The standard potential for the reaction,
`Ag^(+)(aq.)+Fe^(2+)(aq.)toFe^(3+)(aq.)+Ag(s)`
is 0.028V. What is the standard free energy change for this reaction?

Calculate Delta_rG^@ for the following reactions: Fe^(+2) (aq)+Ag^(+) (aq) to Fe^(+3) (aq)+Ag (s)

The standard reduction potentials for the two half-cell reactions are given below : Cd^(2+) (aq) + 2e^(-) to Cd(s) , E^(0) = -0.40 V " "Ag^(+)(aq) + e^(-) to Ag(s) , E^(0) = 0.80 V The standard free energy change for the reaction 2Ag_((aq))^(+) + Cd_((s)) + Cd_((aq))^(2+) is given by

The standard rectuion potentials for two half-cell reactions are given below Cd^(2+)(aq)+2e^(-)rarrCd(s),E^(@)=-0.40V Ag^(+)(aq)+e^(-)rarrAg(s),E^(@)=0.80V The standard free energy change for the reaction 2Ag^(+)(aq)+Cd(s)rarr2Ag(s)+Cd^(2+)(aq) is given by

The standard e.m.f. of the cell involving the reaction 2Ag^(+) (aq)+H_2(g)→2Ag(s)+2H^(+) (aq), is 0.80 V. The standard oxidation potential of Ag electrode is

Calculate the equilibrium constant for the following reaction at 25^@C . Ag^(+)(aq) + Fe^(2+)(aq) to Ag(s) + Fe^(3+)(aq) The standard emf of the corresponding voltaic cell is 0.03 V.

The emf of the cell involving the reaction 2Ag^(+) (aq)+H_(2)(g) rarr 2Ag(s)+2H^(+) (aq) is 0.080 V . The standard oxidation potential od silver electrode is

Consider the reaction 2 Ag^+_("(aq)") + Cd_("(s)") to 2 Ag ("(s)") + Cd ^( +2 ) _ ("(aq)") . The standard electrode potential for Ag ^+|Ag and Cd ^ ( + 2 ) | Cd coples are + 0.80 volt and -0.40 volt respectively. The standard cell potential for this reaction will be

Use the standard potentials of the couples Au^(+)//Au(+1.69V),Au^(3+)//Au(+1.40V), and Fe^(3+)//Fe^(2+)(+0.77V) to calculate the equilibrium constant for the reaction 2Fe^(2+)(aq)+Au^(3+)(aq) leftrightarrow2Fe^(3+)(aq)+Au^(+)(aq)