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:


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}


1.(a)     2. (a)    3. (d)     4. (b)     5. (c)     6. (b)

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