Calculate the emf at `25^@C` for the cell `Mg(s)|Mg^(2+) (0.01M)||Sn^(2+)(0.1M)|Sn(s)` (Given `E_(Mg^(2+)|Mg)^0 = -2.34V` & `E_(Sn^(2+)|Sn)^0 = -0.136V)`

Find the cell potential at 25^@C for the cell- Mg//Mg^(2+)(0.001)//Cu^(2+)(0.0001 M)//Cu Given E^@(Mg^(2+)//Mg) = - 2.37V , E^@(Cu^(2+)//Cu) =+0.34V

Calculate the emf of the following cell. Zn(s)|Zn^(2+) (0.01M)|| Ag^+ (0.001M) | Ag(s) Given E_(Zn|Zn^(2+))^@ = 0.76V and E_(Ag|Ag^+)^@ = -0.80V

Calculate the emf for the given cell at 25^(@)C . Cr| Cr^(3+) ( 0.1M) || Fe^(2+) ( 0.01M) | F e [Given, E_(Cr^(3+)//Cr)^(@)= -0.74V, E_(Fe^(2+)//Fe)^(@) = -0.44V ]

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 standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

Calculate the EMF of following cell at 298K Fe(s) |Fe^(2+)(0.1M)| | Ag^(+)(0.1M)|Ag(s) Fe^(2+)|Fe = - 0.41V, Ag^(+)|Ag = +0.80V

Write the Nernst equation and emf of the following cell at 298 K. (i) Mg(s) |Mg^(2+) ( 0.001 M) || Cu^(2+) ( 0.0001M ) | Cu(s) (ii) Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M) | H_(2)(g) (1 "bar") | Pt(s) Given that, E_(Mg^(2+) //Mg)^(@) = - 2.36V , E_(Cu^(2+) Cu)^(@) = 0.34V, E_(Fe^(2+)Fe)^(@) = -0.44V

Calculate the emf of the following cell at 25^(@)C Fe|Fe^(@+) ( 0.001 M ) || H^(+) ( 0.01M ) || H_(2) ( g) ( 1 "bar" ) | Pt (s) E_((Fe^(@+) //Fe))^(@) = - 0.44 V , E_((H^(+) //H_(2)))^(@) = 0.00V

Calculate the equilibrium constant for the reaction. Fe(s) + Cd^(2+) (aq) hArr Fe^(2+)(aq) + Cd(s) [ Given, E_(Cd^(2+) //Cd)^(@) = - 0.40V , E_(Fe^(2+)//Fe)^(@) = - 0.44 V ]