25g of 80% pure Ca $C O_{3}$ is made to react with excess of HCl. Calculate volume of $C O_{2}$ evolved at NTP.

1.18 L

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2.28 L

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3.38 L

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4.48 L

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Solution

The correct option is D
4.48 L

From the question, it is a volume-volume problem.
The balanced reaction $\Rightarrow C a C O_{3} + 2 H C l$ $\to C a C l_{2} + C O_{2} + H_{2} O$
25 g of 80 % pure Ca $C O_{3} \Rightarrow \times \frac{25 X 80}{100}$ $= 20 g o f C a C O_{3}$
$∴$ From reaction, 1 mole of $C a C O_{3}$ gives 1 mole of $C O_{2}$
At NTP, 1 mole of Ca $C O_{3}$ = 22.4 L of $C O_{2}$
100g of Ca $C O_{3}$ = 22.4 L of $C O_{2}$
20g of Ca $C O_{3}$ =( 22.4 X20)/100 = 4.48 L

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