One mole of methane undergoes complete combustion in a stoichiometric amount of air. The reaction proceeds as CH4 + 2O2 → CO2 + 2H2O. Both the reactants and products are in gas phase. ΔH°298 = - 730 kJ/mole of methane. Mole fraction of water vapour in the product gases is about_____________________?
Correct answer: A. 0.19
- A. 0.19
- B. 0.33
- C. 0.40
- D. 0.67
Explanation
The products contain 1 mol of CO₂, 2 mol of H₂O, and about 7.52 mol of N₂ from the stoichiometric air. Thus, yH₂O = 2/(1 + 2 + 7.52) ≈ 0.19.
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