1 mole of equimolar mixture of ferric oxalate and ferrous oxalate requres x mole of `KMnO_(4)` in acidic medium for complete oxidation. X is:

Options

A. 0.5 mole
B. 0.9 mole
C. 1.2 mole
D. 4.5 mole

Answer

To solve the problem of how many moles of KMnO4 are required for the complete oxidation of 1 mole of an equimolar mixture of ferric oxalate (Fe2(C2O4)3) and ferrous oxalate (FeC2O4), we can follow these steps:

### Step 1: Identify the components and their n-factors
1. **Ferric oxalate (Fe2(C2O4)3)**:
- Each molecule contains 6 carbon atoms (3 C2O4 groups).
- The oxidation state of carbon in oxalate (C2O4) goes from +3 to +4 when oxidized to CO2.
- Therefore, the total change in oxidation state for 6 carbon atoms is 6 (1 electron change per carbon).
- Hence, the n-factor for ferric oxalate is **6**.

2. **Ferrous oxalate (FeC2O4)**:
- Each molecule contains 2 carbon atoms.
- The oxidation state of iron changes from +2 to +3 (1 electron change).
- The oxidation state of carbon also changes from +3 to +4 (1 electron change per carbon).
- Therefore, the total change in oxidation state is 1 (for Fe) + 2 (for 2 carbon atoms) = **3**.
- Hence, the n-factor for ferrous oxalate is **3**.

### Step 2: Calculate the equivalence of each component
- Since we have an equimolar mixture, we have:
- 0.5 moles of ferric oxalate (Fe2(C2O4)3)
- 0.5 moles of ferrous oxalate (FeC2O4)

- The equivalence of ferric oxalate:
\[ \text{Equivalence of Fe2(C2O4)3} = \text{moles} \times \text{n-factor} = 0.5 \times 6 = 3 \]

- The equivalence of ferrous oxalate:
\[ \text{Equivalence of FeC2O4} = \text{moles} \times \text{n-factor} = 0.5 \times 3 = 1.5 \]

### Step 3: Total equivalence of the mixture
- Total equivalence of the mixture:
\[ \text{Total equivalence} = 3 + 1.5 = 4.5 \]

### Step 4: Relate to KMnO4
- The n-factor for KMnO4 in acidic medium is **5** (as it reduces from +7 to +2).
- Let \( x \) be the number of moles of KMnO4 required.

- The equivalence of KMnO4:
\[ \text{Equivalence of KMnO4} = x \times 5 \]

### Step 5: Set up the equation
- Setting the total equivalence of the mixture equal to the equivalence of KMnO4:
\[ 4.5 = 5x \]

### Step 6: Solve for \( x \)
- Rearranging gives:
\[ x = \frac{4.5}{5} = 0.9 \]

Thus, the number of moles of KMnO4 required for the complete oxidation of the mixture is **0.9 moles**.

### Final Answer:
**X = 0.9 moles of KMnO4**

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