A significant contribution to atmospheric Carbon dioxide levels comes from the thermal decomposition of limestone in the manufacture of cement and of lime for agricultural purposes.
Cement works roast 1000 million tones of limestone per year and a further 200 million tones is roasted in kilns to make lime.
What is the total annual mass output of carbon dioxide (in million tones) from these two processes?
Solution:
The thermal decomposition of limestone is:
CaCO3→CaO+CO2
Using atomic masses from the periodic table, we will find the following:
M(CaCO3)=40+12+16.3=100 g/mol=100 kg/kmolM(CaO)=40+16=56 g/mol=56 kg/kmol;M(CO2)=12+16.2=44 g/mol=44 kg/k/mol.
If we roast 100 kg of limestone we obtain 44 kg of CO2, for the equation of reaction. From 1000 million tones of limestone we obtain:
m(CO2)=1001000⋅44=440 million tones
When we prepare 56 kg lime (CaO) we also obtain 44 kg CO2. If we prepare 200 million tones CaO we also obtain the mass of CO2:
m(CO2)=56200⋅44=157.14 million tones.
The total mass CO2 output from two processes:
m(CO2)=440.0+157.4=597.4 million tones.Answer:
The total mass CO2 output from two processes is 597.4 million tones.