Determine the density of chlorine gas at 22.0°C at 1 ATM? Chemistry Gases Ideal Gas Law 1 Answer anor277 Apr 27, 2017 Well, since #PV=nRT#, #rho~=3*g*L^-1# Explanation: If #PV=nRT# by the Ideal Gas equation, then............. #P/(RT)=n/V=("mass"/"molar mass")/V#..........and Thus, #(P)/(RT)xx"molar mass"="mass"/"volume"=rho, "i.e. density."# So thus #rho=(1*atmxx70.9*g*mol^-1)/(0.0821*(L*atm)/(K*mol)xx295*K)=2.93*g*L^-1# #"Is the molar mass of chlorine gas correct? Why?"# Answer link Related questions How do you find the ideal gas constant? How do you solve ideal gas law problems? How do you know which ideal gas constant to use? What is the ideal gas constant for butane? Why is ideal gas law in kelvin? Why is the ideal gas constant important? What is the di-electric constant? What volume (L) will 0.20 mol HI occupy at 300 K and 100.0 kPa? R = 8.314 kPa L / (K mol) =... How do you calculate the molar mass of a gas? When should I use the ideal gas law and not the combined gas law? See all questions in Ideal Gas Law Impact of this question 17854 views around the world You can reuse this answer Creative Commons License