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In reaction A +2 ~B 2 C + D , initial concentration of B was 1.5 times of [A] , but at equilibrium the concentrations of A and B became equal. The equilibrium constant for the reaction is :

Options

  1. A8
  2. B4
  3. C12
  4. D6

Correct answer

B. 4

Step-by-step solution

Hence K _ C = (2 x)^2 x (a-x)(1.5 a-2 x)^2 Given, at equilibrium array ll & (a-x)=(1.5 a-2 x) & a=2 x array On solving K_C=4

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