Ask a New Question
Menu

Zn (s) + 2HCl (aq) → ZnCl₂ (aq) + H₂ (g) Which elements are oxidized and reduced in the reaction?

A. Zinc (Zn) is oxidized, and hydrogen (H) is reduced.
B. Hydrogen (H) is oxidized, and chlorine (Cl) is reduced.
C. Zinc (Zn) is reduced, and hydrogen (H) is oxidized.
D. Chlorine (Cl) is oxidized, and zinc (Zn) is reduced.

1 answer

In the reaction:

\[ \text{Zn (s) + 2HCl (aq) → ZnCl}_2 \text{ (aq) + H}_2 \text{ (g)} \]

we can analyze the oxidation states of the involved elements to determine which are oxidized and which are reduced.

  1. Zinc (Zn) starts as an elemental solid with an oxidation state of 0 and is transformed into \( \text{ZnCl}_2 \), where the oxidation state of zinc is +2. Since zinc is losing electrons, it is being oxidized.

  2. Hydrogen (H) in hydrochloric acid (HCl) has an oxidation state of +1. In the product \( H_2 \), the oxidation state of hydrogen is 0, as it is in its elemental form. Since hydrogen is gaining electrons, it is being reduced.

So, we can conclude:

  • Zinc (Zn) is oxidized (oxidation state increases from 0 to +2).
  • Hydrogen (H) is reduced (oxidation state decreases from +1 to 0).

Therefore, the correct answer is:

A. Zinc (Zn) is oxidized, and hydrogen (H) is reduced.