Answer:
Q = - 730 KJ
730 KJ is transferred out of the system
Explanation:
According to the first law of thermodynamics, energy can neither be created nor destroyed, but can be transformed from one form to another.
For a particular process/system, the first law is interpreted as
ΔU = Q + W (depending on convention, some textbooks give this relation as ΔU = Q - W)
ΔU is the change in internal energy of the system, in my convention, it is positive if the internal energy increases and negative otherwise.
Q = Heat transferred into or out of the system. Q is positive for heat transferred into the system and negative for heat transferred out of the system.
W = workdone by the system or work done on the system. W is positive for workdone on the system and W is negative for when work is done by the system.
ΔU decreases by 250 KJ, that is, ΔU = - 250 KJ
Q = ?
W = 480 KJ (Work is done on the system)
- 250 = Q + 480
Q = - 250 - 480 = - 730 KJ
The heat is transferred out of the system.
