1. Dec 1, 2006

### mikefitz

1. The problem statement, all variables and given/known data
A monatomic, ideal gas is in a sealed container (the number of gas molecules is always constant: n = 2 moles); the initial pressure is Pi = 1.01 x 10^5 Pa and the initial volume is Vi = 0.0224 m^3.

* First, the volume of the gas is decreased at a constant pressure (at Pi = 1.01 x 10^5 Pa) to a final volume of Vf = 0.0155 m^3.
* Second, the pressure of the gas is increased at a constant volume (at Vf = 0.0155 m3) to a final pressure of Pf = 1.35 x 10^5 Pa.

How much heat was added to (give as a positive number) or removed from (give as a negative number) the system? (The gas constant R = 8.31 J/mole-K.)

2. Relevant equations
PV = nRT

3. The attempt at a solution

I guess I am confused as to how I am supposed to solve this problem without knowing the heat capacity or the specific heat of the substance.

I have calculated Ti=94.14 and Tf=125.83 - deltaT=31.692 C - why is this incorrect?

2. Dec 1, 2006

The heat capacity at constant volume of an ideal gas is: $$c_{v}NR$$.

$$c_{v} = \frac{3}{2}$$ for a monatomic gas, and $$\frac{5}{2}$$ for a diatomic gas.

The heat capacity at constant pressure of an ideal gas is:

$$(c_{v}+1})NR$$

3. Dec 3, 2006

### mikefitz

Problem Solved.

Please look at case one of the pressure vs volume graph:

http://img99.imageshack.us/img99/2964/followuphz6.gif [Broken]

I thought to get the total work done by the system I would take the work done by decreasing volume and add the work done by increasing pressure.

To get the total work done all I had to do was use the work done by the system decreasing volume. (-696.9J)

Why didn't I have to add on the work done by the increase in pressure? I calculated that to be 527J, where does this energy disappear to?

thanks

Last edited by a moderator: May 2, 2017
4. Dec 3, 2006

$$W = P\Delta V$$
$$W = \int_{V_{1}}^{V_{2}} P\; dV$$