1. Sep 4, 2010

### marissy

1. The problem statement, all variables and given/known data
Hello,

I have been stuck on this problem for about an hour so any hep would be greatly appreciated!

One mole of argon at 25 degrees C and 1 atm pressure is allowed to expand reversibly t a volume of 50 L (a) isothermally (b) adiabatically. Calculate the final pressure in each case assuming ideal gas behavior.
The answers have been given and they are: (a) 0.489 atm and (b) 0.303 atm

I can't get either a or b for some reason I don't know what I am doing wrong! Please help me :(

2. Relevant equations
Cv = 3/2 R Cp= 5/2 R
Boyle's law

3. The attempt at a solution

my answers dont even come close...?

2. Sep 4, 2010

### D H

Staff Emeritus

Show some work please. It's impossible to show you where you went wrong if you don't show us what you have done.

3. Sep 4, 2010

### marissy

nevermind i got it all -- I just didnt have my P and V in the right units.... anyway i found V1 using the ideal gas law, and the used boyle's law to find P2. Seems so simple when you have the correct units :)

for part b i did PV(5/3)=nRT to find V1 and then used boyle's law to find P2. I got 0.296 for the answer tough. maybe my sig. figs. are off? i can't find out why.

4. Sep 4, 2010

### Andrew Mason

You will have to use the adiabatic condition:

$$PV^\gamma = \text{constant} \ne nRT$$

for part b). $PV^1 = nRT$

AM

5. Sep 5, 2010