X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules.

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11-10-2016
Chemistry

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X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules.

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Hussain514 Hussain514 · Answer 1 · 2016-10-16T13:55:29+02:00

Isobaric transition, first law: H=ΔU+w for a gas expansion: w=Pext∗ΔV to convert to joules, you need the gas constants. R = 0.08206 L atm/mol*K, R=8.314 J/mol*K w=Pext∗ΔV∗8.314 J/mol∗K0.08206 L atm/mol∗K ΔU=ΔH−[Pext∗ΔV∗8.314 J/mol∗K0.08206 L atm/mol∗K] ΔU=−75000 J−[(43.0atm)∗(2−5)L∗8.314 J0.08206 L atm] Then you need to convert to kJ. by the way U=E, internal energy.