How much heat is involved in the complete combustion of 2.50 kg propane,C₃H₈?
Δ_rH_comb = -2219 kJ/mol

Question

How much heat is involved in the complete combustion of 2.50 kg propane,C₃H₈? Δ_rH_comb = -2219 kJ/mol

Quizplus · Accepted Answer

The complete combustion of propane can be represented by the equation: C3H8 + 5O2 → 3CO2 + 4H2O. The given ΔHcomb is -2219 kJ/mol, which is the amount of heat released when 1 mole of propane combusts completely. The molar mass of propane (C3H8) is approximately 44.1 g/mol. To find the total heat involved in the combustion of 2.50 kg of propane, first convert the mass of propane to moles: 2500 g / 44.1 g/mol ≈ 56.69 mol. Then, multiply the moles of propane by the heat released per mole: 56.69 mol × (-2219 kJ/mol) ≈ -1.26 × 10^5 kJ.

How Much Heat Is Involved in the Complete Combustion of 2.50