Question

Given the reaction:
4 HCl(aq) + MnO2(s) MnCl2(aq) + 2 H2O() + Cl2(g)
The manganese is

A) reduced and its oxidation number changes from +4 to +2
B) reduced and its oxidation number changes from +2 to +4
C) oxidized and its oxidation number changes from +4 to +2
D) oxidized and its oxidation number changes from +2 to +4

Answer 1

Redox is the oxidation-reduction reaction that includes the gain and loss of electrons. The oxidation of the manganese changes from +4 to +2  and gets reduced.

What are oxidation and reduction?

In a redox reaction, the electrons are gained and lost by the chemical species. In oxidation, the electrons are lost by the species to another, while in reduction the electrons are gained by the species.

When the electrons are lost by the species their oxidation number gets increased, whereas when the species gains electrons their oxidation state decreases.

The oxidation number of manganese oxide and manganese(II) chloride is calculated as:

$\begin{aligned}\rm Mn^{x}O_{2}^{2-}: \rm x -4 &= 0\\\\&= +4\end{aligned}$

and,

$\begin{aligned}\rm Mn^{x}Cl^{2-}: x -2 &= 0\\\\&= +2\end{aligned}$

Therefore, the manganese is option A. reduced, and the oxidation number changes from +4 to +2.

Learn more about oxidation numbers here:

https://brainly.com/question/25673335

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