1 mole of equimolar mixture of `Fe_(2)(C_(2)O_(4))_(3)` and `FeC_(2)O_(4)` required X moles of `KMnO_(4)` in acid medium for complete reaction. The value of X is:

Options

A. `0.9`
B. `0.6`
C. `1.2`
D. `0.8`

Answer

To solve the problem, we need to determine how many moles of KMnO4 are required to react with 1 mole of an equimolar mixture of Fe2(C2O4)3 and FeC2O4 in an acidic medium.

### Step-by-Step Solution:

1. **Identify the Moles of Each Compound:**
Since we have an equimolar mixture of Fe2(C2O4)3 and FeC2O4, we can assume:
- Moles of Fe2(C2O4)3 = 0.5 moles
- Moles of FeC2O4 = 0.5 moles

2. **Write the Reactions:**
- For Fe2(C2O4)3:
\[ \text{Fe}_2(\text{C}_2\text{O}_4)_3 + 6 \text{KMnO}_4 + 12 \text{H}^+ \rightarrow 2 \text{Fe}^{3+} + 6 \text{CO}_2 + 6 \text{Mn}^{2+} + 6 \text{H}_2\text{O} \]
Here, 6 moles of KMnO4 are required for 1 mole of Fe2(C2O4)3.

- For FeC2O4:
\[ \text{FeC}_2\text{O}_4 + 2 \text{KMnO}_4 + 8 \text{H}^+ \rightarrow \text{Fe}^{3+} + 2 \text{CO}_2 + 2 \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]
Here, 2 moles of KMnO4 are required for 1 mole of FeC2O4.

3. **Calculate the Total Moles of KMnO4 Required:**
- For 0.5 moles of Fe2(C2O4)3:
\[ 0.5 \text{ moles} \times 6 \text{ moles of KMnO}_4 = 3 \text{ moles of KMnO}_4 \]
- For 0.5 moles of FeC2O4:
\[ 0.5 \text{ moles} \times 2 \text{ moles of KMnO}_4 = 1 \text{ mole of KMnO}_4 \]

4. **Add the Moles of KMnO4 Together:**
\[ \text{Total KMnO}_4 = 3 + 1 = 4 \text{ moles of KMnO}_4 \]

5. **Calculate the Value of X:**
Since we need to find the total moles of KMnO4 required for the complete reaction, we have:
\[ X = 4 \text{ moles} \]

### Final Answer:
The value of X is 4.