Ok, so here is my problem: Suppose 2.00 mole of an ideal, monatomic gas is initially at a pressure of 3.00 atm and a temperature of 350K. It is expanded irreversibly and adiabatically against a constant external pressure of 1.00 atm until the volume has doubled. A) Calculate delta S for the system, the surroundings, and the universe (i.e. total). Hint: To find delta S of system, consider breaking up the expansion into two steps. Based on the properties of and relationships for delta S, think of why you can and must do this. B)If the absolute entropy per mole of the gas before the expansion is 158.2 J/K mol, calculate delta Gibbs free energy for the process. Hint: You must use the generally defined relationship for delta G. We do not want the answers, but my friend and I have no idea where to start. IF you could at least tell us what the hint in part A means we could go from there. Thank you.