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

Standard reduction p[otentials of the half rections are given bvelow:

1.	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
Answer» `F_(2) and I^(-)`<BR>`Br_(2) and CI^(-)` `CI_(2) and Br^(-)` `CI_(2) and I_(2)` Solution :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.