The right option for the mass of produced by heating 20 g of 20% pure limestone is (Atomic mass of Ca = 40) [2023]

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Solution

Q.
The right option for the mass of ${CO}_{2}$ produced by heating 20 g of 20% pure limestone is (Atomic mass of Ca = 40)

${[CaCO}_{3} \overset{1200 K}{\to} CaO + {CO}_{2}]$ [2023]

1 2.64 g

2 1.32 g

3 1.12 g

4 1.76 g

Ans.
(4)

$\underset{40 + 12 + 16 \times 3 = 100 g}{{CaCO}_{3}}$ $\overset{1200 K}{\to}$ $\underset{40 + 16 = 56 g}{CaO}$ $+$ $\underset{44 g}{{CO}_{2}}$

100 g ${CaCO}_{3}$ produced ${CO}_{2}$ gas = 44 g

20 g ${CaCO}_{3}$ will produce ${CO}_{2}$ gas = $\frac{44}{100} \times 20 = 8.8 g$

If sample is 100% pure, ${CO}_{2}$ produced = 8.8 g

If sample is 20% pure, ${CO}_{2}$ produced = $\frac{8.8}{100} \times 20 = 1.76 g$

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