1. The problem statement, all variables and given/known data A 740g quantity of an ideal gas undergoes a reversible isothermal compression at a temperature of 330 K. The compression reduces the volume of the gas from 0.40 m3 initially, to 0.32 m3 finally. The entropy change of the gas is equal to: A) -43 J/K B) -150 J/K C) 43 J/K D) 150 J/K E) 0 J/K 2. Relevant equations ΔS = nR*ln(Vf/Vi) 3. The attempt at a solution I actually know exactly how to solve this problem. The only thing is, I haven't been able to determine n, the number of moles, without being given the molar mass. Is there some method to determine n that I'm missing, or has my prof omitted a vital piece of information (the molar mass)?