What is the value of the equilibrium constant for the following reaction ach  at 25 degree C?  Ni(s) and Ag^+    



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Posted on (Answer #1)

The relation between `E^0` and the equilibrium constant K is given by


`rArr lnK=(nFE^0)/(RT)`

Here, relevant `E^0` values are:

Ni(s) → Ni^(2+) +2e- (`E^0=0.25` V)

and Ag^+ + e- → Ag(s) (`E^0=0.80` V) *2

2Ag^+ + 2e- → 2Ag(s) (`E^0=0.80` V)

`E^0` (overall) = 0.80+0.25 = 1.05 V

Plugging in the valuesin the relation of K,

`lnK= (2*96485*1.05)/(8.314*298)`


`rArr K =3.26*10^35`

Hence the value of equilibrium constant for the reaction between Ni(s) and `Ag^+` is `3.26*10^35` .


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