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3 years ago

7

If 500 cal of heat are added to a gas, and the gas expands doing 500 J of work on its surroundings, what is the change in the in

ternal energy of the gas?

1 answer:

poizon [28]3 years ago

6 0

Answer:

The change in the internal energy of the gas 1,595 J

Explanation:

The first law of thermodynamics establishes that in an isolated system energy is neither created nor destroyed, but undergoes transformations; If mechanical work is applied to a system, its internal energy varies; If the system is not isolated, part of the energy is transformed into heat that can leave or enter the system; and finally an isolated system is an adiabatic system (heat can neither enter nor exit, so no heat transfer takes place.)

This is summarized in the expression:

ΔU= Q - W

where the heat absorbed and the work done by the system on the environment are considered positive.

Taking these considerations into account, in this case:

Q= 500 cal= 2,092 J (being 1 cal=4.184 J)

W=500 J

Replacing:

ΔU= 2,092 J - 500 J

ΔU= 1,592 J whose closest answer is 1,595 J

<u><em>The change in the internal energy of the gas 1,595 J </em></u>

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A sample of an ideal gas is in a tank of constant volume. The sample absorbs heat energy so that its temperature changes from 33

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