Answer:
-80 J
Explanation:
The first law of thermodynamics states that:
[tex]\Delta U = Q - W[/tex]
where
[tex]\Delta U[/tex] is the change in internal energy of the system
Q is the heat absorbed by the system
W is the work done by the system
In this problem, we have:
Q = -30 J is the heat released by the system (negative because the system releases it)
W = +50 J is the work done by the system on the surrounding (positive since it is done by the system)
Therefore, the change in internal energy is
[tex]\Delta U = -30 J - (+50 J) = -80 J[/tex]
