At 298 K, the standard reduction potentials are 1.51 V for `MnO_(4)^(-), Mn^(2+),1.36V for Cl_(2)/CI^(-) , 1.07 V Br_(2)|. Br^(-)`, and 0.54 V for `l_(2)|l^(-)` At pH=3, permaganate is expected to oxidize (2.303RT/F -0.059 V)

Options

A. `Cl^(-), Br^(-) and I^(-)`
B. `Cl^(-) and Br^(-)`
C. `Br^(-) and I^(-)`
D. `I^(-)` only

Answer

A

Explanation

The reduction potential of `MnO_(4)//Mn^(2)` is more than that of `Cl_(2)//Cl^(-), Br_(2)//Br and I_(2)//I^(-)`, so permanganate is expected to oxidize `Cl^(-), Br^(-) and I^(-)` because `E_("cell")^(@) gt 0`