Represent the cell for the reaction
`Mg_(s)+Cu_(aq)^(+2)rarrMg_(aq)^(+2)+Cu_(s)`

(a) What are fuel cells ? Explain the electrode reactions involved in the working of H_(2)-O_(2) fuel cell. (b) Represent the galvanic cell in which the reaction Zn(s) + Cu^(2)(aq) to Zn^(2+) (aq) + Cu(s) takes place.

The standard electrode potential for Daniel cell is 1.1V . Calculate the standard Gibbs energy of the reaction (In KJ/mol) Zn_((s))+Cu_((aq))^(2+)rarrZn_((aq))^(2+)+Cu_((s))

The electrochemical cell representing the given reaction Ni(s)+Cu^(2+) rarr Ni^(2+)+Cu(s)

Consider the cell reaction : Mg(s)+Cu^(2+)(aq) rarr Cu(s) +Mg^(2+)(aq) If E^(c-)._(Mg^(2+)|Mg(s)) and E^(c-)._(Cu^(2+)|Cu(s)) are -2.37 and 0.34V , respectively. E^(c-)._(cell) is

(a) Calculate Delta_(r)G^(@) for the reaction Mg(s)+Cu^(2)(aq)rarrMg^(2+)(aq)+Cu(s) Given : E^(@)cell=+2.71 V,1F=96500 C mol^(-1) (b) Name the type of cell which was used Apollo space progromme for providing electrical, power

(CU^(+) ((aq)) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu_((aq))^(+) Cu_((aq))^(2+) +Cu_((s)) choose E^(@) for the above reaction if E_(Cu^(2+)//Cu^(@))= 0.34V and E_(Cu^(2+)//Cu^(+) )= 0.15V

The standard electrode potential for Deniell cell is 1.1V . Calculate the standard Gibbs energy for the reaction. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)

Calculate the standard free energy change for the following reaction Zn(s) + Cu^(2+)(aq) to Zn^(2+) (aq) + Cu(s) Given : Delta_fG^@ [Cu^(2+)(aq)] = 65.0kJ mol^(-1) Delta_f G^@ [ Zn^(2+) (aq)] = -147.2 kJ mol^(-1)

E^(@) for the electrochemical cell Zn(s)|Zn^(2+) 1 M (Aq.)||Cu^(2+) 1 M (aq.)|Cu(s) is 1.10 V at 25^(@)C . The equilibrium constant for the cell reaction, Zn(s) +Cu^(2+) (aq.) hArr Zn^(2+) (aq.)+Cu(s) Will be :

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V