Question

What is the number of electrons transferred considering Mn when \( \text{KMnO}_4 \) is converted into \( \text{Mn}_2\text{O}_3 \)?

• A. 3
• B. 4
• C. 5
• D. 6

Hint:

The number of electrons transferred can be calculated by comparing the oxidation states of the metal in both the reactant and the product.

Answer 1

The Correct Option is C

Step 1: Understanding the Question:
We need to find the change in the oxidation state of Manganese (Mn) when it transforms from \( \text{KMnO}_4 \) to \( \text{Mn}_2\text{O}_3 \). This change corresponds to the number of electrons transferred per atom of Mn.
Step 2: Key Formula or Approach:
Calculate the oxidation state of Mn in both compounds using the rule that the sum of oxidation states in a neutral molecule is zero.
Step 3: Detailed Explanation:
1. In \( \text{KMnO}_4 \):
Let the oxidation state of Mn be \( x \).
Potassium (K) is \( +1 \), and Oxygen (O) is \( -2 \).
\( (+1) + x + 4(-2) = 0 \)
\( x - 7 = 0 \Rightarrow x = +7 \).
2. In \( \text{Mn}_2\text{O}_3 \):
Let the oxidation state of Mn be \( y \).
\( 2(y) + 3(-2) = 0 \)
\( 2y - 6 = 0 \Rightarrow y = +3 \).
The difference in oxidation states is \( (+7) - (+3) = 4 \).
This indicates that each Mn atom gains 4 electrons.
Step 4: Final Answer:
The number of electrons transferred per Mn atom is 4.