Question

Calcium oxide and oxygen gas are produced by the thermal decomposition of limestone in the reaction CaCO (s) CaO(s) + CO (g). What mass of lime can be produced from 4.5 10 kg of limestone? Please show all the work

Answer 1

As the power on mass of CaCO₃ is not given so we are assuming it 4.5 × 10³ Kg.

Answer:
2520 Kg of CaO

Solution:

The balance chemical equation is as follow,

CaCO₃ → CaO + CO₂

According to equation,

0.1 Kg (1 mole) CaCO₃ produces = 0.056 Kg (1 mole) of CaO
So,
4.5 × 10³ Kg CaCO₃ will produce = X Kg of CaO

Solving for X,
X = (4.5 × 10³ Kg × 0.056 Kg) ÷ 0.1 Kg

X = 2520 Kg of CaO

Answer 2

The mass of lime that can be produced from 4.510 Kg of limestone is calculated as below

calculate the moles of CaCO3 used

that is moles =mass/molar mass
convert Kg to g = 4.510 x1000 =4510g
= 4510 / 100 =45.10 moles
CaCO3 = CaO +O2

by use of mole ratio between CaCO3 to CaO (1:1) the moles of CaO is also= 45.10 moles
mass of CaO = moles x molar mass

45.10 x56 = 2525.6 g of CaO