A `2.5 L` flask contains `0.25 mol` each of sulphur dioxide and nitrogen gas at `27^(@)C`. Calculate the partial pressure exerted by each gas and also the total pressure.

Explanation

Partial pressure of sulphur dioxide.
`P_(SO_(2))=nRT//V`
`=(0.25 molxx8.314 J mol^(-1)xx300 K)/(2.5xx10^(-3)m^(3))`
`=2.49xx10^(5)N m^(-2)=2.49xx10^(5)Pa`
Similarly, `P_(N_(2))=2.49xx10^(5)Pa`
Following Dalton's law, we get
`P_(Total)=P_(N_(2))+P_(SO_(2))`
`=2.49xx10^(5)Pa+2.49xx10^(5)Pa`
`=4.98xx10^(5)Pa`