When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? Mn²+ I₂ + MnO₂→ 103 + Water appears in the balanced equation as a for neither.) How many electrons are transferred in this reaction? (reactant, product, neither) with a coefficient of . (Enter 0

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### Balancing Redox Reactions

#### Problem Statement

When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown?

\[ \square \, \text{I}_2 + \square \, \text{MnO}_2 \rightarrow \square \, \text{IO}_3^- + \square \, \text{Mn}^{2+} \]

**Questions:**

1. Water appears in the balanced equation as a _______ (reactant, product, neither) with a coefficient of _______. (Enter 0 for neither.)

2. How many electrons are transferred in this reaction? _______ 

#### Explanation

To solve this problem:

- **Balancing Steps:** Break down the redox reaction into oxidation and reduction half-reactions. Balance each half-reaction for both mass and charge, considering the acidic conditions that may involve adding \(\text{H}^+\) and \(\text{H}_2\text{O}\).
- **Combine Half-Reactions:** Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction. Adjust coefficients accordingly.
- **Determine Water's Role:** Analyze the balanced equation to identify if water appears as a reactant, product, or not at all.
- **Calculate Electrons Transferred:** Count the total number of electrons that are transferred in the redox process.

This exercise aids in understanding how to balance chemical equations and the conservation of mass and charge in reactions, particularly under acidic conditions.
Transcribed Image Text:### Balancing Redox Reactions #### Problem Statement When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? \[ \square \, \text{I}_2 + \square \, \text{MnO}_2 \rightarrow \square \, \text{IO}_3^- + \square \, \text{Mn}^{2+} \] **Questions:** 1. Water appears in the balanced equation as a _______ (reactant, product, neither) with a coefficient of _______. (Enter 0 for neither.) 2. How many electrons are transferred in this reaction? _______ #### Explanation To solve this problem: - **Balancing Steps:** Break down the redox reaction into oxidation and reduction half-reactions. Balance each half-reaction for both mass and charge, considering the acidic conditions that may involve adding \(\text{H}^+\) and \(\text{H}_2\text{O}\). - **Combine Half-Reactions:** Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction. Adjust coefficients accordingly. - **Determine Water's Role:** Analyze the balanced equation to identify if water appears as a reactant, product, or not at all. - **Calculate Electrons Transferred:** Count the total number of electrons that are transferred in the redox process. This exercise aids in understanding how to balance chemical equations and the conservation of mass and charge in reactions, particularly under acidic conditions.
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