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A cylinder with a piston holds 3.50 moles of a diatomic gas. The gas in the cylinder absorbs 875 J of energy due to the higher temperature of the environment. At the same time, the cylinder expands to a larger volume, doing 112 J of work on the environment. (a) What is the change in internal energy of the gas in the cylinder (in J)

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The change in the internal energy of the gas in the cylinder is 763 J

From the first law of thermodynamics, the change in internal energy(U) of a system is equivalent to the difference between net heat transfer(Q) into the system and the net work done(W) on the system

The equation for the change in the internal energy from the first law of thermodynamics is:

ΔU = ΔQ - ΔW

ΔU = 875 J - 112 J

ΔU = 763 J

Learn more about the first law of thermodynamics here:

https://brainly.com/question/9614649

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