Question

In the reaction \( \text{Zn(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu(s)} \), what is the oxidation state of zinc in the products?}

• A. \( +2 \)
• B. \( +1 \)
• C. \( 0 \)
• D. \( -2 \)

Hint:

In redox reactions, oxidation corresponds to an increase in oxidation state, while reduction corresponds to a decrease in oxidation state. Always identify the oxidation states of elements in both reactants and products to determine the changes.

Answer 1

The Correct Option is A

The reaction provided is: \[ \text{Zn(s)} + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu(s)} \] 1. Oxidation state identification: - Zn(s): Zinc is in its elemental state, oxidation state is \( 0 \). - Cu\(^{2+}\)(aq): Copper's oxidation state is \( +2 \). 2. Oxidation and reduction processes: - Zinc is oxidized from \( 0 \) to \( +2 \). - Copper is reduced from \( +2 \) to \( 0 \). 3. Zinc's oxidation state in the product: - In the product, Zn\(^{2+}\)(aq), zinc exhibits an oxidation state of \( +2 \). Consequently, the oxidation state of zinc in the products is \( +2 \).