` E^@` for ` F_2 + 2e rarr 2F^- `is ` 2. 8 V, E^@ ` for ` 1/2 F_2 +e rarr F^- is .

E^@ for F_2 +2erarr 2F^- is 2.8V,E^@ for 1//2F_2+erarr F^- is :

E^(@) for F_(2)+2e^(-) rarr 2F^(-) is 2.8V,E^(@) for (1)/(2)F+e^(-)rarrF^(-) is

E^(0) for F_2 + 2e^(-) to 2F^(-) is 2.8 V , E^(0) for 1//2 F_2 + e^(-) to F^(-) is

E^@ for F_2+2e=2F^(-) is 2.8V, E^@ for 1/2 F_2+e=F^(-) is

E^(@) for F_(2)+2e^(-) hArr 2F^(-) is 2.8V,E^(@) for (1)/(2)F+e^(-)=F^(-) is -

E^(@) for F_(2)+2e^(-) hArr 2F^(-) is 2.8V,E^(@) for (1)/(2)F+e^(-)=F^(-) is -

E^(@) for F_(@)+2e hArr2F^(-) is 2.7 V Thus, E^(@) for F^(-) hArr(1)/(2)Fe +e is :

E^(0) for F_(2)+2eto2F^(-) is 2.8V,E^(0) for (1)/(2)F_(2)toF^(-) is

Standrd reduction potentials of the half reactions are given below : F_2 (g) +re^- rarr 2 F^(-) (aq) E^@ = + 2.85 V Cl_2 (g) +2e^- rarr 2 Cl^-(aq) , E^2 = + 1.36 V Br _2 (i) + 2 e^- rarr 2Br (aq) , E^2 = + 1. 06 V I_2 (s) + 2 e^- rarr 2I^(-) (aq) , E^2 = + . 53 V . The strongest oxidizing and reducing agents respectively