy change for the reaction 2H₂O(l) $\rarr$ 2H₂(g) + O₂(g). A)($\Delta$H^$\circ$) = -286 kJ/mol B)($\Delta$H^$\circ$) = +286 kJ/mol C)($\Delta$H^$\circ$) = -572 kJ/mol D)($\Delta$H^$\circ$) = +572 kJ/mol E)($\Delta$H^$\circ$) = -143 kJ/mol

Question

Quizplus · Accepted Answer

The reverse reaction of forming water from hydrogen and oxygen has the opposite sign for enthalpy change. Since the reaction is doubled, the enthalpy change is also doubled, resulting in +572 kJ/mol.

Given H2(g) + (1/2)O2(g) →\rarr→ H2O(l) Δ\DeltaΔ H ∘\circ∘ = -286 KJ/mol, Determine the Standard Enthalpy Change for =

Given H₂(g) + (1/2)O₂(g) $\rarr$ H₂O(l) $\Delta$ H^$\circ$ = -286 KJ/mol, Determine the Standard Enthalpy Change for =