1. The problem statement, all variables and given/known data 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? 2. Relevant equations PV=N*kB*T where Boltzmann's Constant is kB=1.38*10^-23 J/K 3. 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). 0.300/[(4.652*10^-26)(0.5)]=1.29*10^25 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.