1.

The reaction, 2NO+br_(2)to2NOBris supposed to have the meachanism Step -I NO+Br_(2)hArrNOBr_(2) Step-II NOBr_(2)+NOoverset("slow")(to)2NOBr Predict the rate expression for the reaction

Answer»

Solution :The RATE expression is derived by step-II of the reaction mechanism which is a slow step.thus
Rate `=K[NOBr_(2)][NO]`………`(i)`
HOWEVER, `NOBr_(2)` is an intermediate and thus `[NOBr_(2)]` should be eliminated from Eq. `(i)`
Also for, step `(i)` Equilibrium constant `K_(c )` is
`K_(c )=([NOBr_(2)])/([NO][Br_(2)])`...........`(ii)`
`:.[NOBr_(2)]=K_(c )[NO][Br_(2)]`
Then from Eqs. `(i)` and `(ii)`
Rate `=k.K_(c )[NO]^(2)[Br]^(2)`
Rate `=K.[NO]^(2)[Br_(2)]`


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