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

a. Mn

b. Cl

c. O

d. H

Respuesta :

shelovesdeedee

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

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: Option (a) is the correct answer.

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, [tex]MnO_{2} + HCl \rightarrow H_{2}O + MnCl_{2} + Cl_{2}[/tex]

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.

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