Represent the Galvanic cell in which the reaction is
Zn(s) + `Cu^(2+)` `rarr` `Zn^(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.

Depict the galvanic cell in which the cell reaction is Cu+2Ag^(+)rarr2Ag+Cu^(2+)

Depict the galvanic cell in which the reaction : Zn(s)+2Ag^(o+)(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show : a. Which of the electrode is negatively charged ? b. The carriers of the current in the cell. c. Individual reaction at each electrode.

Depict the galvanic in whiCHM the reaction : Zn(s)+2Ag^(o+)(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show : a. WhiCHM of the electrode is negatively CHMarged ? b. The carriers of the current in the cell. c. Individual reaction at eaCHM electrode.

Depict the galvanic in whiCHM the reaction : Zn(s)+2Ag^(o+)(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show : a. WhiCHM of the electrode is negatively CHMarged ? b. The carriers of the current in the cell. c. Individual reaction at eaCHM electrode.

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

The cell reaction Zn(s) + Cu^(+2)rarr Zn^(+2) + Cu(s) is best represented as :

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

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

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