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

Question

Andrej [43]

3 years ago

15

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.

Chemistry

1 answer:

vlabodo [156] · Answer 1 · 2022-08-21T20:46:09+03:00

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.