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Chapter 21: Problem 53

In steelmaking, nonmetallic impurities such as \(\mathrm{P}, \mathrm{S}\) and \(\mathrm{Si}\) are removed as the corresponding oxides. The inside of the furnace is usually lined with \(\mathrm{CaCO}_{3}\) and \(\mathrm{MgCO}_{3},\) which decompose at high temperatures to yield \(\mathrm{CaO}\) and \(\mathrm{MgO}\). How do \(\mathrm{CaO}\) and \(\mathrm{MgO}\) help in the removal of the nonmetallic oxides?

Short Answer

Expert verified
In steelmaking, nonmetallic impurities are removed with the help of \(\mathrm{CaO}\) and \(\mathrm{MgO}\) which are produced from the decomposition of \(\mathrm{CaCO}_{3}\) and \(\mathrm{MgCO}_{3}\) at high temperatures. These compounds act as fluxes that lower the melting point of the nonmetallic oxides, promoting their removal. They react with the nonmetallic oxides to form less dense compounds which can be easily separated from the steel.

Step by step solution

01

Understanding the role of Calcium oxide and Magnesium oxide

Firstly, it's important to get a basic understanding of the roles \(\mathrm{CaO}\) and \(\mathrm{MgO}\) play in the steelmaking process. These compounds act as fluxes, which are substances that can lower the melting point of another substance. In this case, \(\mathrm{CaO}\) and \(\mathrm{MgO}\) lower the melting point of these nonmetallic oxides.
02

Role of \(\mathrm{CaO}\) and \(\mathrm{MgO}\) in removal of nonmetallic oxides

\(\mathrm{CaO}\) and \(\mathrm{MgO}\) react with the nonmetallic oxides to form compounds that can be separated from the steel. These compounds, being less dense, float to the top of the melting pot and can be skimmed off, thereby effectively removing the nonmetallic oxides from the steel.
03

Process at higher temperatures

When subjected to high temperatures, the \(\mathrm{CaO}\) and \(\mathrm{MgO}\) become more reactive. This provides a better environment, in which the non-metallic oxides are readily reacted and removed from the steel.

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Most popular questions from this chapter

Write a balanced equation for each of the following reactions: (a) Sodium reacts with water; (b) an aqueous solution of \(\mathrm{NaOH}\) reacts with \(\mathrm{CO}_{2} ;\) (c) solid \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) reacts with a HCl solution; (d) solid \(\mathrm{NaHCO}_{3}\) reacts with a HCl solution; (e) solid \(\mathrm{NaHCO}_{3}\) is heated; (f) solid \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is heated.

It has been shown that \(\mathrm{Na}_{2}\) species form in the vapor phase. Describe the formation of the "disodium molecule" in terms of a molecular orbital energylevel diagram. Would you expect the alkaline earth metals to exhibit a similar property?

Describe the uses of the following compounds: \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{NaOH}, \mathrm{KOH}, \mathrm{KO}_{2}\)

What action renders aluminum inert?

A certain mine produces \(2.0 \times 10^{8} \mathrm{~kg}\) of copper from chalcopyrite (CuFeS \(_{2}\) ) each year. The ore contains only 0.80 percent Cu by mass. (a) If the density of the ore is \(2.8 \mathrm{~g} / \mathrm{cm}^{3},\) calculate the volume (in \(\mathrm{cm}^{3}\) ) of ore removed each year. (b) Calculate the mass (in kg) of \(\mathrm{SO}_{2}\) produced by roasting (assume chalcopyrite to be the only source of sulfur).
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