The mass of CaO that would be obtained by heating 20 kg of 90 % pure lime stone is: Options: A . &nbsp 11.2 k g B . &nbsp 8.4 k g C . &nbsp 10.08 k g D . &nbsp 16.8 k g

Answer: Option C : C Mass of pure limestone = ( 90 100 ) × 20 = 18 k g C a C O 3 Δ − → 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 ( 18 × 56 ) 100 = 10.08 kg of CaO

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

Discussion Forum : Mole Concept

Question -

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

Options:

A .

11.2 k g

B .

8.4 k g

C .

10.08 k g

D .

16.8 k g

Answer: Option C
:
C

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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