# Thermodynamics debacle

1. Dec 3, 2006

### a_lawson_2k

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

Quantity of SO2 occupies volume of 5E-3 m^3 at pressure of 1,1E5 Pa. The gas expands adiabatically to volume of 1E-2 m^3 doing 285J worth of work on its surroundings. Assume the gas may be treated as ideal.
A) Find final pressure of the gas if $$\gamma$$=1,29
B) How much work does the gas do on its surroundings?
C) What is the final ratio of the gas to its initial temperature?

2. Relevant equations

$$W=\frac {{\it P_1 V_1}-{\it P_2 V_2}}{\gamma-1}$$

3. The attempt at a solution

I plugged in gamma, P1, V1 and V2, and got 4,67E4 Pa. The book says 4,50E4 Pa. Not sure how they got this.

The second part puzzles me, didn't they just tell me that the gas did 285J worth of work on its surroundings? (book says 345J)

I'm not even going to touch C until I get these out of the way.

2. Dec 3, 2006

### Andrew Mason

Your equation is not correct. If the adiabatic expansion is reversible (constant equilibrium during expansion), the adiabatic condition applies and W will be:

$$W = \frac{P_1V_1^\gamma(V_2^{1-\gamma}-V1^{1-\gamma})}{1-\gamma}$$

Try that and see if you get their answer. Ignore the 285J. It is an error if the expansion is reversible. If it is not reversible, the question makes no sense.

AM

3. Dec 3, 2006

### a_lawson_2k

How does the $$P_2$$ come into play in that case?

EDIT: used the wrong equation in this case, $$p_1 V_1^\gamma=p_2 V_2^\gamma$$ works.

Last edited: Dec 3, 2006