The equlibrium constant `K_(c)` for the reaction of `H_(2)` with `I_(2)` is 57.0 at 700K
`H_(2)(g)+I_(2)(g)underset(k_(b))overset(k_(f))(hArr) 2HI, K_(c)=57` at 700K Select correct statement `:`

Options

A. rate constant `k_(f)` for the formation of HI is smaller than that of rate constant `k_(b)` f for the dissociation of HI
B. `k_(f)gtk_(b)`
C. addition of catalyst increases value of `K_(c)`
D. addition of catalyst decreases value of `K_(c)`.

Answer

B

Explanation

`R_(f)=k_(f)[H_(2)][I_(2)]`
`R_(b)=k_(b)[HI]^(2)`
At equilibrium,
`R_(f)=R_(b)`
`k_(f)[H_(2)][I_(2)]=k_(b)[HI]^(2)`
`(k_(f))/(k_(b))=([HI]^(2))/([H_(2)][I_(2)])=K_(c)`
As `K_(c)=57`
`:. k_(f)gtk_(b)`