(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

Fivemoles of an ideal monotomic gas initially occupies a volume of 100 x 10^{-3}m^{3}at a temperature of 280 K. (state 1)

The gas is then subject to the following processes in sequence:

* heated at constant volume to a temperature of 600K (state 2)

* allowed to expand isothermally to its initial pressure (state 3)

* compressed isobarically to its original volume (state 1)

(a) Find the pressure and volume of the gas in state 3

(b) Calculate the work done on the gas in going from state2 to state 3.

(c) Calculate the heat exchanged between the gas and its environment during each of the 3 processes of the cycle 1->2, 2->3, 3->1.

In each case, indicate whether the heat enters or leaves the gas.

(d) Calculate the net work done on the gas in one cycle

2. Relevant equations

PV=nRT=Nk_{B}T

pV^{r}=constant,r=C_{p}/C_{v}

dW=-PdV

W=nRT*ln(V_{i}/V_{f})

E_{int}=3/2Nk_{b}T

C_{v}=5/2R

3. The attempt at a solution

I'm stuck on question (a).

I calculated the pressure using PV=nRT where the initial volume, temperature and number of moles of gas is provided. P=(5*8.314*280)/(100x10^{-3})

Now, I dont know how to calculate the volume in state 3. Do I use T=600K and P=the above I calculated, to obtain the volume?

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# Thermodynamics problem Help!

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