Question

In the unbalanced equation below, what element is being reduced? MnO2 + HCl → H2O + MnCl2 + Cl2

a. Mn

b. Cl

c. O

d. H

Answer 1

Manganese is reduced from MnIV+ to MnII+, so option A.

Step-by-step explanation:

And of course, for every reduction there is a corresponding oxidation: here, chloride ion is oxidized to zerovalent chlorine gas.

The overall (balanced) redox equation is:

MnO2(s)+4HCl(aq)→MnCl2(s)+Cl2(g)+2H2O(l)

Answer 2

Answer: Option (a) is the correct answer.

Step-by-step explanation:

Reduction is a process in which there is loss of oxygen atom from a molecule. Also in reduction there is a decrease in oxidation state of the metal.

Whereas in oxidation process there is gain of oxygen atom.

In the given reaction,
`MnO_(2) + HCl \rightarrow H_(2)O + MnCl_(2) + Cl_(2)`

Here, oxidation state of manganese reduces from +4 to +2 and also there in loss of oxygen form manganese oxide molecule to form manganese chloride.

Thus, we can conclude that Mn has been reduced.