Following reactions occurs at cathode during the electrolysis of aqueous silver chloride solutoin:
`Ag^(+)(aq)+barerarrAg(s)`
`E^@=+0.80V` and `H^(+)(aq)+barerarr1/2H_2(g)`
`E^@=0.00V`
On the basis of their standard reduction potential values. which reaction is feasible at the cahode 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

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)

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?

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

Two metals A and B have reduction potentials values -0.76V and +0.34V respectively. Which of these will liberate H_2 from dil H_2SO_4 ?

Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V

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

The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is

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.

The equilibrium constant of the following redox reaction is 298K is 1xx10^8 2Fe^(3+)(aq)+2I^-(aq)Leftrightarrow2Fe^(2+)(aq)+I_2(s) If the standard reduction potential of iodine becoming iodide is +0.54V, what is the standard reduction potential of Fe^(3+)/Fe^(2+) ?