Question

In the redox reaction \[ \text{MnO}_4^- + \text{C}_2\text{O}_4^{2-} \to \text{Mn}^{2+} + \text{CO}_2 + \text{H}_2\text{O} \] The correct coefficients of \( \text{C}_2\text{O}_4^{2-} \) and \( \text{H}^+ \) are

• A. 5, 8
• B. 5, 4
• C. 2, 3
• D. 2, 1

Hint:

For redox reactions, balance the atoms and charges on both sides by adjusting coefficients, paying attention to the oxidation states of elements involved.

Answer 1

The Correct Option is B

Balancing the redox reaction involves ensuring the number of atoms and the charges are equal on both sides.
The oxidation state of manganese in \( \text{MnO}_4^- \) is +7, and it is reduced to +2 in \( \text{Mn}^{2+} \).
The number of electrons transferred is 5.
Similarly, the oxalate ion \( \text{C}_2\text{O}_4^{2-} \) is oxidized to \( \text{CO}_2 \), requiring 4 protons (\( \text{H}^+ \)) to balance the equation.
Thus, the correct coefficients for \( \text{C}_2\text{O}_4^{2-} \) and \( \text{H}^+ \) are 5 and 4, respectively.