Problem: An oxygen sample of 1.62 L is at 92.3 kPa and 30.0 degrees celsius. (a) What volume would the oxygen occupy if the pressure was 120.0 kPa and the temperature was 0.0 degrees celsius. (b) How many moles of oxygen are in the sample? My Approach: Conversions: 0 degrees celsius = 273k 30 degrees celsius = 303k 92.3 kPa = .911 atm 120.0 kPa = 1.18 atm (a) PV = nRT (.911 atm) (1.62 L) = n (.08206 l*atm/mol*k) (303k) --- finding n from given information n = 0.0594 mol then, i plug that n into PV= nRT ---using second set of given information (1.18 atm) V2 = (0.0594 mol) (.08206 l*atm/mol*k) (273k) V2 = 11.3 L (b) 0.0594 mol O2 ( this was figured earlier) Anyways, I'd like someone to check my work here!!! THANKS!