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podryga [215]
3 years ago
11

A cylinder-piston system contains an ideal gas at a pressure of 1.2 x 10° Pa.

Physics
1 answer:
MAVERICK [17]3 years ago
4 0

The change in internal energy of the gas is -9 J

Explanation:

First of all, we need to calculate the amount of work done by the gas. This is given by the equation:

W=p(V_f - V_i)

where

p=1.2\cdot 10^5 Pa is the gas pressure

V_f = 0.0003 m^3 is the final volume of the gas

V_i = 0.0006 m^3 is the initial volume of the gas

Substituting, we find:

W=(1.2\cdot 10^5)(0.0003-0.0006)=-36 J

Now we can apply the 1st law of thermodynamics to calculate the change in internal energy of the gas:

\Delta U = Q - W

where

\Delta U is the change in internal energy of the gas

Q = -45 J is the heat released by the gas (negative because it is given off bu the system)

W = -36 J is the work done by the gas (negative because it is done by the surrounding on the gas)

Substituting, we find:

\Delta U = -45 - (-36) = -9 J

Learn more about ideal gases:

brainly.com/question/9321544

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brainly.com/question/3658563

#LearnwithBrainly

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