Equilibrium Constant - Practice Questions & MCQ

The equilibrium constant (K_C) for the reaction at temperature T is  . The value of K_C for the given reaction at the same temperature is : 

A vessel at 1000 K contains CO₂ with a pressure of 0.5 atm. Some of the CO₂ is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is

K_c for m₁A + m₂B = n₁C + n₂D is given by:

The reaction quotient $(\Theta)$ for the reaction is given by:

$
\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \leftrightarrow 2 \mathrm{NH}_3 ; \quad \Theta=\frac{\left[\mathrm{NH}_3\right]^2}{\left[\mathrm{~N}_2\right]\left[H_2\right]^3}
$

The reaction will proceed from right to left if.

The values of K_P1 and K_P2 for the reactions , 

$\begin{aligned} & X \leftrightarrow Y+Z------1 \\ & A \leftrightarrow 2 B------2\end{aligned}$

are in the ratio 9:1 . If degree of dissociation of X and A be equal , then total pressure at equilibrium of equation 1 and 2 are in the ratio :

What range of K_c both reactants and products are equally present in mixture

A vessel at 1000 K contains $\mathrm{CO}_2$ with a pressure of 0.5 atm . Some of $\mathrm{CO}_2$ is converted into CO on addition of graphite. If total pressure at equilibrium is 0.8 atm , then $\mathrm{K}_{\mathrm{P}}$ is :

At $1200 \mathrm{~K}, K_c=36$ for the reaction: $\mathrm{H}_2(g)+\mathrm{I}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$. What is $K_c$ for the following reaction at $1200 \mathrm{~K}$ ?

$
HI(g) \rightleftharpoons \frac{1}{2} H_2(g)+\frac{1}{2} \mathrm{I}_2(g)
$

The formation of these phosgene is represented as , $\mathrm{CO}+\mathrm{Cl}_2 \leftrightarrow \mathrm{COCl}_2$. The reaction is carried out in 500 ml flask . At equilibrium 0.3 mole of phosgene , 0.1 mole of CO and 0.1 mole of Cl₂ are present. The equlibrium constant of the reaction is :