The standard potential of a cell using the reaction `+3HgO(s)+2(overset(c-)(O)H) (aq)` is `0.489V` at `25^(@)C`. What is the equilibrium constant of the reaction ?

Explanation

Anode `: MnO_(4)^(c-)+2H_(2)O+3e^(-) rarrMnO_(2)(s)+4overset(c-)(O)H]xx2 ` Cathode `: Hg(s)+2overset(c-)(O)H rarr H_(2)O+HgO+2e^(-)]xx3`

Cell is in equilibrium,
`:. E_(cell)=0`
`=E_(cell)=E^(c-)._(cell)-(0.059)/(6)log K`
`:. log K =(nE^(c-)._(cell))/(0.059)=(6xx0.489)/(0.059)=49.56`
`K=3.631xx10^(49)`