Question

Which of the following is correct about the oxidation in the given equation?

$Zn\left(s\right)+2HCl\left(aq\right)\to ZnC{l}_2\left(aq\right)+H_2\left(g\right)$

• A. Zinc is oxidized
• B. Chlorine is oxidized
• C. Hydrogen is oxidized
• D. Zinc is reduced

Answer 1

The correct option is A Zinc is oxidized

The oxidation number of atom in an elemental state is zero, so zinc has 0 oxidation state in reactant side. Whereas on the product side it has oxidation state +2.

$ZnC{l}_2$ = X +2(-1) = 0

X - 2 = 0

X = +2

Hence, the oxidation state increases.

Hydrogen is reduced in the reaction. The +1 charge on each reactant hydrogen ion is reduced to 0 when it becomes $H_2$ molecule.

There is no change in the oxidation state of chlorine.