Hello everyone. I would like to know if I did this correctly. 1. The problem statement, all variables and given/known data Calculate the heat, internal energy and work of 1 mol of hydrogen, which undergoes a reversible adiabatic expansion from a volume of 5.25 m^3 at 300 K to a volume of 25.5 m^3 3. The attempt at a solution The first thing that I have to do is to find the final temperature using the following equation: (Vf/Vi)^1-y * Ti = Tf y = gamma y = Cp/Cv Because it's HYDROGEN (diatomic gas): y = 7/2/5/2 = 1.4 (25.5 m^3/5.25 m^3)^1.4 * 300 K = Tf Tf = 2741.9 K so... a) Heat becuase it's an ADIABATIC expansion Q = 0 J b) Internal energy: E = n Cv (Tf - Ti) Cv = 5/2 * R E = 1 mol * (5/2) * 8.31 J/mol K * ( 2741.9 K - 300 K) E= 50730.47 J c) Work I've seen the equation in two different ways: E = Q + W AND... E = Q - W Anyway, I'll use the second one (because is the one I have to use according to the worksheet)... W = Q - E W = 0 J - 50730.47 J W = - 50730.47 J Is it ok? Please check it out, because the worksheet doesn't have the answers and I want to know if I did it correctly. Thanks in advance!