The standard emf of a galvanic cell involving 2 moles of electrons in it redox reaction is 0.59 V.The equilibrium constant for the redox reaction of the cell is

Options

A. `10^(20)`
B. `10^(5)`
C. 10
D. `10^(10)`

Answer

A

Explanation

Galvanic cell redox reaction is
`Zn_(s)+Cu_((aq))^(2+)hArrZn_((aq))^(2+)+Cu_(s)`
At the equibrium state the concentration of `Cu^(2+)`
and `Zn^(2+)` ions are in equibrium .So `E_(cell)`=0.
Then equilibrium constant ,`K_(c)` is calculated as
`E_(cell)^(@)=(0.059)/(n)logK_(c)` or `0.59=(0.059)/(2)logK_(c)`
or `logK_(c)=(0.59xx2)/(0.059)=20`
`K_(c)`=antilog 20 =`10^(20)`