When exactly of pure Gypsum () are heated carefully in a kiln to , how many moles of water vapor () — s Block Elements Chemistry Question
Question
When exactly $2 \text{ moles}$ of pure Gypsum ($CaSO_4 \cdot 2H_2O$) are heated carefully in a kiln to $393\text{ K}$, how many moles of water vapor ($H_2O$) are evolved in the process?
Answer: 3
💡 Solution & Explanation
The balanced chemical equation for the formation of Plaster of Paris is: $2(CaSO_4 \cdot 2H_2O) \xrightarrow{393 K} 2(CaSO_4) \cdot H_2O + 3H_2O \uparrow$. Thus, from 2 moles of Gypsum, exactly 3 moles of water vapor are lost.
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