An oxidation- reduction reaction in which 3 electrons are transferred has a `DeltaG^(0)` of `17.37 kJ mol^(-1)` at `25^(@) C` . The value of `E_("cell")^(0)` (in V) is _________ `xx 10^(-2)`
`(1 F = 96, 500 C mol^(-1))`

The value of DeltaG ((KJmol^(-1)) for the given cell is : ( Taken 1F = 96500C mol^(-1)

For the reduction of silver ions with copper metal, the standard cell potential was foound to be +0.46 V at 25^(@) C . The value of standard Gibbs energy, DeltaG^(@) will be (F = 96,500C mol^(-1)) :

For an endothermic reaction energy of activation is E_(a) and enthlpy of reaction is Delta H (both in kJ "mol"^(-1) ). Minimum value of E_(a) will be

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25^(@) C . The value of standard Gibbs energy, DeltaG^(@) will be (F = 96,500C mol^(-1)) :

The standard potential of a cell using the reaction is 1.12 . The heat of the reaction is -504.2kJ mol ^(-1) at 25^(@)C . Calculate the entropy change.

The standard free energy change of a reaction is DeltaG^(@)=-115kJ//mol^(-1) at 298 K. Calculate the value of log_(10)K_(p) (R=8.314JK^(-1)mol^(-1))

Certain reaction is at equilibrium at 82^(@)C and Delta H for this reaction is 21.3 kJ mol^(-1) . What would be the value of Delta S(in JK^(-1) mol^(-1)) for the reaction.

Fuel cells : Fuel cells are galvanic cells in which the chemical energy of fuel cell is directly converted into electrical energy. A type of fuel cell is a hydrogen - oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst ( platinum, silver, or metal oxide ). The electrodes are placed in aqueous solution of NaOH . Oxygen and hydrogen are continuously fed into the cell. Hydrogen gets oxidized to H^(o+) which is neutralized by overset(c-)(O)H, i.e., anodic reaction. At cathode, O_(2) gets reduced to overset(c-)(O)H Hence, the net reaction is The overall reaction has DeltaH=-285.6 kJ mol^(-1) and DeltaG=-237.4 kJ mol^(-1) at 25^(@)C What is the value of DeltaS^(c-) for the fuel cell at 25^(@)C ?

The E^(@) at 25^(@) C for the following reaction at the indicated concentrations is 1.50 V. Calculate the DeltaG in kJ // mol 25^(@) C :

Identify the reaction order form each of the following rate constants: a. k = 7.06 xx 10^(-3) mol L^(-1) s^(-1) b. k = 5.6 xx 10^(-5) s^(-1) c. k = 1.25 xx 10^(-2) mol^(-1)l s^(-1) d. k = 1.25 xx 10^(-2) mol L^(2)s^(-1) e. k = 5.0 xx 10^(-6) atm^(-1)s^(-1)