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#
