913

Volume: $\Delta S = nR\ln \frac{V_{2}}{V_{1}}$
Temperature: $\Delta S = nC\ln \frac{T_{2}}{T_{1}}$

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Hyein Cha 2I
Posts: 103
Joined: Fri Sep 29, 2017 7:05 am
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913

the question says "During the test of an internal combustion engine, 3.00L of nitrogen gas at 18.5 degrees C was compressed suddenly (and irreversibly) to .500L by driving in a piston. In the process the temperature of the gas increased to 28.1 degrees C. Assume ideal behavior. What is the change in entropy of the gas?"

I know how to solve the problem, but I didn't get why the solutions manual assumed that it was 1 mol of gas. How do you figure out the moles of gas when it's not given?

sahiltelang-Discussion 1J
Posts: 50
Joined: Thu Jul 13, 2017 3:00 am

Re: 913

Since it states assume ideal behavior, we can assume that it is 1 mol of gas within the combustion engine

Meredith Steinberg 2E
Posts: 50
Joined: Thu Jul 13, 2017 3:00 am

Re: 913

Ideal gas behavior assumes that the ideal gas has a quantity of 1 mol.

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