At a constant external pressure of 43.6 bar , a mole of X reacts via the reaction

X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ mol−1

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, ΔU , in kJ mol−1

Question

At a constant external pressure of 43.6  bar , a mole of  X  reacts via the reaction

X(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJ mol−1

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,  ΔU , in   kJ mol−1

Narad · Answer

$$\Delta U=\Delta H-P \Delta V$$