Acetylene (C₂H₂)undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water.Given $\Delta$H°_f[CO₂(g)] = -393.5 kJ/mol, $\Delta$H°_f[H₂O(g)] = -241.8 kJ/mol, and $\Delta$H°_f[C₂H₂(g)] = 226.6 kJ/mol, how much energy is released (kJ)when 10.5 moles of acetylene is burned? A)2,510.8 kJ B)26,400 kJ C)13,200 kJ D)52,700 kJ E)9,050 kJ

Question

Quizplus · Accepted Answer

The balanced combustion reaction is: 2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O. The enthalpy change for the reaction is calculated using ΔH = ΣΔH°f(products) - ΣΔH°f(reactants). For 1 mole of C₂H₂: ΔH = [4(-393.5) + 2(-241.8)] - [2(226.6)] = -2598.8 kJ. For 10.5 moles: 10.5 * (-1299.4) = -13,200 kJ.

Acetylene (C2H2)undergoes Combustion in Excess Oxygen to Generate Gaseous Carbon Δ\DeltaΔ

Acetylene (C₂H₂)undergoes Combustion in Excess Oxygen to Generate Gaseous Carbon $\Delta$