$ \begin{array}{l} \mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \stackrel{\Delta, 120^{\circ} \mathrm{C}}{\longrightarrow} \mathrm{A} \ \mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \stackrel{\Delta, 200^{\circ} \mathrm{C}}{\longrightarrow} \mathrm{B} \end{array} $ In the above reaction, $ \mathrm{A} $ and $ \mathrm{B} $, respectively, are:

Question

$ \begin{array}{l} \mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \stackrel{\Delta, 120^{\circ} \mathrm{C}}{\longrightarrow} \mathrm{A} \ \mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \stackrel{\Delta, 200^{\circ} \mathrm{C}}{\longrightarrow} \mathrm{B} \end{array} $ In the above reaction, $ \mathrm{A} $ and $ \mathrm{B} $, respectively, are:, $ \mathrm{CaSO}_{4}, \mathrm{CaSO}_{4} \cdot \frac{1}{2} \mathrm{H}_{2} \mathrm{O} $, $ \mathrm{CaSO}_{4} \cdot \frac{1}{2} \mathrm{H}_{2} \mathrm{O}, \mathrm{CaSO}_{4} $, $ \mathrm{CaSO}_{4} \cdot \frac{1}{2} \mathrm{H}_{2} \mathrm{O} $, Gypsum., Gypsum, $ \mathrm{CaSO}_{4} $.

MARKS App · Accepted Answer

CaSO 4 · 2 H 2 O at 120 o C CaSO 4 · 1 2 H 2 O + 1 1 2 H 2 O The commercial name of the compound Calcium sulphate hemihydrate, i.e., Plaster of Paris. CaSO 4 · 2 H 2 O → ∆ , 200 ° C anhydrous CaSO 4 + 2 H 2 O Anhydrous calcium sulphate formed this way is commonly called dead burnt plaster.

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