Calculate the equilibrium constant for the reaction between silver nitrate and metallic zinc.

Explanation

Step 1 : Write the equation for the reaction
`2Ag^(+)+Zn rArr Zn^(2+)+2Ag" "E_("cell")^(@)=1.56V`
Step 2 : Substitute values in the Nernst equation at equilibrium
`kigK=(nE_("cell)^(@))/(0.591)`
`0=2xx1.56-0.03logK`
`-1.56xx2=-0.03logK`
`logK=(-1.56xx2)/(-0.03)=52.79`
`K=6.19xx10^(52)`