Redox reactions play a vital role in chemistry and biology. The values of standard redox potential `(E^(@))` of two half-cells reactions decide which way the reaction is expected to proceed. A simple example is a Daniell cell in which zince goes into solution and copper gets deposited. Given below are set of half-cell reactions (acidic medium ) along with their `E^(@)` in V with respect to normal hydrogen electrode values.
`{:(l_(2)+2e^(-)rarr2l^(-),E^(@)=0.54),(Cl_(2)+2e^(-)rarr2Cl^(-)" ",E^(@)=1.36),(Mn^(3+)+e^(-)rarrMn^(2+),E^(2)=1.50),(Fe^(3+)+e^(-)rarrFe^(2+)" ",E^(@)=0.77),(O_(2)+4H^(+)+4e^(-)rarr2H_(2)O,E^(@)=1.23):}`
Among the following, identify the correct statement
A. Chloride ion is oxidised by `O_(2)`
B. `Fe^(2+)` is oxidised by chlorine
C. Iodide ion is oxidised by chlorine
D. `Mn^(2+)` is oxidised by chlorine
