Calculate the standard enthalpy of formation of CH3OH(l) from the following data: CH3OH (l) + 3/2 O2(g) → CO2(g) + 2H2O(l) ; ∆rH = –726 kJ mol–1 C(graphite) + O2(g) → CO2(g) ; ∆cH = –393 kJ mol–1 H2(g) + 1/2 O2(g) → H2O(l); ∆f H = –286 kJ mol–1.

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TextHess's Law of Constant Heat Summation

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Enthalpies of formation of CO(g), CO2(g), N2O(g) and N2O4(g) are –110, – 393, 81 and 9.7 kJ mol–1 respectively. Find the value of ∆rH for the reaction: N2O4(g) + 3CO(g) → N2O(g) + 3CO2(g)

TextHess's Law of Constant Heat Summation

(a) Use the information in the table to calculate the enthalpy of this reaction C2H6(g) + 7/2 O2(g) → 2CO2(g) + 3H2O(l) Reactions and ΔHf° kJ/mol: 2C(s) + 3H2(g) → C2H6(g): -84.7 C(s) + O2(g) → CO2(g): -393.5 H2(g) + 1/2 O2(g) → H2O(l): -285.8 (b) Will the heat released in the following two reactions be equal? Give reasons in support of your answer. H2(g) + 1/2 O2(g) → H2O(g) H2(g) + 1/2 O2(g) → H2O(l)

TextEnthalpy of Combustion, Formation and Atomization