During the preparation of Plaster of Paris, Gypsum is carefully heated to . If of Gypsum () undergo — s Block Elements Chemistry Question
Question
During the preparation of Plaster of Paris, Gypsum is carefully heated to $393\text{ K}$. If $2 \text{ moles}$ of Gypsum ($CaSO_4 \cdot 2H_2O$) undergo this ideal decomposition, what is the total number of moles of water ($H_2O$) released as vapor?
Answer: 3
💡 Solution & Explanation
The balanced decomposition reaction is: $2(CaSO_4 \cdot 2H_2O) \xrightarrow{393 K} 2(CaSO_4) \cdot H_2O + 3H_2O \uparrow$ (or equivalently $CaSO_4 \cdot \frac{1}{2}H_2O$). From the stoichiometry, heating 2 moles of gypsum releases 3 moles of water.
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