For the reaction, 2 CO + O 2 → 2 CO 2 ; Δ H = − 560 kJ . Two moles of CO and one mole of O 2 are taken in a container of volume 1 L . They completely form two moles of CO 2 , the gases deviate

Question

For the reaction, 2 CO + O 2 ​ → 2 CO 2 ​ ; Δ H = − 560 kJ . Two moles of CO and one mole of O 2 ​ are taken in a container of volume 1 L . They completely form two moles of CO 2 ​ , the gases deviate appreciably from ideal behaviour. If the pressure in the vessel changes from 70 to 40 atm , find the magnitude (absolute value) of Δ U at 500 K . ( 1 L − atm = 0.1 kJ )

TestHub · Accepted Answer

∵ ∵ or or ​ Δ H = Δ U + Δ ( P V ) Δ H = Δ U + V Δ P Δ U = Δ H − V Δ P ​ Given that, Δ H = − 560 kJ Δ P = 40 − 70 = − 30 atm ∴ ∴ ​ ∴ V Δ P Δ U ​ V Δ P 1 L -atom = − 30 × 0.1 kJ = − 560 − ( − 30 × 0.1 ) = − 557 kJ ​ = 1 L × − 30 atm = − 30 L atom = 0.1 kJ

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