The first law of thermodynamics states that the change in internal energy of a system equals the heat added to the system minus the work done by the system:
ΔU = Q - W
where:
ΔU = change in internal energy
Q = heat added to the system
W = work done by the system
In this case, we have:
ΔU = 80 J
W = -50 J (since work is being done on the system by the surroundings, the sign is negative)
So, we can rearrange the equation to solve for Q:
Q = ΔU + W
Q = 80 J + (-50 J)
Q = 30 J
Therefore, the heat change of the system is 30 J.
A system with an increase in internal energy of 80 J and at the same time has 50 J of work done on it by the surrounding. What is the heat change of the system?
1 answer