The equilibrium constant for the reaction 2no(g)+br2(g)⥫⥬==2nobr(g) is kc=1.3×10−2 at 1000 k. at this temperature does the equilibrium favor no and br2, or does it favor nobr? calculate kc for 2nobr(g)⥫⥬==2no(g)+br2(g). calculate kc for nobr(g)⥫⥬==no(g)+12br2(g).

Answer :

The equilibrium favors NO and .

(1) The value of equilibrium constant for this reaction is, 76.9

(2) The value of equilibrium constant for this reaction is, 8.77

Explanation:

The given chemical equation is:

The value of equilibrium constant for the above equation is .

The value of that means equilibrium lies to the left side. Thus, the equilibrium favors NO and .

We need to calculate the equilibrium constant for the given equation of above chemical equation, which is:

(1)

The equilibrium constant for the reverse reaction will be the reciprocal of the initial reaction.

The value of equilibrium constant for reverse reaction is:

Thus, the value of equilibrium constant for this reaction is, 76.9

(2)

The equilibrium constant for the reverse reaction will be the reciprocal of the initial reaction.

If the equation is multiplied by a factor of '1/2', the equilibrium constant of the reverse reaction will be the 1/2 power of the equilibrium constant of initial reaction.

The value of equilibrium constant for reverse reaction is:

Thus, the value of equilibrium constant for this reaction is, 8.77

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