Find the standard enthalpy of formation of ethylene, C₂H₄(g), given the following data: heat of combustion of C₂H₄(g)= -1411 kJ/mol; $\Delta$H°_f[CO₂(g)] = -393.5 kJ/mol; $\Delta$H°_f[H₂O(l)] = -285.8 kJ/mol. A)52 kJ/mol B)87 kJ/mol C)731 kJ/mol D)1.41 × 10³ kJ/mol E)2.77 × 10³ kJ/mol

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The standard enthalpy of formation of ethylene can be calculated using the combustion reaction: C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(l). Using Hess's law: ΔH° = [2(-393.5) + 2(-285.8)] - (-1411) = 52 kJ/mol.

Find the Standard Enthalpy of Formation of Ethylene, C2H4(g), Given Δ\DeltaΔ

Find the Standard Enthalpy of Formation of Ethylene, C₂H₄(g), Given $\Delta$