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

$Z n (s) + 2 H C l (a q) \to Z n C l_{2} (a q) + H_{2} (g)$

Hydrogen is oxidized

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Zinc is reduced

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Zinc is oxidized

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Chlorine is oxidized

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Solution

The correct option is C 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.
$Z n C l_{2}$ = 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.

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