Question

Calculate mass of Co₂ produced by heating 40g of 20% pure limestone.​

Answer 1

Answer:

Reaction of CaCO3 -> CaO + CO2

The decomposition equation shows 1 CaCO3 gives 1 CaO and 1 CO2.

Mass of CaCO3 = 40 g + 12 g + (16 g x 3) = 100 g

Mass of CO2 = 12 g + (16 g x 2) = 44 g

So ,it is clear that 100g of caco3 gives 44g of co2.

We have 40g of 20% pure caco3

Mass of caco3 = 40×(20/100)

= 40/5 = 8g

Co2 obtained from 8 g of caco3 = 8×(44/100)

= (352/100) g

= 3.52 g

Hope this answer will help you

Please mark as Brainliest

Answer 2

CaCO₃ → CaO+CO₂----------------(i)

Pure CaCO₃=

$\frac{40 \times 20}{100} = 8g$

From equation,

100g CaCO₃ gives CO₂= 44g

∴ 8g CaCO₃ gives CO₂ =

$\frac{44}{100} \times 8 = 3.52g$✔

Hope this will help you ❤