At T K,the equilibrium constants for the fol | vedclass

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(C) Given reactions:$(i) \ 2 A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)} ; K_1 = 16$$(ii) \ 2 B_{(g)} + C_{(g)} \rightleftharpoons 2 D_{(g)} ; K_2 =

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$20$

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(C) Given reactions:$(i) \ 2 A_{(g)} ightleftharpoons B_{(g)} + C_{(g)} ; K_1 = 16$$(ii) \ 2 B_{(g)} + C_{(g)} ightleftharpoons 2 D_{(g)} ; K_2 = 25$We need the equilibrium constant $(K_3)$ for:$(iii) \ A_{(g)} + \frac{1}{2} B_{(g)} ightleftharpoons D_{(g)}$From $(i)$,$K_1 = \frac{[B][C]}{[A]^2} = 16$.From $(ii)$,$K_2 = \frac{[D]^2}{[C][B]^2} = 25$.Multiplying $(i)$ and $(ii)$:$K_1 	imes K_2 = \frac{[B][C]}{[A]^2} 	imes \frac{[D]^2}{[C][B]^2} = \frac{[D]^2}{[A]^2 [B]} = 16 	imes 25 = 400$.Taking the square root of the expression:$\sqrt{\frac{[D]^2}{[A]^2 [B]}} = \frac{[D]}{[A][B]^{1/2}} = \sqrt{400} = 20$.Thus,$K_3 = 20$.

Similar Questions

Explain the use of the equilibrium constant to predict the extent of a reaction with an example.

Assertion: Reaction quotient is defined in the same way as equilibrium constant at any stage of the reaction.
Reason: If $Q_c < K_c$,the reaction moves in the direction of reactants.

$A$ reaction with reaction quotient $Q_C$ and equilibrium constant $K_C$ will proceed in the direction of the products when:

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