Question

What is the change in internal energy (deltaE ) of a system when it loses 76.0 J of heat while the surroundings perform 29.0 J of work

Answer 1

Answer:

-47 J

Explanation:

Given that,

Heat loss = -76 J (negative for loss)

Work done by the surroundings = -29 J

We need to find the change in internal energy of a system.

The first law of thermodynamics is given by :

$\Delta U=Q-W$

W is work done by the system

Putting all the values,

$\Delta U=(-76)-(-29)\\\\=-47\ J$

Hence, the change in internal energy is -47 J.