One half mole each of nitrogen, oxygen and carbon dioxide are mixed in enclosure of volume 5 litres and temperature `27^(@) C`. Calculate the pressure exerted by the mixture. Given `R = 8.31 J mol^(-1) K^(-1)`.

Explanation

Here, `V=5 litre = 5 xx 10^(-3) m^(3)`
`T= 27^(@)C = 27+273 = 300K, p=?`
According to Dalton's law of partial pressure,
`p=p_(1)+p_(2)+p_(3)`
`p = (mu Rt)/(V) + (mu Rt)/(V) +(mu Rt)/(V)= (3mu Rt)/(V)`
As, `mu = 1/2`, therefore,
`p=(3RT)/(2V) = (3xx 8.31 xx(27+273))/(2 xx 5 xx 10^(-3))`
`p=(3xx8.31 xx 300)/(10^(-2)) = 7.48 xx 10^(5)Nm^(-2)`.