Standard reduction potentials of the half reactions are given below:
`F_(2)(g) + 2e^(-) to 2F^(-) (aq): E^(@) = + 2.85 V`
`Cl_(2)(g) + 2e^(-) to 2Cl^(-) (aq), E^(@) = + 1.36 V`
`Br_(2)I + 2e^(-) (aq): E^(@) = +1.06 V`
`I_(2)(s) + 2e^(-) to 2l^(-) (aq): E^(@) =+0.53 V`
The strongest oxidising and reducing agents respectively are:

Options

A. `F_(2)` and `I^(-)`
B. `Br_(2)` and `Cl^(-)`
C. `Cl_(2)` and `Br^(-)`
D. `Cl_(2)` and `I_(2)`

Answer

A

Explanation

`E^(@)` more positive, reducing agent will be greater.