a) Cr.0,2- + Fe* → Fe3* + Cr3+ (in acidic solution) b) Mn* + BiO3 → MnOq¯ + Bi³* (in acidic solution) c) HSO3 + MnO4¯ → HSO4¯+ Mn²* (in acidic solution)

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### Oxidation Number Assignment and Equation Balancing

1. **Objective**: Assign oxidation numbers to each element in the following reactions and balance the equations.

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#### a) Reaction in Acidic Solution
\[ \text{Cr}_2\text{O}_7^{2-} + \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + \text{Cr}^{3+} \]

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#### b) Reaction in Acidic Solution
\[ \text{Mn}^{2+} + \text{BiO}_3^- \rightarrow \text{MnO}_4^- + \text{Bi}^{3+} \]

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#### c) Reaction in Acidic Solution
\[ \text{HSO}_3^- + \text{MnO}_4^- \rightarrow \text{HSO}_4^- + \text{Mn}^{2+} \]

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#### d) Reaction in Basic Solution
\[ \text{H}_2\text{O}_2 + \text{ClO}_2 \rightarrow \text{ClO}_2^- + \text{O}_2 \]

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#### e) Reaction in Basic Solution
\[ \text{Cl}_2 \rightarrow \text{ClO}_2^- + \text{Cl}^- \]

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#### f) Reaction in Acidic Solution
\[ \text{MnO}_4^- + \text{H}_2\text{C}_2\text{O}_4 \rightarrow \text{CO}_2 + \text{Mn}^{2+} \]

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### Explanation for Students
- **Oxidation Numbers**: Determine the oxidation state of each element in the reactants and products.
- **Balancing Equations**: Ensure that atoms and charges are balanced on both sides of the equation, considering the medium (acidic or basic).
- **Acidic and Basic Solutions**: Note that balancing may require adding H⁺ in acidic solutions and OH⁻ in basic solutions to achieve a balance in hydrogen and oxygen atoms.
Transcribed Image Text:### Oxidation Number Assignment and Equation Balancing 1. **Objective**: Assign oxidation numbers to each element in the following reactions and balance the equations. --- #### a) Reaction in Acidic Solution \[ \text{Cr}_2\text{O}_7^{2-} + \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + \text{Cr}^{3+} \] --- #### b) Reaction in Acidic Solution \[ \text{Mn}^{2+} + \text{BiO}_3^- \rightarrow \text{MnO}_4^- + \text{Bi}^{3+} \] --- #### c) Reaction in Acidic Solution \[ \text{HSO}_3^- + \text{MnO}_4^- \rightarrow \text{HSO}_4^- + \text{Mn}^{2+} \] --- #### d) Reaction in Basic Solution \[ \text{H}_2\text{O}_2 + \text{ClO}_2 \rightarrow \text{ClO}_2^- + \text{O}_2 \] --- #### e) Reaction in Basic Solution \[ \text{Cl}_2 \rightarrow \text{ClO}_2^- + \text{Cl}^- \] --- #### f) Reaction in Acidic Solution \[ \text{MnO}_4^- + \text{H}_2\text{C}_2\text{O}_4 \rightarrow \text{CO}_2 + \text{Mn}^{2+} \] --- ### Explanation for Students - **Oxidation Numbers**: Determine the oxidation state of each element in the reactants and products. - **Balancing Equations**: Ensure that atoms and charges are balanced on both sides of the equation, considering the medium (acidic or basic). - **Acidic and Basic Solutions**: Note that balancing may require adding H⁺ in acidic solutions and OH⁻ in basic solutions to achieve a balance in hydrogen and oxygen atoms.
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