Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.) You may want to reference (Page) Section 20.2 while completing this problem. Part A Complete and balance the following equation: H2O2(aq)+ClO2(aq)→ClO2−(aq)+O2(g)(basic solution)Express your answer as a net chemical equation including phases. nothing

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dsdrajlin dsdrajlin · Answer 1 · 2020-04-16T03:07:33+02:00

Answer:

Oxidizing agent: ClO₂

Reducing agent: H₂O₂

2 ClO₂(aq) + H₂O₂(aq) → 2 ClO₂⁻(aq) + O₂(g) + 2 H⁺(aq)

Explanation:

In order to balance a redox reaction, we will use the ion-electron method.

Step 1: Identify both half-reactions

Reduction: ClO₂(aq) → ClO₂⁻(aq)

Oxidation: H₂O₂(aq) → O₂(g)

ClO₂ is reduced, so it is the oxidizing agent, while H₂O₂ is oxidized so it is the reducing agent.

Step 2: Perform the mass balance, adding H⁺ and H₂O where appropriate

ClO₂(aq) → ClO₂⁻(aq)

H₂O₂(aq) → O₂(g) + 2 H⁺

Step 3: Perform the charge balance, adding electrons where appropriate

1 e⁻ + ClO₂(aq) → ClO₂⁻(aq)

H₂O₂(aq) → O₂(g) + 2 H⁺(aq) + 2 e⁻

Step 4: Multiply both half-reactions by numbers that assure that the number of electrons gained and lost are equal, and add them

2 × [1 e⁻ + ClO₂(aq) → ClO₂⁻(aq)]

1 × [H₂O₂(aq) → O₂(g) + 2 H⁺(aq) + 2 e⁻]

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2 ClO₂(aq) + H₂O₂(aq) → 2 ClO₂⁻(aq) + O₂(g) + 2 H⁺(aq)