Calculate `E_(cell)^(@)` for the following reaction at `25^(@)C`.
`A+B^(2+)(0.001 M) to A^(2+)(0.0001 M)+B`
(Given. `E_(cell)=2.6805 V, 1 F=96500 C mol^(-1)`

Calculate E_(cell)^(@) and DeltaG^(@) for the following reaction at 25^(@)C . A^(2+)+B^(+) to A^(3+)+B (Given K_(c)=10^(10) , 1F=96500" C mol"^(-1) )

Write the Nernst equation and calculate E.M.F of the following reaction at 298 K Mg // Mg^(2+) (0.1 M)"//" Cu^(2+) (0.01 M) // Cu (s) given E_("cell")^0 = 2.71V,F=96500 C//mol

Calculate the emf of the following cell at 25^(@)C : Ag+(0.001M|Ag(S)||Cu(s) |Cu^(2+)(10^(-1)M), E0Cell =0.46V

b) Calculate Delta_(r)G^(@) for the following reaction: Fe_((aq))^(+2)+Ag_((aq))^(+)rarr Fe_((aq))^(+3)+Ag(s)." "("Given : "E_("cell")^(@)=+0.03V, F=96500C) .

Calculate the cell emf and Delta_(r ) G^(@) for the cell reation at 25^(@)C . Zn(s) | Zn^(@+) ( 0.1 M )|| Cd^(2+) ( 0.01M) | Cd(s) Given, E_(Zn^(2+) //Zn)^(@) = - 0.763V , E_(Cd^(2+) //Cd) ^(@) = - 0.403 V 1F = 96500 C "mol"^(-1) R = 8.314 JK^(-1) "mol"^(-1) ], Find E_("cell")^(@) = E_("cathode")^(@) - E_("anode")^(@) then Delta _(r ) G^(@) by using formula, Delta _(r ) G^(@) = - n FE_("cell")^(@)

Calculate the emf of the following cell at 25^(@)C . Zn|Zn^(2+) (0.001 M) || H^(+)(0.01 M) | H_(2) (1 bar) | Pt(s). Given that E_((Zn^(2+)//Zn))^(@)=-0.76V, E_((H^(+)//H_(2)))^(@)=0.00" V "

Calculate emf of the following cell reaction at 2968 K : Ni(s)//Ni^(2+)(0.01 M) || Cu^(2+)(0.1 M)//Cu(s) [Given E_(Ni^(2+)//Ni)^(@)=-0.25" V ",E_(Cu^(2+)//Cu)^(@)=+0.34 " V " ] Write the overall cell reaction.