When the following redox reaction is balanced in basic medium, `MnO_(4)^(-) +C_2 O_(4)^(2-) to MnO_2 +CO_(3)^(2-)` Which of the following statements applies appropriately to the balanced reaction?

Options

A. 1.50 moles of oxalate would be oxidized per mol of permanganate
B. Oxidation number of carbon is changing from 2 to+4
C. The equivalent weight of `KMnO_4` in the above redox reaction is one-third of its molar mass
D. In the balanced reaction, `4OH^(-) ` appears on the reactants side

Answer

A, C, D

Explanation

The balanced redox reaction is : ` 2 MnO_(4)^(-) + 3C_2 O_(4)^(2-) + 4OH^(-) to 2MNO_(2) + 6CO_(3)^(2-) + 2 H_2 O`