A `2L` flask contains `1.6 g` of methane and `0.5 g` of hydrogen at `27^(@)C`. Calculate the partial pressure of each gas in the mixture and hence calculate the total pressure.

Explanation

Moles of `CH_(4)=(W)/(Molar weight)=(1.6)/(16)mol=0.1 mol`
Partial pressure of `CH_(4)`
`P_(CH_(4))=n_(CH_(4))xx(RT)/(V)=(0.1xx0.0821xx300)/(2)=1.23 atm`
Moles of `H_(2)=(W)/(Molar weight)=(0.5)/(0.2) mol=0.25 mol`
Partial pressure of `H_(2)`
`P_(H_(2))=n_(H_(2))xx(RT)/(V)=(0.25xx0.0821xx300)/(2)=3.079 atm`
`:. ` Total pressure `=P_(CH_(4))+P_(H_(12))=1.23+3.079=4.31 atm`