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 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)

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

Calculate the emf of the following cell at 25^(@) C Ag(s) |Ag^(+) ( 10^(-3) M ) | | Cu^(2+) ( 10^(-1) M ) | Cu (s) Given, E_("cell")^(@) = + 0.46 V and log 10^(n) = n .

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")^(@)

Write the cell reaction and calculate the emf of the Cell Zn|Co^2+(aq)|| Zn^2+(aq)| Co (Given E_(Zn|Zn^2+)^@=+0.76V and E_(Co|Co^2+)^@=+0.28V .

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 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 ]

Write the cell reaction and cell potential of the cell Zn//Zn^(2+)(0.01 M)abs"Ag^+(0.1M)//Ag. Given E^0(Zn^(2+)//Zn)=-0.76V E^0(Ag^+//Ag)=+0.80V .

Calculate the standard emf of the cell having the cell reaction. Zn(s) + Co^(2+) ( aq) rarr Zn^(2+) ( aq) + Co(s) E_(Zn//Zn^(2+)) ^(@) = 0.76V, E_(Co//Co^(2+))^(@) = 0.25V