For C(s) + CO2(g) 2CO(g) with Delta H > 0, in a closed vessel, which statements are correct?

Raising the temperature increases K_p

Adding more C(s) at constant T and V does not shift the equilibrium

Raising the temperature increases K_p

Adding more C(s) at constant T and V does not shift the equilibrium

Compressing the gases at constant T increases K_p

JEE Main levelOne or more correct optionsDifficulty 2 of 3ce087

For $C (s) + CO X_{2} (g) 2 CO (g)$ with $Δ H > 0$ , in a closed vessel, which statements are correct?

The forward reaction is endothermic, so

K_{p}

rises with

T

. Pure solid

C

does not appear in

K

, so adding it has no effect.

K_{p}

depends only on temperature, so compression does not change it (compression shifts the equilibrium back towards

CO X_{2}

instead). Here

Δ n = 2 - 1 = + 1

, so

K_{p} = K_{c} RT

holds. Statements 1, 2 and 4 are correct.