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 0.0

Question

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

TestHub · Accepted Answer

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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