At constant temperature and pressure volume of an ideal gas (molecular mass `28g*mol^(-1)`) is 23.36 times greater than its mole number. Find out its density at the same temperature and pressure.

Explanation

Let us suppose, the volume and density of n mol of an ideal gas are V L and d `g*L^(-1)` at P atm and T K.
Now, `PV=nRT and d=(PM)/(RT), i.e., d=Mxx(n)/(V)`
as given, `V=23.36xxnL and M=28g*mol^(-1)`
`theefore d=28g*mol^(-1)xx(n" mol")/(23.36xxnL)=1.198g*L^(-1)`.