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## Homework Statement

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

Given:

n = 1 mol

T1 = 294 K

P1 = 0.83 atm

P2 = 10 atm

Q = 0

Find

V1, V2, [itex]\Delta[/itex]U, Q, [itex]\Delta[/itex]H, T2, W

## Homework Equations

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.