Redox reactions play a pivotal role in chemistry and biology. The values standard redox potential `(E^(c-))` of two half cell reactions decided which way the reaction is expected to preceed. A simple example is a Daniell cell in which zinc goes into solution and copper sets deposited. Given below are a set of half cell reactions `(` acidic medium `)` along with their `E^(c-)(V` with respect to normal hydrogen electrode `)` values. Using this data, obtain correct explanations for Question.
`I_(2)+2e^(-) rarr 2I^(c-)," "E^(c-)=0.54`
`Cl_(2)+2e^(-) rarr 2Cl^(c-), " "E^(c-)=1.36`
`Mn^(3+)+e^(-) rarr Mn^(2+), " "E^(c-)=1.50`
`Fe^(3+)+e^(-) rarr Fe^(2+)," "E^(c-)=0.77`
`O_(2)+4H^(o+)+4e^(-) rarr 2H_(2)O, " "E^(c-)=1.23`
Among the following, identify the correct statement.

Options

A. Chloride ion is oxidized by `O_(2)`.
B. `Fe^(2+)` is oxidized by iodine.
C. Iodide ion is oxidized by chlorine
D. `Mn^(2+)` is oxidized by chlorine.

Answer

c

Explanation

`2I^(c-)+Cl_(2) rarr I_(2)+2Cl^(c-),E^(c-)._(cell)=1.36-0.54=0.82V`
`E^(c-)._(cell)` is `+ve` . Thus, the cell reaction is feasible.