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The equilibrium constant at 25 ° C for the reaction, 2 N O ( g ) + B r 2 ( g ) ⇌ 2 N O B r ( g ) is equal to 160 a t m - 1 . If the partial pressures of NO, B r 2 and NOBr in a flask at 25 ° C are 0.01, 0.1 and 0.04 atm respectively. It can be said that

Options

  1. Athere is equilibrium in the flask
  2. Bthere reaction will proceed in the forward direction
  3. Cthe reaction will proceed in the backward direction
  4. Dthe partial pressure of NOBr finally will be 0.05 atm

Correct answer

A. there is equilibrium in the flask

Step-by-step solution

Q p = p N O B r ( g ) 2 p N O ( g ) 2 . p B r 2 ( g ) = ( 0.04 a t m ) 2 ( 0.1 a t m ) 2 × ( 0.1 a t m ) = 16 × 1 0 - 4 a t m 2 1 × 1 0 - 4 a t m × 1 × 1 0 - 1 a t m = 160 a t m - 1 Since Q p = K p , therefore there is equilibrium in the flask.

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