A vessel of volume 4 litres contains a mixture of 8 grams of `O_(2)`, 14 grams of `N_(2)` and 32 grams of `SO_(2) at 27^(@) C`. Find the pressure exerted by the mixture. Given, `R = 8.3 J mol_(-1) K_(-1)`.

Explanation

Here, `T=27^(@)C = 27 + 273 = 300K`
From Dalton's law of partial pressures,
`P=P_(o_2) +P_(N_2) +P_(So_2)`
`=(RT)/(V) [ (m_(o_2))/(M_(o_2))+ (m_(N_2))/(M_(N_2)) + (m_(SO_2))/(M_(SO_2))]`
`= (8.3 xx 300)/(4 xx 10^(-3)) [8/32 + 14/28 +32/64]`
`= 7.78 xx 10^(5) N//m^(2)`.