Question

Question #90bc3

Answer 1

Given

Volume of nitrogen `V=82.1mL=0.0821L`

Pressure of the gas collected excluding aqueous tension

`P=(774.5-14.5)mm=760/760=1atm`

Temperature of the gas `T=(27+273)=300K`

Universal gas constant `R=0.0821LatmK^-1mol^-1`

Let mass of the gas be `w` g

Molar mass of the gas `M=2xx14=28g"/"mol`

So applying Ideal gas equation

`PV=w/MRT`

`=>w=(PVM)/(RT)`

`=>w=(1xx0.0821xx28)/(0.0821xx300)=28/300g`

So percentage of nitrogen in the compound

`=(28/300)/0.14xx100=66.7%`