Question

In the balanced redox reaction below:

Ba²⁺(aq)+ 2 OH⁻(aq) +H₂O₂(aq)+ 2 ClO₂(g)óBa(ClO₂)₂(s)+ 2 H₂O(l) +O₂(g)

A. Ba²⁺ is the oxidizing agent and H₂O₂ is the reducing agent
B. H₂O₂ is the oxidizing agent and ClO₂ is the reducing agent
C. ClO₂ is the oxidizing agent and Ba²⁺ isthe reducing agent
D. H₂O₂ is the oxidizing agent and Ba²⁺ is the reducing agent
E. ClO₂ is the oxidizing agent and H₂O₂ is the reducing agent

Answer 1

In the balanced redox reaction given, ClO₂ is the oxidizing agent as it is reduced, and H₂O₂ is the reducing agent as it is oxidized; hence, answer E is correct.

Step-by-step explanation:

In the given balanced redox reaction, we have the following species involved: Ba²⁺, OH⁻, H₂O₂, ClO₂, Ba(ClO₂)₂, H₂O, and O₂. To identify the oxidizing and reducing agents, we must look at the changes in oxidation states of the reactants and the products.

Hydrogen peroxide (H₂O₂) acts as the reducing agent because it gets oxidized during the reaction, losing electrons, as evidenced by oxygen going from a -1 oxidation state in H₂O₂ to a 0 oxidation state in O₂. Meanwhile, chlorine dioxide (ClO₂) is the oxidizing agent as it is reduced, gaining electrons during the reaction, evident by chlorine changing from a +4 to a +3 oxidation state in Ba(ClO₂)₂.

Barium ion (Ba²⁺) is not an oxidizing or reducing agent as it does not undergo a change in oxidation state; it remains as Ba²⁺ in Ba(ClO₂)₂. Therefore, the correct answer to the student's question is E. ClO₂ is the oxidizing agent and H₂O₂ is the reducing agent.