The mass of CaO that would be obtained by heating 20 kg of $90 %$ pure lime stone is:

$11.2 k g$

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$8.4 k g$

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$10.08 k g$

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$16.8 k g$

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Solution

The correct option is C
$10.08 k g$

Mass of pure limestone = $(\frac{90}{100}) \times 20 = 18 k g$
$C a C O_{3} Δ - \to C a O + C O_{2}$
100 kg of $C a C O_{3}$ forms 56 kg of CaO
18 kg of $C a C O_{3}$ forms $\frac{(18 \times 56)}{100} = 10.08 kg of CaO$

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