Which element is reduced in the unbalanced reaction below? I− + MnO4− + H+ = I2 + MnO2 + H2O
I
no reduction occurred in this reaction
O
H
Mn
In the unbalanced reaction, I− + MnO4− + H+ = I2 + MnO2 + H2O, the element that is reduced is Mn.
To determine which element is reduced in the unbalanced reaction, we need to identify the oxidation states of the elements before and after the reaction.
In this reaction:
I− + MnO4− + H+ = I2 + MnO2 + H2O
- The oxidation state of iodine in I− is -1.
- The oxidation state of iodine in I2 is 0.
- The oxidation state of manganese in MnO4− is +7.
- The oxidation state of manganese in MnO2 is +4.
Therefore, iodine undergoes a change from an oxidation state of -1 to 0, which means it is being reduced. The element that is reduced in this reaction is iodine (I).