Moles of` KCIO_3` required for producing sufficient `O_2` to react with` 1` mole of aluminium will be (Molar mass of `KCIO_3 = 122.5`)

Options

A. 2 mole
B. 1 mole
C. 1/2 mole
D. 3/2 mole

Answer

To solve the problem, we need to determine how many moles of potassium chlorate (KClO₃) are required to produce enough oxygen (O₂) to react with 1 mole of aluminum (Al).

### Step-by-Step Solution:

1. **Write the balanced chemical equation for the decomposition of KClO₃:**
The decomposition of potassium chlorate can be represented as:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]
This equation shows that 2 moles of KClO₃ produce 3 moles of O₂.

2. **Determine the amount of O₂ needed for 1 mole of Al:**
The reaction between aluminum and oxygen to form aluminum oxide (Al₂O₃) can be represented as:
\[ 4 \text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3 \]
From this balanced equation, we see that 4 moles of Al react with 3 moles of O₂. Therefore, 1 mole of Al will react with:
\[ \frac{3}{4} \text{ moles of O}_2 = 1.5 \text{ moles of O}_2 \]

3. **Calculate the moles of KClO₃ required to produce 1.5 moles of O₂:**
From the first balanced equation, we know that:
- 2 moles of KClO₃ produce 3 moles of O₂.
To find out how many moles of KClO₃ are needed to produce 1.5 moles of O₂, we set up a proportion:
\[ \frac{2 \text{ moles KClO}_3}{3 \text{ moles O}_2} = \frac{x \text{ moles KClO}_3}{1.5 \text{ moles O}_2} \]
Cross-multiplying gives:
\[ 2 \times 1.5 = 3x \implies 3 = 3x \implies x = 1 \]
Therefore, 1 mole of KClO₃ is required to produce enough O₂ to react with 1 mole of Al.

4. **Conclusion:**
The moles of KClO₃ required to produce sufficient O₂ to react with 1 mole of aluminum is **1 mole**.

### Final Answer:
1 mole of KClO₃ is required.