Calculate the volume occupied at `27^(@)C` and 2 bar pressure of a gas evolved from 2 mL of solid carbon dioxide. Given the density of solid carbon dioxide is `1.53 g mL^(-1)`.

Answer

`0.865 L`

Explanation

Step I. No. of moles of `CO_(2)(g)`
No. of moles of `CO_(2)(n) = ("Mass of " CO_(2)(g))/("Molar mass ") = ("Density" xx "Volume")/("Molar mass")`
`= ((1.53 g mL^(-1)) xx (2 mL))/((44 g mol^(-1))) = 0.0695` mol.
Step II. Volume of `CO_(2)(g)`
According to ideal gas equation,
`PV = nRT , n = 0.0695 mol, P = 2 "bar", T = 300 K`,
`:. V = (nRT)/(P) = ((0.0695 mol) xx (0.083 L "bar" K^(-1) mol^(-1)) xx (300 K))/((2 "bar")) = 0.865 L`