Law of Mass Action worksheet
Law of Mass Action states that, ” The rate of chemical reaction at constant temperature is directly proportional to the active mass of the reactant present at that time. If more than one reactant take part in the reaction then the rate of the reaction is proportional to the product of the active masses of the reactants.”
Here, you can find some questions related to “Law of Mass Action” and their answers:
1. Equilibrium constant for the reaction at 780 K and 10 atm pressure is 3.52 . The equilibrium constant of this reaction at 780 K and 20 atm pressure is:
2. The equilibrium constant for the reaction, is 100. If rate constant for forward reaction is , then rate constant for the backward reaction is:
3. For the reaction: , the rate constants for the forward and backward reactions are found to be , respectively, What is the equilibrium constant for the reaction?
4. The rate constants for the forward and backward reactions of hydrolysis of ester are, , respectively. The equilibrium constant of the reaction is:
5. Reaction quotient for the reaction:
Is given by from right to left, if i.e., equilibrium constant:
(b) Q = 0
6. For the reaction; , Equilibrium concentrations of and HI are 8, 3 and 28 mol respectively. Equilibrium constant of the reaction is:
7. For the reaction at equilibrium the concentrations of respectively. The value of Kc for reaction is:
8. What will be the value of equilibrium constant for the reaction, , if its value for the reaction is 64?
9. The equilibrium constant for the reactions, for reaction
and for reaction .
The equilibrium constant (K) for will be:
10. At constant temperature, the equilibrium constant for the decomposition reaction; is expressed by , where p = pressure, x = extent of decomposition. Which one of the following statements is true?
(a) Kp remains constant with change in p & x
(b) Kp increases with decrease of x.
(c) Kp increases with increase of x
(d) Kp increases with increase of p.
11. For a gaseous reaction: , the partial pressures of A, B, C and D at equilibrium are 0.5, 0.8, 0.7and 1.2 atm. The value of Kp for this reaction is:
(a) 2.4 atm
12. For the reaction , the partial pressures of and CO are 4 and 8 atm respectively. The value of Kp for this reaction is:
(a) 14 atm
(b) 16 atm
(c) 18 atm
(d) 12 atm
13. In an equilibrium reaction: the partial pressures and are 0.662, 0.101 and 0.331 atm, respectively. What should be the partial pressure of oxygen if the equilibrium concentration of becomes equal?
1.(d) 2. (a) 3. (b) 4. (b) 5. (c)
6. (a) 7. (a) 8. (b) 9. (a) 10. (a)
11. (c) 12. (b) 13. (a)
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