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Question
Write down the reactions taking place in Blast furnace related to the metallurgy of iron in the temperature range 500-800 K.
Solution
The following reactions take place in blast furnace during the metallurgy of iron at the temperature range 500-800 K.
\[\ce{3Fe2O3 + CO -> 2Fe3O4 + CO2}\]
\[\ce{Fe3O4 + CO -> 3FeO + CO2}\]
\[\ce{Fe2O3 + CO -> 2FeO + CO2}\]
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RELATED QUESTIONS
Why is the extraction of copper from pyrites more difficult than that from its oxide ore through reduction?
The choice of a reducing agent in a particular case depends on thermodynamic factor. How far do you agree with this statement? Support your opinion with two examples.
The impurity that is added externally to remove the impurity already present in the ore is known as ____________.
For the reduction of \[\ce{FeO}\] at the temperature corresponding to point D, which of the following statements is correct?
For the metallurgical process of which of the ores calcined ore can be reduced by carbon?
(i) Haematite
(ii) Calamine
(iii) Iron pyrites
(iv) Sphalerite
The mixture of compounds A and B is passed through a column of \[\ce{Al2O3}\] by using alcohol as eluant. Compound A is eluted in preference to compound B. Which of the compounds A or B, is more readily adsorbed on the column?
Why is sulphide ore of copper heated in a furnace after mixing with silica?
Explain the following:
\[\ce{CO2}\] is a better reducing agent below 710 K whereas \[\ce{CO}\] is a better reducing agent above 710 K.
Explain the following:
Carbon and hydrogen are not used as reducing agents at high temperatures.
Assertion: For the extraction of iron, haematite ore is used.
Reason: Haematite is a carbonate ore of iron.
