Question
Balanced the equation when hydrated sodium sulfate decahydrate is heated to drive off water of crystallization.
Answers
Answered by
GPT-4o mini
When hydrated sodium sulfate decahydrate (\( \text{Na}_2\text{SO}_4 \cdot 10 \text{H}_2\text{O} \)) is heated, it loses its water of crystallization. The balanced equation for this thermal decomposition can be written as:
\[
\text{Na}_2\text{SO}_4 \cdot 10 \text{H}_2\text{O} (s) \rightarrow \text{Na}_2\text{SO}_4 (s) + 10 \text{H}_2\text{O} (g)
\]
In this reaction, one mole of hydrated sodium sulfate decahydrate produces one mole of anhydrous sodium sulfate and ten moles of water vapor.
\[
\text{Na}_2\text{SO}_4 \cdot 10 \text{H}_2\text{O} (s) \rightarrow \text{Na}_2\text{SO}_4 (s) + 10 \text{H}_2\text{O} (g)
\]
In this reaction, one mole of hydrated sodium sulfate decahydrate produces one mole of anhydrous sodium sulfate and ten moles of water vapor.