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How many moles of limestone will be required to produce 5.6g of CaO?


Question

How many moles of limestone will be required to produce 5.6g of CaO?

Options

A)
0.20 mol
B)
0.10 mol
C)
1.12 mol
D)
0.56 mol
E)
0.30 mol

The correct answer is B.

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 * 100)/56 = 10g of CaCO3
moles = mass/molar mass = 10/100 = 0.10m


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Dicussion (1)

  • CaCO3 —> CaO + CO2
    1 : 1. 1
    40 + 12 + (16x3) —> 40 x 16

    100g = 56 g
    X = 5.6g
    X = (100 X 5.6)/56 = 10g

    Let the mole of CaCO3 that produced 5.6g of CaO be y

    But 1mole = 100g
    Y. =. 10
    Y = 10/100 = 0.1mole.

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