A diatomic ideal gas is in a rigid container at an initial sate of 300K and 1.3x10^5 Pa is heated to a final state of 330K by 623.25J of heat. calculate the pressure in the container after the heating, the work done by the gas, the change in internal energy and the volume of the container. if the same gas is now continued in another cylinder and is compressed with a different compression process from the same initial to final states as above, calculate the change of the internal energy. The universal gas constant is given as 8.31. I 've managed to do the first three parts of the question but i'm curently stuck at finding the volume. I've tried using pV=nRT but it doesn't work since i do not know the number of moles of gas present. Aside from finding the volume, i don't really understand what does the last part of the question mean. Could someone explain it to me?