A steel rigid vessel of volume 1 l is filled with a mixture of methane and oxygen at a total pressure of one atm at 27°C. The gas mixture is exploded. What would be the final pressure of the products

Question

A steel rigid vessel of volume 1 l is filled with a mixture of methane and oxygen at a total pressure of one atm at 27°C. The gas mixture is exploded. What would be the final pressure of the products at 127°C? Aqueous tension at 27°C = 0.04 atm.

TestHub · Accepted Answer

CH 4 + 2O 2 → CO 2 + 2H 2 O. At 127°C (> 100°C) water is entirely vapour, so 3 mol reactants give 3 mol gas products per mole of CH 4 burned: total moles of gas are unchanged by the explosion at any mixture ratio. In the rigid vessel P ∝ T: P 2 = 1 atm × 400/300 = 1.33 atm. (Aqueous tension is irrelevant at 127°C.) Confirms Ans: (b) 1.33 atm.

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