For a reaction `A(s)+2B^(+) (aq) rarr A^(2+) (aq) rarr A^(2+)(aq)+2B, K_(C)` has been found to be `10^(12)`. The `E_("cell")^(@)` is 0.354 V

For a reaction A(s)+2B^(o+) rarr A^(2+)+2B K_(c) has been found to be 10^(12) . The E^(c-)._(cell) is

For a reaction A(s)+2B^(o+) rarr A^(2+)+2B K_(c) has been found to be 10^(12) . The E^(c-)._(cell) is

For a reaction A(s) + 2B^(+) rarr A^(2+)+2B(s). K_(c) has been found to be 10^(14) The E^(o) ""_(cell) is :

For a reaction A(s) + 2B^(+) rarr A^(2+)+2B(s). K_(c) has been found to be 10^(14) The E^(o) ""_(cell) is :

For a reaction: A(s) + 2B ^(+) rarr A^(2+) +2 B (s). K_(aq) has been found to be 10^(12) The E^(o) cell is :

For the cell reaction, A(s) + 2B^(-)"(aq) rarr A^(2+) (aq) + 2B(s) , the value of Kc is 3.98 xx 10^(15) .Calculate E_(cell)^(@) at 298 K.

For the cell reaction, Mg(s)+2Ag^(+) (aq.) rarr Mg^(2+) (aq) + 2Ag(s) E_(cell)^(@) : +3.17 V at 298 K. The value of E_(cell)^(@) triangle G^(@) and at Ag^(+) and Mg^(2+) concentrations of 0.001 M and 0.02 M respectively are:

Consider the following cell reaction Cu(s)+2Ag^(+)(aq) rarr Cu^(2+) (aq) +2Ag(s) E_("cell")^(@)=0.46 V By boubling the concentration of Cu^(2+) , E_("cell") is

The cell in which the following reaction occurs, 2Fe^(3+) (aq) + 2I^(-)(aq) rarr 2Fe^(2+) (aq) + I_(2)(s) has E_("cell")^(@) = 0.236V at 298K , calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.