Question

Calculate the mass of $C{O}_2$ produced by decomposing 40 g of 60 % pure limestone.

• A. 10.56 g
• B. 12.38 g
• C. 8.20 g
• D. 14.52 g

Answer 1

The correct option is A 10.56 g

$CaC{O}_3\to CaO+C{O}_2$
Mass of 60% pure $CaC{O}_3$ = 60 % $\times$40 g = 24 g
Moles of $CaC{O}_3=\frac{\text{given mass}}{\text{molar mass}}=\frac{24}{100}=0.24$ moles
As per the reaction,
1 mole of $CaC{O}_3$ decomposes to give 1 mole of $C{O}_2$ gas
0.24 moles of $CaC{O}_3$ will give 0.24 mole of $C{O}_2.$
mass of $C{O}_2$ produced = $0.24\times 44$ = 10.56 g