1. The problem statement, all variables and given/known data 5 litres of an ideal gas which is initially at 300K and 10atm, and is expanded to a final pressure of 1atm. Find work done, change in internal energy, heat absorbed and change in enthalpy of the system if the process is isothermal and reversible. 2. Relevant equations PV=nRT dU=dQ+W 3. The attempt at a solution I just want to check if I have the correct method here. So using PiVi=nRT to find the number of moles, then the work done is -nRTln(Vf/Vi), where Vf/Vi is the ratio Pi/Pf. Because it is an isothermal process dU=0 → dQ=-W. Also the change in enthalpy will be zero. Thank you for any help. (I have posted this here because there is a second part to the question which I may need help for, but I just want to check if I have the right idea).