`Ag^(+) + NH_(3) ltimplies [Ag(NH_(3))]^(+), k_(1)=6.8 xx 10^(-5)`
`[Ag(NH_(3))]^(+) + NH_(3) ltimplies [Ag(NH_(3))_(2)]^(+)`,
`k_(2) = 1.6xx10^(-3)`
The formation constant of `[Ag(NH_(3))_(2)]^(+)` is :

Options

A. `6.8xx10^(-6)`
B. `1.08xx10^(-5)`
C. `1.08xx10^(-6)`
D. `6.8xx10^(-5)`

Answer

B

Explanation

The required reaction is `Ag^(+) +2NH_(3) + [Ag (NH_(3))_(2)]^(+), K=` ?
From the given equations, we have
`k_(1)=([Ag(NH_(3))]^(+))/([Ag^(+)][NH_(3)]), k_(2) =([Ag (NH_(3))_(2)]^(+))/([Ag (NH_(3))]^(+)[NH_(3)])`
If equations are added, their rate constants are multiplied.
`therefore` The value of K is given by
`K=k_(1)xxk_(2) =6.8xx10^(-2)xx1.6xx10^(-3)=1.08xx10^(-5)`