# Equilibrium constant Worksheet

Equilibrium constant (kc)  are derived from experimental data. Equilibrium constant is highly temperature dependent.

Equilibrium constant doesn’t change due to the presence of catalyst.

Here are some questions related to “Equilibrium constant” and their answers:

Questions:

1. The relation between $K_p \hspace{3mm} \text{and} \hspace{3mm} K_c$ for the reaction $2NO (g) + Cl_2(g) \leftrightharpoons NOCI (g)$ is:

(a)    $K_p = K_c(RT)^{-1}$

(b)   $K_P = K_c$

(c)    $K_P = K_c / (RT)^2$

(d)   $K_p = K_c/RT$

2. In which of the following gaseous reactions,$K_p \text{and} K_c$ have the same values?

(a)    $2HI \leftrightharpoons H_2 + I_2$

(b)   $N_2 + 3H_2 \leftrightharpoons 2NH_3$

(c)    $2SO_2 + O_2 \leftrightharpoons 2SO_3$

(d)   $PCl_5 \leftrightharpoons PCl_3 + Cl_2$

3. In which of the following gaseous reactions, the value of $K_p$  is less than $K_c$?

(a)    $PCl_5 \leftrightharpoons PCl_3 + Cl_2$

(b)   $2SO_2 + O_2 \leftrightharpoons 2SO_3$

(c)    $2HI \leftrightharpoons H_2 + I_2$

(d)   $N_2 + 3H_2 \leftrightharpoons 2nh_3$

4. The value of $K_c$ for the reaction $N_2 + 3H_2 \leftrightharpoons NH_3$ at 400K is 0.5. The value of $K_p$for the reaction is $(R = 0.0821 L \hspace{2mm}atm \hspace{2mm} mol^{-1} K^{-1})$:

(a)    $25.6 \times 10^{-2}$

(b)   $4.6 \times 10^{-4}$

(c)    $46.6 \times 10^{-4}$

(d)   $16.6 \times 10^{-8}$

5. At 700 K, the equilibrium constant $K_p$ for the reaction $2SO_3 (g) \leftrightharpoons 2SO_2 (g) + O_2 (g)\hspace{2mm} \text{is} \hspace{2mm} 1.80 \times 10^{-3}$.What is the numerical value in mole per litre of equilibrium constant $K_c$ for this reaction at the same temperature?

(a)    $8.1 \times 10^{-8}$

(b)   $9.1 times 10^{-9} mol L^{-1}$

(c)    $3.1 \times 10^{-7}$

(d)   $6.1 \times 10^{-7} mol ^{-1}$

6. For the reaction : $CO(g) + Cl_2 (g) \leftrightharpoons COCl_2(g)$ The value of $K_p / K_c$ is equal to:

(a)    RT

(b)   1/ RT

(c)    1

(d)   $\sqrt{RT}$