Posted by **mary** on Monday, February 15, 2010 at 9:42pm.

One mole of an ideal monatomic gas initially at 300 K is expanded from an initial pressure of

10 atm to a final pressure of 1 atm. Calculate ��E, q, w, ��H, and the final temperature T2 for

this expansion carried out according to each of the following paths. The molar heat capacity

at constant volume for a monatomic gas is CV = 3/2 nR. Taken from Tinoco 2.8.

(a) An isothermal, reversible expansion.

(b) An expansion against a constant external pressure of 1 atm in a thermally isolated

(adiabatic) system.

Hint for part b: The transition is not isothermal. Be patient and write down everything you

know. You will find that ��E = -1.35 x 103 J.

(c) An expansion against zero external pressure (against a vacuum) in an adiabatic system.

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