If 500 calorie of heat energy is added to a system and the system does 350 calorie of work is done on surroundings, what is the energy change of the system?
The first law of thermodynamics can be given by ΔU = q + w
When q is positive, it is the heat added to the system.
When q is negative, it is the heat taken from the system.
When w is positive, it is the work done on the system.
When w is negative, it is the work done by the system.
Where ′q′ = the heat added to the system and ′w′ = the work done on the system
Heat added to the system = 500 calorie = q
Work done by system = −350 calorie = w
Negative value of work because it is work done by the system
ΔU = q + w = 500 − 350 = 150 calories