KMnO₄ + FeSO₄ + H₂SO₄ → Mnso4 + Fe2 (So4,)5 + H₂O

It looks like you want to balance the given redox reaction involving potassium permanganate (\( \text{KMnO}_4 \)), iron(II) sulfate (\( \text{FeSO}_4 \)), and sulfuric acid (\( \text{H}_2\text{SO}_4 \)):

**Unbalanced Reaction:**

\[
\text{KMnO}_4 + \text{FeSO}_4 + \text{H}_2\text{SO}_4 \rightarrow \text{MnSO}_4 + \text{Fe}_2(\text{SO}_4)_3 + \text{H}_2\text{O}
\]

### Steps to Balance the Reaction:

1. **Identify the oxidation states** of the elements that are undergoing oxidation and reduction.
   
   - Manganese in \( \text{KMnO}_4 \) is in the +7 oxidation state and is reduced to +2 in \( \text{MnSO}_4 \).
   - Iron in \( \text{FeSO}_4 \) is in the +2 oxidation state and is oxidized to +3 in \( \text{Fe}_2(\text{SO}_4)_3 \).

2. **Write the half-reactions** for oxidation and reduction:
   
   - Reduction (Mn): \( \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \)
   - Oxidation (Fe): \( \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} \)

3. **Balance the half-reactions** for mass and charge.

   - Reduction half-reaction:
     \[
     \text{MnO}_4^- + 8\text{H}^+ + 5\text{e}^- \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O}
     \]

   - Oxidation half-reaction:
     \[
     \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + \text{e}^-
     \]

4. **Balance the electrons** between the two half-reactions by multiplying the oxidation half-reaction by 5 so the electrons cancel:

   - Oxidation half-reaction multiplied by 5:
     \[
     5\text{Fe}^{2+} \rightarrow 5\text{Fe}^{3+} + 5\text{e}^-
     \]

5. **Combine the half-reactions:**

   \[
   \text{MnO}_4^- + 8\text{H}^+ + 5\text{Fe}^{2+} \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O} + 5\text{Fe}^{3+}
   \]

6. **Add the sulfate ions** (\( \text{SO}_4^{2-} \)) to balance the compounds:

   \[
   \text{MnO}_4^- + 5\text{FeSO}_4 + 8\text{H}_2\text{SO}_4 \rightarrow \text{MnSO}_4 + 5\text{Fe}_2(\text{SO}_4)_3 + 4\text{H}_2\text{O}
   \]

### Balanced Equation:

\[
\text{KMnO}_4 + 5\text{FeSO}_4 + 3\text{H}_2\text{SO}_4 \rightarrow \text{MnSO}_4 + 5\text{Fe}_2(\text{SO}_4)_3 + \text{K}_2\text{SO}_4 + 8\text{H}_2\text{O}
\]

Would you like further details or have any questions?

### Related Questions:

1. How do you determine the oxidation states of elements in a compound?
2. What are the rules for balancing redox reactions in acidic solutions?
3. How can you balance redox reactions in basic solutions?
4. What is the significance of balancing half-reactions separately in redox reactions?
5. How does the presence of acidic or basic medium affect redox reactions?

### Tip:
Always balance the atoms other than oxygen and hydrogen first, then balance oxygen atoms by adding \( \text{H}_2\text{O} \) molecules, and balance hydrogen atoms by adding \( \text{H}^+ \) ions in acidic solutions.

KMnO₄ + FeSO₄ + H₂SO₄ → MnSO₄ + Fe₂(SO₄)₃ + H₂O

Learn how to balance the redox reaction between potassium permanganate, iron(II) sulfate, and sulfuric acid in an acidic medium. This problem covers key chemistry concepts such as oxidation states, redox reactions, and balancing chemical equations. Suitable for students in Grades 10-12.

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