`KClO_(3) to KCl + O_(2)`(unbalanced),
If in above reaction 5 moles of `KClO_(3)` was heated, then find moles
of `O_(2)` produced on completion of reaction.

Answer

To solve the problem, we will follow these steps:

### Step 1: Write the unbalanced chemical equation
The unbalanced reaction is:
\[ \text{KClO}_3 \rightarrow \text{KCl} + \text{O}_2 \]

### Step 2: Balance the chemical equation
To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation.

1. **Potassium (K)**: There is 1 K on the left (in KClO3) and 1 K on the right (in KCl). So, K is balanced.
2. **Chlorine (Cl)**: There is 1 Cl on the left (in KClO3) and 1 Cl on the right (in KCl). So, Cl is balanced.
3. **Oxygen (O)**: There are 3 O on the left (in KClO3) and 2 O on the right (in O2).

To balance the oxygen, we can find a common multiple of 3 and 2, which is 6.

- To get 6 O on the left, we need 2 KClO3:
\[ 2 \text{KClO}_3 \rightarrow \text{KCl} + \text{O}_2 \]
- This gives us 6 O on the left (2 x 3 = 6).
- To get 6 O on the right, we need 3 O2:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]

Now, the balanced equation is:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]

### Step 3: Determine the mole ratio
From the balanced equation, we see that:
- 2 moles of KClO3 produce 3 moles of O2.

### Step 4: Calculate moles of O2 produced from 5 moles of KClO3
Using the mole ratio from the balanced equation:
- If 2 moles of KClO3 produce 3 moles of O2, then 1 mole of KClO3 produces \( \frac{3}{2} \) moles of O2.
- Therefore, 5 moles of KClO3 will produce:
\[ \text{Moles of O}_2 = 5 \times \frac{3}{2} = \frac{15}{2} = 7.5 \text{ moles of O}_2 \]

### Final Answer
Thus, when 5 moles of KClO3 are heated, 7.5 moles of O2 are produced.

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