chemistry in industry and technology option c. the blast furnace
TRANSCRIPT
Chemistry in Industry and Technology
Option C
The Blast Furnace
• This follows closely from IGCSE work. If you can’t remember the work you did at IGCSE then you need to revise!
• You will learn about some different sources of iron, and you will learn more detail about the chemical reactions that happen in a blast furnace.
Syllabus Statements
• C1.1 State the main sources of iron.
• C1.2 Describe the main reactions that occur in the blast furnace.
Tuyere
• The Iron Ore fed into the blast furnace may be a number of different compounds:
I. Haematite Fe2O3 (this is the one you learnt at IGCSE)
II. Magnetite Fe3O4
III. Iron Pyrites FeS2 (Fool’s gold!)
FeS2 must be converted to the oxide:
4FeS2 + 11O2 2Fe2O3 + 8SO2
• Coke is also fed in at the top.• This provides a source of carbon to reduce the
iron oxide.
• Fe2O3 + 3C 2Fe + 3CO
• This DOES happen to a small extent – but from IGCSE you know its not really that simple!
• Most of the reduction is done by Carbon Monoxide CO.
• C + O2 CO2
• CO2 + C 2CO
• This carbon monoxide then reduces the iron ore.
• Either
• Fe2O3 + 3CO 2Fe + 3CO2
• Or
• Fe3O4 + 4CO 3Fe + 4CO2
• Both these reactions are exothermic.• The iron produced is molten because of the
high temperature. (Iron melts at 1536 °C or 2797 °F (1811 K). It boils at 2862 °C or 5182 °F (3134 K).)
• It sinks to the bottom of the furnace where it can be “tapped”
• There are 2 more possible reaction mechanisms that you need to learn:
• If methane (“natural gas”) is blown into the furnace, then incomplete combustion can take place.
• 2CH4 + O2 2CO + 4H2
• Then either the CO can act as the reducing agent as before, or the H2 can act as the reducing agent.
• Write balanced equations for hydrogen reducing both the forms of iron oxide present.
• Fe3O4 + 4H2 3Fe + 4H2O
• Fe2O3 + 3 H2 2Fe + 3H2O
Getting rid of impurities
• The iron ore fed into the blast furnace is NOT a pure chemical.
• It contains impurities such as silicon (IV) oxide and aluminium oxide.
• These come from the rocks which contain the iron compounds.
Relative abundance of elements in the Earth’s crust
• Oxygen 46.6% • Silicon 27.7% • Aluminum 8.1% • Iron 5.0% • Calcium 3.6% • Potassium 2.6% • Magnesium 2.6%
• The third raw material added at the top of the blast furnace is powdered limestone.
• This decomposes at the high temperatures involved.
• CaCO3 CaO + CO2
• Calcium oxide is “quicklime”• Quicklime is very basic and reacts with the
impurities we have mentioned.
• CaO + SiO2 CaSiO3
• CaO + Al2O3 CaAl2O4
• Silicon oxide is a non-metal oxide and is therefore acidic.
• Aluminium oxide is amphoteric!!
• Both the compounds formed are liquids.• We call them “slag”• They float on top of the molten iron and can
be removed through a second outlet.• They are used for roads and making cement.• Because they can be easily removed the blast
furnace can be run continuously for a number of years (good economics!).
• Eventually the lining of the furnace breaks down and we have to let the whole thing cool down so we can replace it.
Reminder . . .
• C1.1 State the main sources of iron.
• C1.2 Describe the main reactions that occur in the blast furnace.
Summary . . .
Iron Ore Carbon Limestone
Reduction reactions Reactions to remove impurities
Making CO CO reducing oxides
methane giving H2 H2 reducing oxides
Forming quicklime reaction with Al2O3 reaction with SiO2
Tuyere