For the reaction: N2 (g) + 3H2 (g) 2NH3 (g)

Equilibrium constant Kc =


Some reactions are written below in Column I and their Equilibrium constants in terms of Kc are written in Column II. Match the following reactions with the corresponding Equilibrium constant


Column I (Reaction) Column II (Equilibrium constant)




Given, N2 (g) + 3H2 (g) 2NH3 (g)


(i) 2N2 (g) + 6H2 (g) 4NH3 (g) - (d) K2c


Explanation: The Equilibrium constant depends on the stoichiometric coefficient of reactants and products. Here the no of moles is getting double therefore if the initial value of Equilibrium constant was Kc so it will increase two times i.e. K2c.


(ii) 2NH3 (g) N2 (g) + 3H2 (g) - 1/Kc


Explanation: In this equation, the reaction is in reverse order therefore if the initial value of Equilibrium constant was Kc then now it will also get inversed for the given reaction and will become 1/Kc because Equilibrium constant for the reverse reaction is the inverse of the Equilibrium constant for the reaction in the forward direction.


(iii) N2 (g) + H2 (g) NH3 (g) - (b) K1/2c


Explanation: Here the stoichiometric coefficient are changed by multiplying throughout by 1/2 so if the initial value of Equilibrium constant was Kc then now it will get multiplied by 1/2 throughout for the given reaction and the value of Kc will become Knc here n=1/2 so Kc= K1/2c.


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