Standard electrode potentials of few half-cell reactions are given below :
`{:(MnO_4^(-)+8H^(+)+5e^(-) to Mn^(2+)+ 4H_2O,,E^@=1.51V),(Cr_2O_7^(2-)+14H^(+)+6e^(-)to 2Cr^(3+)+7H_2O,,E^@=1.33V),(Fe^(3+)+e^(-)to Fe^(2+),,E^@=0.77V),(Cl_2+2e^(-) to 2Cl^(-),,E^@=1.36):}`
Based on the above information match the column I with column II and mark the appropriate choice.

Options

A. A-(i),B-(ii),C-(iii),D-(iv)
B. A-(ii),B-(iii),C-(i),D-(iv)
C. A-(iii),B-(i),C-(iv),D-(ii)
D. A-(iv),B-(ii),C-(iii),D-(i)

Answer

C

Explanation

`MnO_4^(-)`=96500 x 5 F = 482500 C
`Cr_2O_7^(2-)`=96500 x 6 F = 579000 C
`Fe^(3+)` = 96500 x 1 F = 96500 C
`Cl_2`=96500 x 2 F = 193000 C