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3 years ago

12

A system absorbed 44 joules of heat from its surroundings. After doing work, the increase in the internal energy of the system i

s 32 joules. How much energy was used by the system to do useful work?

2 answers:

Minchanka [31]3 years ago

7 0

12 j is correct on edge

Lelu [443]3 years ago

4 0

We can solve the problem by using the first law of thermodynamics:
$\Delta U = Q-W$
where
$\Delta U$ is the variation of internal energy of the system
Q is the heat absorbed by the system
W is the work done by the system

In this problem, the heat absorbed by the system is Q=+44 J, and the increase in internal energy is $\Delta U = +32 J$ . So we can rearrange the equation to calculate the work done:
$W=Q-\Delta U=44 J-32 J=+12 J$
and the work is positive, which means that it is done by the system on the surrounding.

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