Given :
`Hg_(2)^(2+) rightarrow 2Hg`, `E^(@) = 0.789 V` and `Hg^(2+) + 2e^(-) rightarrow Hg`, `E^(@) = 0.854V`
Calculate the equilibrium consant for `Hg_(2)^(2+) rightarrow Hg + Hg^(2+)`.

Given : Hg_(2)^(2+) +2 e ^(-)rightarrow 2Hg , E^(@) = 0.789 V and Hg^(2+) + 2e^(-) rightarrow Hg , E^(@) = 0.854V Calculate the equilibrium consant for Hg_(2)^(2+) rightarrow Hg + Hg^(2+) .

Standard potentials (E°) for some half-reactions are given below: Sn^(4+) + 2e rightarrow Sn^(2+) , E^(@) = + 0.15V 2Hg^(2+) + 2e rightarrow Hg_(2)^(2+) , E^(@) = 0.92 V pbo_(2) + 4H^(+) + 2e rightarrow pb^(2+)+ 2H_(2)O , E^(@) = + 1.45 V Based on the above , Which one of the following statement is correct?

Mercurous ion exists as Hg_(2)^(2+) . Explain.

In the reaction, 2HgOrarr2Hg+O_(2),Hg^(2+) act as

Hg_(2)CI_(2) is produced by the electrolytic reduction of Hg^(2+) ion in presence of CI^(-) ion is 2Hg^(2+) +2CI^(-) +2e^(Theta) rarr Hg_(2)CI_(2) . Calculate the current required to have a rate production of 44g per hour of Hg_(2)CI_(2) . [Atomic weight of Hg = 200.6] :-

Hg_(2)CI_(2) is produced by the electrolytic reduction of Hg^(2+) ion in presence of CI^(-) ion is 2Hg^(2+) +2CI^(-) +2e^(Theta) rarr Hg_(2)CI_(2) . Calculate the current required to have a rate production of 44g per hour of Hg_(2)CI_(2) . [Atomic weight of Hg = 200.6] :-

Hg_(2)CI_(2) is produced by the electrolytic reduction of Hg^(2+) ion in presence of CI^(-) ion is 2Hg^(2+) +2CI^(-) +2e^(Theta) rarr Hg_(2)CI_(2) . Calculate the current required to have a rate production of 44g per hour of Hg_(2)CI_(2) . [Atomic weight of Hg = 200.6] :-