For the following redox reaction, write a balanced equation for the whole reaction and include the states of matter: MnO4 (aq) + CI (aq) Balanced equation: palette. 2+ Mn²+ (aq) + Cl₂(g) (in acidic solution)

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**Redox Reaction Balancing**

For the following redox reaction, write a balanced equation for the whole reaction and include the states of matter:

\[ \text{MnO}_4^- \, (\text{aq}) + \text{Cl}^- \, (\text{aq}) \rightarrow \text{Mn}^{2+} \, (\text{aq}) + \text{Cl}_2 \, (\text{g}) \] 

*(in acidic solution)*

**Balanced equation:**

\[ \boxed{} \rightarrow \boxed{} \]

**Explanation:**  
This exercise requires balancing a redox reaction occurring in an acidic solution. The reactants and products are given with their respective states of matter:

- \(\text{MnO}_4^-\) is in aqueous form (\(\text{aq}\)).
- \(\text{Cl}^-\) is in aqueous form (\(\text{aq}\)).
- \(\text{Mn}^{2+}\) is the product in aqueous form (\(\text{aq}\)).
- \(\text{Cl}_2\) is released as a gas (\(\text{g}\)).

The objective is to find the stoichiometric coefficients to balance both mass and charge for the entire reaction.
Transcribed Image Text:**Redox Reaction Balancing** For the following redox reaction, write a balanced equation for the whole reaction and include the states of matter: \[ \text{MnO}_4^- \, (\text{aq}) + \text{Cl}^- \, (\text{aq}) \rightarrow \text{Mn}^{2+} \, (\text{aq}) + \text{Cl}_2 \, (\text{g}) \] *(in acidic solution)* **Balanced equation:** \[ \boxed{} \rightarrow \boxed{} \] **Explanation:** This exercise requires balancing a redox reaction occurring in an acidic solution. The reactants and products are given with their respective states of matter: - \(\text{MnO}_4^-\) is in aqueous form (\(\text{aq}\)). - \(\text{Cl}^-\) is in aqueous form (\(\text{aq}\)). - \(\text{Mn}^{2+}\) is the product in aqueous form (\(\text{aq}\)). - \(\text{Cl}_2\) is released as a gas (\(\text{g}\)). The objective is to find the stoichiometric coefficients to balance both mass and charge for the entire reaction.
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