1. The problem statement, all variables and given/known data A monatomic, ideal gas is in a sealed container (the number of gas molecules is always constant: n = 2 moles); the initial pressure is Pi = 1.01 x 10^5 Pa and the initial volume is Vi = 0.0224 m^3. * First, the volume of the gas is decreased at a constant pressure (at Pi = 1.01 x 10^5 Pa) to a final volume of Vf = 0.0155 m^3. * Second, the pressure of the gas is increased at a constant volume (at Vf = 0.0155 m3) to a final pressure of Pf = 1.35 x 10^5 Pa. How much heat was added to (give as a positive number) or removed from (give as a negative number) the system? (The gas constant R = 8.31 J/mole-K.) 2. Relevant equations PV = nRT 3. The attempt at a solution I guess I am confused as to how I am supposed to solve this problem without knowing the heat capacity or the specific heat of the substance. I have calculated Ti=94.14 and Tf=125.83 - deltaT=31.692 C - why is this incorrect?