Assuming constant pressure, rank these reactions from most energy released by the system to most energy absorbed by the system, based on the following descriptions:

Surroundings get colder and the system decreases in volume.

Surroundings get hotter and the system expands in volume.

Surroundings get hotter and the system decreases in volume.

Surroundings get hotter and the system does not change in volume.

Also assume that the magnitude of the volume and temperature changes are similar among the reactions.

Rank from most energy released to most energy absorbed. To rank items as equivalent, overlap them.

Part B

A mole of X reacts at a constant pressure of 43.0 atm via the reaction

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.

Express your answer with the appropriate units.