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Redox reactions play a vital role in che...

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 iodide

C

Iodide ion is oxidised by chlorine

D

`Mn^(2+)` is oxidised by chlorine

Text Solution

Verified by Experts

The correct Answer is:
D
Calculate the EMF of all the cells. Only the EMF of the cell involving the oxidation of `I^(-)` ion by `Cl_(2)` is +ve.
`{:(2I^(-) rarr I_(2)+2e^(-)", "E^(@)=-0.54 V),(Cl_(2)+2e^(-) rarr 2Cl^(-)", "E^(@)=+1.36 V),(bar(Cl_(2)+2I^(-) rarr 2Cl^(-)+I_(2), E_("cell")^(@)+0.82 V)):}`
Thus, option (c) is correct.
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