1. The problem statement, all variables and given/known data Two identical samples of ideal gas are initially at P1 and V1. The first sample undergoes an isothermal transformation to P2, V2 and second sample undergoes an adiabatic transformation to P3, V2. If P3<P2, is V2 higher or lower than V1? Explain 2. Relevant equations Ideal Gas Law, Thermo Laws. 3. The attempt at a solution P1V1 --isotherm-->P2V2 P1V1 --adiabatic-->P3V2 If P2>P3, is V2>V1 or V2<V1? __ For isotherm we have ΔU=Q+W, but since there is ΔT=0, then via 1st law of Thermo - ΔU=0 and Q=-W. For adiabatic we have constant heat, Q=0, W=PΔV, ΔU=W=PΔV. Yet... it seems useless. My gut tells me V2>V1, though somehow I am having trouble wrapping my mind around it.