Suppose 1.2 mol of a monatomic ideal gas initially at 11 L and 300 K is heated at constant volume to 590 K, allowed to expand isothermally to its initial pressure, and finally compressed at constant pressure to its original volume, pressure, and temperature. During the cycle, what are (a) the net energy entering the system (the gas) as heat and (b) the net work done by the gas? (c) What is the efficiency of the cycle? ok so heres what i got, (Ta, Va, refer to point a's temp, volume, etc) did some work and i figured these numbers out Pa= .40625atm = 41163.28 Pa Va= .0042 cubic meters Ta= 21 Kelvin Pb= 13atm = 1317225 Pa Vb= .0042 cubic meters Tb= 666 Kelvin Pc= .40625 atm = 41163.28 Pa Vc= .0336 cubic meters Tc= 166 Kelvin Now, im not sure if im using the right formulas? DeltaE (internal energy) = (3/2)nRT ? Q = nC DeltaT ? W = nC DeltaT ? I'm not sure if i wrote them wrong in my notes or something, but is this not how you get the heat, work, energy for each transition? And then, after the full cycle, DeltaE should = 0 correct? Also, i need to get this answered asap as i have a lab writeup due tomorrow... given volume, diameter of a cylinder, initial room pressure, how do you find the pressure of a gas inside said cylinder?