Calculate the emf of the cell in which the following reaction takes place at two electrodes. `ZnrarrZn^(2+)"_((aq))+2e^-`, `E^@=+0.76V` `Ag^+"_((aq))+e^(-)rarrAg`, `E^@=+0.80V`

Calculate the emf of the cell in which the following reaction takes place, Ni(s) + 2Ag^(+) ( 0.002M) rarr Ni^(2+) ( 0.160M) + 2Ag(s) Given that E_("cell")^(@) = 1.05V

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

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place 2Cr(s) + 3Cd^(2+) ( aq) rarr 2Cr^(3+) ( aq) + 3Cd(s) Calculate Delta_( r) G^(@) and equilibrium constant K of the above reaction at 25^(@)C . [Given, E_(Cr^(3+) //Cr)^(@) = - 0.74 V, E_(Cd^(2+)//Cd)^(@) = - 0.40V, 1F = 96500 C "mol"^(-1)]

Formulate the galvanic cell in which the following reaction takes place. Zn (s) + 2Ag^(+) ( aq) rarr Zn^(2+) (aq) + 2Ag(s) (i) Which one of its electrodes is negatively charged ? (ii) The reaction taking place at each of its electrode. (iii) The carriers of current within this cell.

In the button cells, widely used in watches and other devices, the following reaction takes place Zn (s) + Ag_(2) O(s) + H_(2) O (l) rarrZn^(2+) (aq) + 2Ag(s) + 2OH^(-) (aq) Determine E^(@) and Delta G^(@) for the reaction. (Given, E_(Ag^(+)//Ag)^(@) = + 0.80 V, E_(Zn^(2+)//Zn)^(@) = -0.76 V )