Question #ca88b

1 Answer
Oct 11, 2016

Q1

Given Molar mass of the gas #146" g/mol"#

By Ideal gas law we know

#PV=w/MRT#

where

#P->"Pressure of the gas"=1atm#

#V->"Volume of the gas"#

#R->"Universal gas constant"=0.082LatmK^-1mol^-1#

#T->"Temperature of the gas in K"=(150+273)K=423K#

#w->"Mass of the gas"#

#M->"Molar mass of the gas"=146" g/mol"#

#PV=w/MRT#

#=>P=(w/V)/MRT=D/MxxRT#

#" where " D="Density of the gas at given temperature and pressure"#
So
#D=(PM)/(RT)#

Inserting values we have

#=>D=(PM)/(RT)=(1xx146)/(0.082xx423)=4.21g/L#

Q2

By ideal gas law we have

#(P_1V_1)/T_1=(P_2V_2)/T_2......(2)#

Given
#P_1->"Initial pressure"=73 cm=73/760atm#

#T_1->"Initial Temperature"=68^@F=xK#

#(x-273)/(373-273)=(68-32)/(212-32)#

#=>x=36/180xx100+273=293K#

#V_1->"Initial Volume"=875mL=0.875L#

#P_2->"Final pressure"=12atm#

#T_2->"Finial Temperature"=350K#

#V_2->"Final Volume"=?#

Inserting values in equation (2)

#(P_1V_1)/T_1=(P_2V_2)/T_2#

#=>(P_2V_2)/T_2=(P_1V_1)/T_1#

#=>V_2=(P_1V_1T_2)/(P_2T_1)#

#=>V_2=(73/760xx0.875xx350)/(12xx293)L~~0.0084L=8.4mL#