On heating a mixture containing 1 mol each of `Na_2CO_3` and `Li_2CO_3,`

Options

A. 2 mol of `CO_2` are formed
B. 1 mol of `CO_2` is formed
C. 1.5 mol of `CO_2` are formed
D. no`CO_2` is formed

Answer

To solve the question of how many moles of CO2 will be produced when heating a mixture of 1 mole each of Na2CO3 and Li2CO3, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Compounds**:
- We have two carbonates: Sodium carbonate (Na2CO3) and Lithium carbonate (Li2CO3).
- Sodium carbonate is stable and does not decompose upon heating, while lithium carbonate is unstable and decomposes.

2. **Decomposition of Lithium Carbonate**:
- When Li2CO3 is heated, it decomposes into lithium oxide (Li2O) and carbon dioxide (CO2).
- The reaction can be represented as:
\[ \text{Li}_2\text{CO}_3 \rightarrow \text{Li}_2\text{O} + \text{CO}_2 \]
- From this reaction, we see that 1 mole of Li2CO3 produces 1 mole of CO2.

3. **Behavior of Sodium Carbonate**:
- Sodium carbonate (Na2CO3) does not decompose upon heating. Therefore, it does not produce any CO2.
- The reaction for Na2CO3 can be represented as:
\[ \text{Na}_2\text{CO}_3 \text{ (no decomposition)} \]

4. **Total CO2 Produced**:
- From the heating of 1 mole of Li2CO3, we get 1 mole of CO2.
- From the heating of 1 mole of Na2CO3, we get 0 moles of CO2.
- Therefore, the total moles of CO2 produced from the mixture is:
\[ 1 \text{ mole (from Li2CO3)} + 0 \text{ moles (from Na2CO3)} = 1 \text{ mole of CO2} \]

5. **Conclusion**:
- The total amount of CO2 produced from heating the mixture of 1 mole each of Na2CO3 and Li2CO3 is 1 mole.

### Final Answer:
1 mole of CO2 is produced.

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