On heating a mixture containing 1 mole each of `Li_(2) CO_(3) and K_(2)CO_(3)`……..is / are formed .

Options

A. 2 moles of `CO_2`
B. 1 moles of `CO_2`
C. 1.5 moles of `CO_2`
D. No carbon dioxide

Answer

To solve the problem of what is formed when heating a mixture containing 1 mole each of \( \text{Li}_2\text{CO}_3 \) and \( \text{K}_2\text{CO}_3 \), we can analyze the thermal stability of each compound.

### Step-by-Step Solution:

1. **Identify the Compounds**: We have two compounds: lithium carbonate \( \text{Li}_2\text{CO}_3 \) and potassium carbonate \( \text{K}_2\text{CO}_3 \).

2. **Understand Thermal Decomposition**:
- **Lithium Carbonate**: When heated, lithium carbonate decomposes into lithium oxide and carbon dioxide:
\[ \text{Li}_2\text{CO}_3 \rightarrow \text{Li}_2\text{O} + \text{CO}_2 \]
- **Potassium Carbonate**: Potassium carbonate is more thermally stable and does not decompose upon heating:
\[ \text{K}_2\text{CO}_3 \text{ does not decompose.} \]

3. **Calculate Moles of Products**:
- From 1 mole of \( \text{Li}_2\text{CO}_3 \), we produce 1 mole of \( \text{CO}_2 \) (since 1 mole of \( \text{Li}_2\text{CO}_3 \) produces 1 mole of \( \text{CO}_2 \)).
- From 1 mole of \( \text{K}_2\text{CO}_3 \), there is no \( \text{CO}_2 \) produced.

4. **Total Products Formed**:
- The total amount of \( \text{CO}_2 \) produced from the mixture is 1 mole from \( \text{Li}_2\text{CO}_3 \) and 0 moles from \( \text{K}_2\text{CO}_3 \).
- Therefore, the total amount of \( \text{CO}_2 \) formed is:
\[ \text{Total } \text{CO}_2 = 1 \text{ mole} \]

5. **Final Answer**: The final answer to the question is that 1 mole of \( \text{CO}_2 \) is formed.