For the reaction `:`
`A+2B^(3+) rarr 2B^(2+)+A^(2+)`
`E^(c-)` of the given redox reaction is `:`
`A^(2+)+2e^(-) rarr A` `E^(c-)=Xv`
`B^(3+)+e^(-) rarr B^(2+)` `E^(c-)=yV`

E^(c-) for FeY^(c-)+e^(c-) rarr FeY^(2-)

1/2 F_(2)+e^(-) rarr F^(-)" "E^(@)=+3.02V Electrode potential for given reaction F_(2)+2e^(-) rarr 2F^(-)

1/2 F_(2)+e^(-) rarr F^(-)" "E^(@)=+3.02V Electrode potential for given reaction F_(2)+2e^(-) rarr 2F^(-)

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 :

The standard reduction potential for half reactions for four different elements. A, B, C and D are: (i) A_(2) + 2e^(-) rarr 2A^(-), E^(@) = + 2.85 V (ii) B_(2) + 2e^(-) rarr 2B^(-), E^(@) = + 1.36 V (iii) C_(2) + 2e^(-) rarr 2C^(-), E^(@) = + 1.06 V (iv) D_(2) + 2e^(-) rarr 2D^(-), E^(@) = + 0.53 V The strongest oxidising reducing agents smong these :

Cell equation : A+2B^(-) rarr A^(2+)+2B, A^(2+)+2e^(-) rarr A" "E^(@)=+0.34V " and " log_(10)K=15.6 at 300 K for cell reactions find E^(@) " for " B^(+)+e^(-) rarr B

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