(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)

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TextEnthalpy of Combustion, Formation and AtomizationHess's Law of Constant Heat Summation

Similar Questions

The combustion of one mole of benzene takes place at 298 K and 1 atm. After combustion, CO2(g) and H2O (1) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation, ∆f H of benzene. Standard enthalpies of formation of CO2(g) and H2O(l) are –393.5 kJ mol–1 and – 285.83 kJ mol–1 respectively.

TextEnthalpy of Combustion, Formation and Atomization

The enthalpies of all elements in their standard states are:

MCQ (Single)Enthalpy of Combustion, Formation and Atomization