Following reactions occurs at cathode during the electrolysis of aqueos sodium chloride solution:
`Na^(+)(aq)+barerarrNa(s)`, `E^@=-2.71V` and `H^(+)(aq)+barerarr1/2H_2(g)`, `E^@=0.00V`
On the basis of their standard reducton electrode potential `(E^@)` values, which reaction is feasible at the cathode and why?

The standard reduction potentials for two reactions are given below: AgCl(s)+barerarrAg(s)+Cl^(-)(aq) , E^@=0.22V and Ag^(+)(aq)+barerarrAg(s) , E^@=0.80V The K_(sp) of AgCl under standard conditions of temperature is given by

Using the standard electrode potentials given in Table 3.1 predict if the reaction between the following is feasible: Br_2 (aq) and Fe^(2+) (aq) .

In a simple electrochemical cell, which is in the standard state, the half cell reactions with their appropriate reduction potentials are: Pb^(2+)(aq)+2barerarrPb(s) , (E^@=+0.13V) . Ag^(+)(aq)+barerarrAg(s) , E^@=+0.80V) What is the cell reaction for the cell?

For the following data at 25^@C Cr^(3+)(aq)+1barerarrCr^(2+)(aq),E^@=-0.424V , Cr^(2+)(aq)+2barerarrCr(s),E^@=-0.900V Find E^@ at 25^@ for the reaction: Cr^(3+)+3barerarrCr(s)

The electrode potentiasl for Cu^(2+)(aq)+barerarrCu^(+)(aq) and Cu^(+)(aq)+barerarrCu(s) are +0.15V and 0.50V respectively. The value of E_(Cu^(2+)|Cu) will be

Given E_(Fe^(3+)|Fe)^@=-0.36V , E_(Fe^(2+)|Fe)^@=-0.439V . The value of standard electrode potential for the change, Fe^(3+)+barerarrFe^(2+) will be

Calcualate the Delta_rG for the reaction: Mg(s)+Cu^(2+)(aq)rarrMg^(2+)(aq)+Cu(s) Given: E_(cell)^@=+2.71V, 1F=96500C mol^-1

Fuel cells convert the energy produced during the combustion of fuels cells directly into electrical energy. Probably the most successful fuel cell so far is hydrogen oxygen fuel cell, which has ben used in spacecraft. The electrodes consist of porous screens of titanium coated with a layer of platinum catalyst. concentrated KOH or NaOH soloution is placed beween the electrodes to serve the as electrolyte. hydrogen and oxygen gases are bubbled through the porous electrodes into the electrolyte solution The following electrodes reactions occur: At anode: 2H_2(g)+4OH^(-)(aq)rarr4H_2O(l)+4bare At cathode: O_2(g)+2H_2O(l)+4barerarr4Oh^-(aq) Overall reaction: 2H_2(g)+O_2(g)rarr2H_2O(l) In this cell, the gaseous materials are consumed and continously supplied. The thermodynamic properties of fuel cell reaction at 25^@C are: DeltaH^@=-285.8kJ mol^-1,DeltaG^@=-237.2kJ mol^-1, E^@=1.23V If the potential of the half cell reaction is at cathode is, E^@=0.41V , then E^@ for the half cell reaction at anode is

Consider the following half cell reaction: Br_2+2barerarr2Br^- , E^@=1.09V I_2+2barerarr2I^- , E^@=0.54V If I_2 and Br_2 are added to solution containing 1M concentration of I^- and Br^- resepctively. How will the increase in the concentration of Br^- affect E_(cell) ?

The standard reduction potential for the half cell: NO_3^- (aq)+2H^+ (aq)+barerarrNO_2+H_2O is 0.78v. What will be the reduction of the half cell in a neutral solution? Assume all the other species to be at unit concentration.