Problem: The standard enthalpy of combustion of ethene gas, C2H4(g), is -1411.1 kJ/mol at 298 K. Given the following enthalpies of formation, calculate ΔHf° for C2H4(g).CO2 (g)          -393.5 kJ/molH2O (l)            -285.8 kJ/mol

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FREE Expert Solution

Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved

H°rxn=H°f, products-H°f, reactants



The chemical equation for that reaction is:

C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l)



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Problem Details

The standard enthalpy of combustion of ethene gas, C2H4(g), is -1411.1 kJ/mol at 298 K. Given the following enthalpies of formation, calculate ΔHf° for C2H4(g).

CO2 (g)          -393.5 kJ/mol

H2O (l)            -285.8 kJ/mol

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Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

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Based on our data, we think this problem is relevant for Professor Razunguzwa's class at GWU.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.