An #0.846g# mass of gas exerts a pressure of #752"Torr"#, and expresses a volume of #354*mL#, at a temperature of #100# #""^@C#. What is the molar mass of the gas?

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Answer 1 · 2017-04-20T06:18:18

#"Mass"/"Molar mass"=(PxxV)/(RxxT)#; from where did I get this relationship?

And thus #"Molar mass"=(RxxTxx"mass")/(PxxV)#

#=(0.0821*(L*atm)/(K*mol)xx373*Kxx0.846*g)/((752*"Torr")/(760*"Torr"*atm^-1)xx0.354*L)#

#~=74*g*mol^-1#

An #0.846*g# mass of gas exerts a pressure of #752*"Torr"#, and expresses a volume of #354*mL#, at a temperature of #100# #""^@C#. What is the molar mass of the gas?