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

Explanation

Number of moles of methane `(n_(1)) = ("Mass of methane")/("Molecular mass ") = ((3.2 g))/((16.0 g mol^(-1))) = 0.2 mol`
Number of moles of carbon dioxide `(n_(2)) = ("Mass of" CO_(2))/("Molecular mass") = ((4.4 g))/((44.0 g mol^(-1))) = 0.1 mol`
Partial pressure of methane i.e., `P_(CH_(4)) = (n_(1)RT)/(V) = ((0.2 mol) xx (8.314 Pa m^(3)K^(-1) mol^(-1)) xx (300 K))/((9 xx 10^(-3) m^(3))) = 5.543 xx 10^(4) Pa`
Partial pressure of `CO_(2)` i.e., `P_(CO_(2)) = (n_(2)RT)/(V) = ((0.1 mol) xx (8.314 Pa m^(3) K^(-1) mol^(-1)) xx (300 K))/((9 xx 10^(-3)m^(3)))`
`= 2.771 xx 10^(4) Pa`
Total pressure of gaseous mixture `= 5.543 xx 10^(4) Pa + 2.771 xx 10^(4) Pa`
Total pressure of gaseous mixture `= 5.543 xx 10^(4) Pa + 2.771 xx 10^(4) Pa = 8.314 xx 10^(4) Pa`