Pure CO2 at 3.0 atm is passed into a rigid vessel containing excess hot C(s). At equilibrium of C(s) + CO2(g) 2CO(g) at constant temperature, K_p = 1.5 atm. The total pressure at equilibrium (in atm) is

JEE Advanced levelSingle correct optionDifficulty 3 of 3ce103

Pure $CO X_{2}$ at 3.0 atm is passed into a rigid vessel containing excess hot $C (s)$ . At equilibrium of $C (s) + CO X_{2} (g) 2 CO (g)$ at constant temperature, $K_{p} = 1.5$ atm. The total pressure at equilibrium (in atm) is

Let

CO X_{2}

fall by

x

atm; then

p_{CO} = 2 x

and

p_{CO X_{2}} = 3.0 - x

K_{p} = 4 x^{2} / (3.0 - x) = 1.5

gives

4 x^{2} + 1.5 x - 4.5 = 0

, so

x = 0.8896

atm. Total pressure

= (3.0 - x) + 2 x = 3.0 + x = 3.89

atm.