01: Atoms 02: Periodic Table / Elements 03: Chemical Bonds 04: Nomenclature 05: Structures of Matter 06: Substances of the environment 07: Chemical Reactions 08: Reactions in Equilibrium 09: Acid-base-reactions 10:Redox reactions 11: Carbon chemistry 12: Biochemistry 13: Qualitative analysis 14: Quantitative analysis 15: Chemical Industry 16: Reactions in the environment
C(s) + O2(g) CO2(g)Obviously all other substances present in the coal, will also be burned. Think of Sulphur and Nitrogen, who can, burning, can produce: NO, NO2 and SO2. These oxydes are delevered to the atmosphere and cause acid rain.
2C(s) +O2(g) 2CO(g)
2C(s) + O2(g) 2CO(g)Oxygen from the air will burn the carbon of cokes and the powdered coal; carbonmonoxyde (CO)is produced. This gas with a temperature of about 2200-2400°C will rise through the different layers of cokes and ore.
Fe2O3(s) + 3CO(g) 3 CO2(g) + 2Fe(l) (Reduction of iron ore into iron)
Fe3+ (present in ore) + 3 e- Fe (first in the liquid, later in the solid iron)Those electrons are delivered by the reductor CO, that in this proces will change into CO2. About that more: