1. The problem statement, all variables and given/known data A sphere full of air at room temp and 1 atm is placed in a chamber filled with He gas at room temp and 1 atm. The sphere is permeable to He only. What will the equilibrium pressure in the sphere be? 2. Relevant equations Variables: Po=initial pressure V=vol of sphere V'=vol of chamber Na=number of air particles Nh=number of He particles Ideal gas law: P=NRT/V --------- I think that's all i need, but other eqs that might be relevant: S=ln(Q) : entropy=ln(number of states) dS/dE=1/T : derivative of entropy wrt Energy = 1/temp 3. The attempt at a solution Here's what I think: since He is a noble gas, we can assume it does not interact with the air particles. Therefore, at equilibrium, a single He molecule is equally likely to be found anywhere in the chamber (V'), which means that the mean number of He particles in the sphere (V) will be V/V'*Nh. Then use the ideal gas law: P=(V/V'*Nh+Na)RT/V can also solve for Nh and Na initially in terms of Po, R, T and V or V': Nh=PoV'/(RT), Na=PoV/(RT) and then plug in, rearrange and reduce: P=(Po/(RT))(V/V'*V'/V+V/V)*RT=Po(1+1)=2Po=2 atm So, is there anything wrong with what I did? I don't know what the answer should be, but I'm not confident in my answer because my prof mentioned that we should start by maximizing entropy.... which I could do, but this way seemed so much simpler. Suggestions? Any errors in my assumptions or approach? I don't find this material intuitive, so I could very well have made mistakes. Thanks!