Standard reduction potentials of the half reactions are given below:
`F_(2)(g)+2e^(-) to 2F^(-)(aq),E^(@)=+2.85V`
`Cl_(2)(g)+2e^(-) to 2Cl^(-)(aq),E^(@)=+1.36V" "Br_(2)(l)+2e^(-) to 2Br^(-)(aq),E^(@)=+1.06V" "I_(2)(s)+2e^(-)to2I^(-)(aq):E^(@)=+0.53V`
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

Higher the value of reduction potential higher will be the oxidising power whereas the lower the value of reduction potential higher will be the reducing power.