Question

If 1.4g of calcium oxide is formed by the complete decomposition of calcium carbonate, then the amount of calcium carbonate taken and the amount of carbon dioxide formed will be respectively

Answer 1

1.4 g CaO x (1 mol CaO/56 g CaO) x (1 mol CaCO3/1 mole CaO) x (100 g CaCO3/1 mol CaCO3) = 2.5 g

Answer 2

Answer: a) The amount of calcium carbonate taken is 25 g and the amount of carbon dioxide formed is 11 g.

Explanation: $CaCO_3\rightarrow CaO+CO_2$

As seen from the balanced equation ,

1 mole of  $CaCO_3$ on complete decomposition produces 1 mole of $CaO$ and 1 mole of $CO_2$.

a) 100 g of $CaCO_3$ on complete decomposition produces 56 of $CaO$

Thus 56 g of $CaO$ is produced by  100 g of $CaCO_3$.

14 g of $CaO$ is produced by=$\frac{100}{56}\times 14= 25g of [tex]CaCO_3$.

b) 100 g of $CaCO_3$ on complete decomposition produces 44 g of $CO_2$.

25 g of $CaCO_3$ on complete decomposition produces=$\frac{44}{100}\times 25=11g$ of $CO_2$.