How many moles of electrons are being transferred in the following reaction?

5H2C2O4(aq) + 2MnO4-(aq) + 6H+(aq) --> 2Mn2+(aq) + 10CO2(g) + 8H2O(l)








To determine how many moles of electrons are transferred in the reaction, we need to look at the oxidation states of the atoms involved, particularly for the elements that are being oxidized and reduced.

### Step 1: Identify the elements being oxidized and reduced
- **Oxalate ion (C₂O₄²⁻)**: Carbon is the element of interest here. In oxalate (C₂O₄²⁻), the oxidation state of each carbon is +3. In carbon dioxide (CO₂), the oxidation state of each carbon is +4. This means that the carbon in oxalate is **oxidized** (loses electrons) from +3 to +4.
  
- **Permanganate ion (MnO₄⁻)**: Manganese is the element of interest. In permanganate (MnO₄⁻), the oxidation state of manganese is +7. In the product Mn²⁺, the oxidation state of manganese is +2. This means that manganese is **reduced** (gains electrons) from +7 to +2.

### Step 2: Determine how many electrons are transferred in oxidation and reduction
- **Oxidation (C in C₂O₄²⁻ to CO₂)**: Each carbon in oxalate is oxidized from +3 to +4. The change in oxidation state for one carbon atom is 1 electron. Since there are 2 carbon atoms in oxalate, each oxalate ion loses 2 electrons. The reaction involves 5 oxalate ions, so the total electrons lost are:
  
  \[
  5 \text{ oxalate ions} \times 2 \text{ electrons per oxalate} = 10 \text{ electrons lost}
  \]

- **Reduction (Mn in MnO₄⁻ to Mn²⁺)**: Manganese is reduced from +7 to +2, meaning each manganese atom gains 5 electrons. Since 2 permanganate ions are reduced, the total electrons gained are:
  
  \[
  2 \text{ permanganate ions} \times 5 \text{ electrons per permanganate} = 10 \text{ electrons gained}
  \]

### Step 3: Conclusion
Since both oxidation and reduction involve the transfer of 10 electrons, the total number of **moles of electrons transferred** in the reaction is:

\[
\boxed{10 \text{ moles of electrons}}
\]

Would you like more details on any part of the solution? Here are some related questions to explore:

1. How do you determine oxidation states in compounds?
2. Why is manganese reduced while carbon is oxidized?
3. What is the role of \( \text{H}^+ \) in this redox reaction?
4. Can you explain the concept of half-reactions in redox chemistry?
5. How can you balance redox reactions in acidic or basic solutions?

**Tip:** When balancing redox reactions, always check the oxidation states of atoms before and after the reaction to ensure electron transfer is accounted for.

How many moles of electrons are being transferred in the following reaction? 5H2C2O4(aq) + 2MnO4-(aq) + 6H+(aq) --> 2Mn2+(aq) + 10CO2(g) + 8H2O(l)

Explore how to determine the moles of electrons transferred in a redox reaction. This solution covers the oxidation and reduction processes, including changes in oxidation states of carbon and manganese. Perfect for students in Grades 10-12 studying chemistry.

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