How many moles of limestone will be required to produce 5.6g of CaO? [Ca = 40, C = 12, O= 16]

A. 0.20 mol
B. 0.10 mol
C. 1.12 mol
D. 0.56 mol

Correct Answer:

Option B = 0.10 mol

Explanation

CaCO3 → CaO + CO2
CaCO3 = 40 + 12 + 16 * 3 = 100, CaO = 40 + 16 = 56
56gt of CaO was produced by 100g of CaCO3
∴ 5.6g of CaO will produce by
(5.6 X 100)/56 = 10g of CaCO3
moles = mass/molar mass = 10/100 = 0.10m