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A vessel of volume , V = 5.0 litre conta...

A vessel of volume , `V = 5.0` litre contains `1.4 g` of nitrogen at a temperature `T = 1800 K`. Find the pressure of the gas if `30%` of its molecules are dissociated into atoms at this temperature.

Text Solution

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Mass of molecular nitrogen
`=70/100xx1.4=0.98g`
Mass of atomic nitrogen
`=30/100xx1.4=0.42g`
Number oif moles of molecular nitrogen
`n_(1)=0.98/28=0.035`
Number of moles of atomic nitrogen
`n_(2)=0.42/1.4=0.03`
The pressure of the gas = pressure exerted by molecular nitrogen + pressure exerted by atomic nitrogen
i.e. `P=P_(1)+P_(2)`
`=(n_(1)RT)/V+(n_(2)RT)/V=((n_(1)+n_(2))RT)/V`
`=((0.035+0.03)xx8.31xx1800)/(5xx10^(-3))`
`=1.94xx10^(5)N//m^(2)`
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