![]() The calcium carbonate in the limestone thermally decomposes to form calcium oxide. This is due to the cost and energy required to start the reaction in the first place meaning it would be too expensive and use too much energy if it was started and stopped regularly. The blast furnace is a continuous process (ie reactants are added constantly so that the reaction does not stop). Iron(III) oxide + carbon monoxide → iron + carbon dioxideįe 2 O 3 (s) + 3CO(g) → 2Fe(l) + 3CO 2 (g) In the blast furnace, it is so hot that carbon monoxide can be used, in place of carbon, to reduce the iron(III) oxide: In this reaction, the iron(III) oxide is reduced to iron, and the carbon is oxidised to carbon dioxide. Iron(III) oxide + carbon → iron + carbon dioxideĢFe 2 O 3 (s) + 3C(s) → 4Fe(l) + 3CO 2 (g) Step 2 – More coke is added to the furnace and reduces the carbon dioxide into carbon monoxide, a good reducing agent. Step 1 – Hot air (oxygen) reacts with the coke (carbon) to produce carbon dioxide and heat energy to heat up the furnace. Provides oxygen to allow the coke to burn, and so produces heatĬarbon is more reactive than iron, so it can displace iron from iron(III) oxide. Helps to remove acidic impurities from the iron by reacting with them to form molten slag Used as a fuel and reacts to form carbon monoxide (needed to reduce the iron(III) oxide) ![]() Raw materials for the reaction Raw materialĪ compound that the iron is extracted from Reactions in which oxygen is removed are called reduction reactions. The oxygen must be removed from the iron(III) oxide in order to leave the iron behind. Iron ores such as haematite contain iron(III) oxide, Fe 2 O 3. Iron is extracted from iron ore in a huge container called a blast furnace. ![]()
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