Density of a gas is found to be `5.46g//dm^(3)` at `27^(@)C` and 2 bar presure. What will be its density at STP?

Explanation

Density (d) pressure (P) absolute temperature (T) and molar mass of a gas (M) are related by, d=PV/RT
Under the conditions of T=(273+27)K=300K and
P=2car, the density of the gas (d)`=5.46g*dm^(-3)`
`therefore 5.46g*dm^(-3)=((2xx1.013)atmxxM)/(0.0821atm*dm^(3)*mol^(-1)*K^(-1)xx300K)`
or, `M=66.37g*mol^(-1)`
At STP, if the density of the gas be `d_(1)`, then
`d_(1)=(PM)/(RT)=(1xx66.37)/(0.0821xx273)` [at STP, T=273K, P=1atm]
`=2.96g*L^(-1)=2.96g*dm^(-3)`.