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))`

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)) :

DeltaG^(@) for a reaction 25^(@)C is 3.5kJ xx mol^(-1) . What is the value of K?

The electrochemical cell shown below is a concentration cell M//M^(2+) (saturated solution of a sparingly soluble salt, MX_(2))||M^(2+)(0.001 mol dm^(-3))|M The emf of the cell depends on the difference in concentrations of Mn^(2+) ions at the two electrodes. The emf of the cell at 298 K is 0.059 V . The value of DeltaG ( kJ "mol"^(-1)) for the given cell is : (take 1 F = 96500 C "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.

Calculate E_(cell)^(@) and DeltaG^(@) for the following reaction at 25^(@)C . A^(2+)+B^(+) to A^(3+)+B (Given K_(c)=10^(10) , 1F=96500" C mol"^(-1) )

For the reduction of silver ions with copper metals, the standard cell potential was found to be +0.4V at 25^(@) C. The value of standard Gibb's energy DeltaG^(@) will be (F=96500 C mol^(-1)) :-