The mass of CO 2 that shall be obtained by heating 10 kg of 80 % pure limestone ( CaCO 3) is: CaCO 3( s ) arrow CO 2( g )+ CaO ( s )

Question

The mass of CO 2 that shall be obtained by heating 10 kg of 80 % pure limestone ( CaCO 3) is: CaCO 3( s ) arrow CO 2( g )+ CaO ( s ) (A) 4.4 kg (B) 6.6 kg (C) 3.52 kg (D) 8.8

Tardigrade Admin · Accepted Answer

1 mol 1 mol 100 g 44 g 10 kg 4.4 kg (80/100) × 10 kg 4.4 × (80/100) = 8 kg =3.52 kg

1 mol	1 mol
$100 g$	$44 g$
$10 k g$	$4.4 k g$
$\frac{80}{100} \times 10 k g$	$4.4 \times \frac{80}{100}$
$= 8 k g$	$= 3.52 k g$

Q. The mass of $C O_{2}$ that shall be obtained by heating $10 k g$ of $80%$ pure limestone $(C a C O_{3})$ is:
$C a C O_{3} (s) \to C O_{2} (g) + C a O (s)$

$4.4 k g$

$6.6 k g$

$3.52 k g$

$8.8$

1 mol 1 mol

$100 g$ $44 g$

$10 k g$ $4.4 k g$

$\frac{80}{100} \times 10 k g$ $4.4 \times \frac{80}{100}$

$= 8 k g$ $= 3.52 k g$

Q. The mass of CO2​ that shall be obtained by heating 10kg of 80% pure limestone (CaCO3​) is: CaCO3​(s)→CO2​(g)+CaO(s)

4.4kg

6.6kg

3.52kg

8.8