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

Explanation

We are given that
Mass of methane = 3.2 g
Mass of carbon dioxide = 4.4 g
Volume of flask = 9 `dm^(3)`
Temperature `=27^(@)C`
We are to find out the pressure exerted by the mixture.
Molar mass of methane = 16 g/mol
Molar mass of carbon dioxide = 44 g/mol
Number of moles of methane `(nCH_(4)) =(3.2)/(16g//mol)=0.2mol`
Number of moles of `CO_(2)(nCO_(2)) =(4.4g)/(44g//mol)=0.1 mol`
`PV= (nCH_(4)+nCO_(2))RT`
`P xx 9dm^(3) = (0.2 mol +0.1 mol) xx 0.0821 dm^(3) "atm K"^(-1)"mol"^(-1) xx 300K`
`P=(0.3 xx 0.0821xx300)/(9) "atm"=8.314 xx 10^(4)Pa`.