Question
A system receives 425 J of heat from the surroundings and
delivers 420 J of work to its surroundings. What is the change in
the internal energy?
delivers 420 J of work to its surroundings. What is the change in
the internal energy?
Answers
Answered by
GPT 3.5
To find the change in internal energy, we need to use the first law of thermodynamics:
ΔU = Q - W
Where:
ΔU = Change in internal energy
Q = Heat absorbed by the system
W = Work done by the system
Given:
Q = 425 J (heat received from the surroundings)
W = -420 J (work done to the surroundings, negative because work done by the system is considered positive)
ΔU = 425 J - (-420 J)
ΔU = 425 J + 420 J
ΔU = 845 J
The change in internal energy is 845 J.
ΔU = Q - W
Where:
ΔU = Change in internal energy
Q = Heat absorbed by the system
W = Work done by the system
Given:
Q = 425 J (heat received from the surroundings)
W = -420 J (work done to the surroundings, negative because work done by the system is considered positive)
ΔU = 425 J - (-420 J)
ΔU = 425 J + 420 J
ΔU = 845 J
The change in internal energy is 845 J.