1 mole of ideal gas initially at 294 K is compressed adiabatically and
reversibly from 0.83 atm to 10.0 atm. Calculate the initial and …final volumes,
the final temperature, [itex]\Delta[/itex]U; [itex]\Delta[/itex]H; Q; and W: Assume that Cv = (5/2)R
n = 1 mol
T1 = 294 K
P1 = 0.83 atm
P2 = 10 atm
Q = 0
V1, V2, [itex]\Delta[/itex]U, Q, [itex]\Delta[/itex]H, T2, W
1. The professor gave that specific heat at constant volume is (5/2)R, however, the volume of the problem changes. Is this equation completely irrelevant to the problem?
2. How to you find the final temperature and final volume?
The Attempt at a Solution
I started off with PV = nRT for the initial givens and obtained that V1 = 29.1 L
Now, I'm stuck. I've tried using the ideal gas equation again, but I have 2 unknowns. I tried rearranging the equation and setting it equal the initial equations. I know how to find the other unknowns, but I'm stuck at this part for some reason.