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

A vesel of volume V = 5.0 litre contains 1.4 g of nitrogen at temperat

1.	A vesel of volume V = 5.0 litre contains 1.4 g of nitrogen at temperature, T = 1800 K. Find the pressure of the gas if 30% of its molecules are dissociated into atoms at this temperature.
Answer» SOLUTION :Mass of molecular nitrogen Mass of atomic nitrogen `=30/100 times 1.4=0.42g` Number of moles of atomic nitrogen, `n_(1)=0.42/14=0.03` The PRESSURE of the gas = pressure exerted by molecular + 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) times8.31 times 1800)/(5 times 10^(-3))=1.94 times 10^(5)N//m^(2)`.