A steel rigid vessel of volume 2 L is filled with a mixture of methane and oxygen at a total pressure of 1.5 atm at 127°C. The gas mixture is exploded. What would be the final pressure of the products

Question

A steel rigid vessel of volume 2 L is filled with a mixture of methane and oxygen at a total pressure of 1.5 atm at 127°C. The gas mixture is exploded. What would be the final pressure of the products at 327°C? (Assume water remains entirely vapour at 327°C.)

TestHub · Accepted Answer

CH₄ + 2O₂ → CO₂ + 2H₂O(g): 3 mol reactants give 3 mol gaseous products, so total moles are unchanged by the explosion. In the rigid vessel P ∝ T: P₂ = 1.5 × 600/400 = 2.25 atm. Confirms Ans: (b) 2.25 atm.

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