For the reaction,
`Ag^(+)+2" NH"_(3)iff["Ag"(NH_(3))_(2)]^(+),`
the net rate of reaction is given by
`(dx)/(dt)=2xx10^(7)["Ag"^(+)][NH_(3)]^(2)-1xx10^(-2)["Ag"(NH_(3))_(2)]^(+)`
Then which of the following statement/s is/are correct ?

Options

A. Rate constant for forward reaction `=2xx10^(7)`
B. Rate constant for backward reaction `=1xx10^(-2)`
C. Equilibrium constant of the reaction `=2xx10^(9)`
D. All the above

Answer

D

Explanation

Net reaction = Rate of forward reacion - Rate of backward reaction
`=k_(f)` [Reasctants] `-k_(b)` [Products]
Comparing with the given reaction,
`k_(f) = 2 xx 10^(7), k_(b) = 1 xx 10^(-2)`
Eqm. Const.` = k_(f)lk_(b) = ( 2xx 10^(7))//(10^(-2)) = 2xx 10^(9)`.