What will be the pressure exerted by a mixture of 3.2g of methane and 4.4 g of carbon dioxide contained in a 9`dm^(3)` flask at `27^(@)C` ?

Explanation

Total number of moles (n) in the mixture
`=((3.2)/(16)+(4.4)/(44))=0.3` mol [Molar mass: `CH_(4) implies16, CO_(2) implies 44`]
As given, `V=9dm^(3),T=(273+27)K=300K,P=?`
So, `P=(nRT)/(V)=(0.3xx0.0821L*atm*mol^(-1)*K^(-1)xx300K)/(9dm^(3))`
`=0.821atm[1L=1dm^(3)]`
`=8.316xx10^(4)Pa[1atm=1.013xx10^(5)Pa]`.