One mole each of hydrogen, oxygen and nitrogen are mixed in a close container of volume `10` L and temperature `27^(@)C.` Calculate the pressure exerated by the mixture. `(R=.314Jmol^(-1)K^(-1))`

Explanation

Given, `R=.314Jmol^(-1)K^(-1)`
Temperature, `T=27^(@)C=27+273=300K`
Volume `V=10L=10xx10^(-3)m^(3)`
According to Dalton's law of partial pressure,
`p=p_(1)+p_(2)+p_(3)`
`rArr" " p=(muRT)/V+(muRT)/V+(muRT)/V=(3muRT)/V`
where, `mu=1` mole
`therefore" "p=(3RT)/V=(3xx8.314xx300)/(10xx10^(-3))`
`" " =7.48xx10^(-5)Nm^(-2)`