A 0.300-kg sample of nitrogen gas (diatomic molecules,mN2 = 4.652 × 10^−26 kg) in a chamber fitted with a piston undergoes an isothermal expansion from 0.0500 m^3 to 0.150 m^3 .
If the final pressure is 110 kPa, what is the final temperature?
PV=N*kB*T where Boltzmann's Constant is kB=1.38*10^-23 J/K
The Attempt at a Solution
Because the process is isothermal, PV = constant and Ti = Tf.
To use the formula, I need N (number of molecules).
Plugging this N into T=PV/NkB I get, T = 92.7 K, which is not the right answer.
I don't think diatomic gasses behave ideally, but I have no idea how to reflect that in the formula. I also do not know how the initial volume and pressures are relevant.