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

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

Answer 2

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