Calculate the volume occupied by 8.8 g of `CO_(2)` at `31.1^(@)C` and 1 bar pressure. R= 0.083 bar L `K^(-1)mol^(-1).`

Explanation

From the available data :
No. of moles of `CO_(2)(n) = ("Mass of" CO_(2))/("Molar of mass") = ((8.8 g))/((44 gmol^(-1))) = 0.2 mol`
Pressure of `CO_(2) (P) = 1 "bar"`
Gas constant `(R) = 0.083 "bar" L K^(-1) mol^(-1)`
Temperature `(T) = 273 + 31.1 = 304.1 K`
According to ideal gas equation .
`PV = n RT`
`V = (nRT)/(P) = ((0.2 mol) xx (0.083 "bar" L K^(-1) mol^(-1)) xx (304.1 K))/((1 "bar")) = 5.048 L`.