- Formation of bromine from bromide. Assign oxidation numbers to each atom. Identify the oxidizing agent and the reducing agent.Chemical Equation: \[ 2 \text{Br}^-(\text{aq}) + \text{MnO}_2(\text{s}) + 4 \text{H}^+(\text{aq}) \rightarrow \text{Br}_2(\text{s}) + \text{Mn}^{2+}(\text{aq}) + 2 \text{H}_2\text{O}(\text{l}) \] ### ExplanationIn this reaction:1. **Oxidation Numbers:** - Bromine: Changes from -1 in Br⁻ to 0 in Br₂. - Manganese: Changes from +4 in MnO₂ to +2 in Mn²⁺.2. **Agents:** - Oxidizing Agent: MnO₂ (since Mn is reduced from +4 to +2). - Reducing Agent: Br⁻ (since Br is oxidized from -1 to 0).

The given reaction is: 2Br1- + MnO2 + 4H1+ → Br2 + Mn2+ + 2H2O

Answered: Formation of bromine from bromide.…

Formation of bromine from bromide. Assign oxidation numbers to each atom. Identify the oxidizing agent and the reducing agent. 2 Br!-(aq) + Mn02(s)+ 4 H1+ (aq) → Br2(s) + Mn² * (aq) + 2 H20(1)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

- Formation of bromine from bromide.

Assign oxidation numbers to each atom.

Identify the oxidizing agent and the reducing agent.

Chemical Equation:

\[ 2 \text{Br}^-(\text{aq}) + \text{MnO}_2(\text{s}) + 4 \text{H}^+(\text{aq}) \rightarrow \text{Br}_2(\text{s}) + \text{Mn}^{2+}(\text{aq}) + 2 \text{H}_2\text{O}(\text{l}) \]

### Explanation
In this reaction:

1. **Oxidation Numbers:**
- Bromine: Changes from -1 in Br⁻ to 0 in Br₂.
- Manganese: Changes from +4 in MnO₂ to +2 in Mn²⁺.

2. **Agents:**
- Oxidizing Agent: MnO₂ (since Mn is reduced from +4 to +2).
- Reducing Agent: Br⁻ (since Br is oxidized from -1 to 0).

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