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Chapter 21: Problem 14

How would you obtain zinc from sphalerite (ZnS)?

Short Answer

Expert verified
Zinc can be obtained from sphalerite (ZnS) in two major steps. The first step is roasting where the ZnS is heated in air to obtain ZnO. The second step is reduction, in which the ZnO is reduced using carbon to obtain zinc.

Step by step solution

01

- Roasting

In the roasting process, the zinc sulphide (ZnS) is first converted into zinc oxide (ZnO) by heating in air. The balanced chemical equation for this is: \[ 2ZnS + 3O_2 \rightarrow 2ZnO + 2SO_2 \] With this step, the sulphide ore is converted into an oxide ore which can be reduced more easily.
02

- Reduction

To extract zinc from the zinc oxide formed in Step 1, a reduction process is used. Zinc oxide is heated with carbon, which reduces the zinc oxide to zinc. The balanced chemical reaction is \[ ZnO + C \rightarrow Zn + CO \]
03

- Collection and Refinement

The zinc produced in the reduction process is then collected and refined to remove any remaining impurities. One of the ways to refine zinc is by distillation since zinc has a relatively low boiling point (907°C)

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Most popular questions from this chapter

List three metals that are usually found in an uncombined state in nature and three metals that are always found in a combined state in nature.

Complete and balance the following equations: (a) \(\mathrm{K}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\operatorname{NaH}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow\) (d) \(\mathrm{K}(s)+\mathrm{O}_{2}(g) \longrightarrow\)

In the Mond process for the purification of nickel, CO is passed over metallic nickel to give \(\mathrm{Ni}(\mathrm{CO})_{4}\) : $$\mathrm{Ni}(s)+4 \mathrm{CO}(g) \Longrightarrow \mathrm{Ni}(\mathrm{CO})_{4}(g)$$Given that the standard free energies of formation of \(\mathrm{CO}(g)\) and \(\mathrm{Ni}(\mathrm{CO})_{4}(g)\) are \(-137.3 \mathrm{~kJ} / \mathrm{mol}\) and \(-587.4 \mathrm{~kJ} / \mathrm{mol},\) respectively, calculate the equilibrium constant of the reaction at \(80^{\circ} \mathrm{C}\). (Assume \(\Delta G_{\mathrm{f}}^{\circ}\) to be independent of temperature.

What action renders aluminum inert?

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