Standard reduction p[otentials of the half rections are given bvelow:
`F_(2)(g)+2e^(-)rarr2F_(aq)^(-):" " E^(@)=+2.85V`
`CI_(2)(g)+2e^(-)rarr2CI(aq)^(-):" " E^(@)=+1.36V`
`Br(2)(g)+2e^(-)rarr2Br(aq)^(-):" " E^(@)=+1.06V`
`I_(2)(s)+2e^(-)rarr2I_(aq)^(-):" " E^(@)=+0.53V`
The stronges oxidising and reducing agents respectively are

Options

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

Explanation

More the value of negative reduction potential stronger in the reducing agent. Therefore, `1^(-)` ion is the stongest reducing agent .More the value of p[ositive reduction potential stronger is the oxidising agent .Therefore,`F_(2)` is the strongest oxidising agent.