(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

A compressed cylinder holds nitrogen gas at room temperature. How cold is the gas that is escaping from the cylinder?

T(cylinder) = 298 K

P(cylinder) = 1.034e7 Pa

n = 1

2. Relevant equations

PV = nRT

3. The attempt at a solution

So since I was not given either the volume of the container or its final volume, I assumed that the initial and final volumes were approximately the same. This may be a fatal flaw to my line of reasoning.

Assuming the above is correct, I said:

P/V = constant , and therefore:

P1/T1 = P2/T2 , where P1 and T1 are the pressure and temperature in the cylinder.

I am not sure if I need the adiabatic exponent of f+2/2 in there somewhere or not. Also, I used P2 = 101.3 kPa and yes I put that into Pa before doing the algebra.

Without the adiabatic exponent, I went through the algebra and found the temperature of the escaping gas is 2.94 K. This to me doesn't seem like a reasonable answer since that is really cold. However, I do not have a good understanding of what is reasonable since I do not know much about gas temperatures.

Any comments on whether or not this is correct or flawed would be greatly appreciated.

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# Ideal gas compression

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