Answer:
B > D > C > A
Explanation:
For the first law of the thermodynamics, the total energy variation in a process is:
ΔU = Q - W
Where Q is the heat, and W the work. If the system loses heat, Q < 0, if it absorbs heat, Q>0. If work is done in the system (volume decreases), W < 0, if the system does the work (volume increases), W > 0.
A. If the surroundings get colder, the system is absorbing heat, so Q>0, and the system decreases in volume so W < 0 :
ΔU = +Q - (-W) = +Q + W (absorbs a higher energy)
B. If the surroundings ger hotter, the system is losing heat, so Q<0, and the system expands, so W>0:
ΔU = -Q -W (loses higher energy)
C. Surroundings get hotter, Q<0, and the system decreases in volume, W<0
ΔU = - Q + W = 0 (magnitude of heat and work is similar)
D. Surroundings get hotter, Q<0, and the system is not changing in volume, W = 0.
ΔU = -Q (loses energy)
For the most released (more negative) for the most absorbed (most positive):
B > D > C > A
