If 1 g of each of the following gases are takes at STP, which of the gases will occupy (a) greatest volume and (b) smallest volume ?
`Co, H_(2)O, CH_(4), NO`

Explanation

From Avogadro's law, we know that
Volume of 1 mole of the gas = graw molecular mass =22.4 L at STP
Volume occupied by 28 g CO (1 mol CO) =22.4 L at STP
( `:'` Molar mass of `CO=12+16=28" g mol"^(-1)`)
`:.` Volume occupied by `1 g CO=22.4/28 L` at STP
Similarly, volume occupied by 1 g `H_(2)O=22.4/18L` at STP
`( :'" Molar mass of "H_(2)O=(2xx1)+16=18" g mol"^(-1))`
volume occupied by 1 g `CH_(4)=22.4/16 L` at STP
`( :'" Molar mass of " CH_(4)=12+(4xx1)=16" g mol"^(-1))`
Volume occupied by 1 g `NO=22.4/30 L` at STP
`( :'" Molar mass of NO"=14+16=30" g mol"^(-1))`
Thus, 1 g `CH_(4)` will occupy maximum volume while 1 g of NO will occupy minimum volume at STP.