Question

mass of CO2 obtained when 2 grams of pure limestone is heated

Answer 1

CaCO3 ➡️ Co2 + CaO.

100 gm ➡️ 44gm

2 gm ➡️ x

So, x = 0.88 gm is your answer.

Answer 2

Given:

2 grams of pure limestone is heated.

To find:

We have to find the mass of carbon dioxide obtained.

Solution:

The chemical formula of limestone is $CaCO_3$.

The heating of limestone is given as-

$CaCO_3\rightarrow CaO+CO_2$.

The atomic mass of Ca is 40.

The atomic mass of C is 12 and Oxygen is 16 grams.

Hence the molecular weight of calcium carbonate is 40+12+16×3=100 grams.

The molecular weight of carbon dioxide is 12+16×2=44 grams.

Hence 100 grams of limestone is heated to produce 44 grams of carbon dioxide.

So, 2 grams of limestone is heated to produce 44×2/100=0.88 grams of carbon dioxide.

2 grams of limestone is heated to produce 0.88 grams of carbon dioxide.