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Chapter 22: Q22.28P (page 1018)

Why is cryolite used in the electrolysis of aluminum oxide?

Short Answer

Expert verified

Cryolite( ${Na}_{3} {AlF}_{6}$ ) is used in the electrolysis of aluminum oxide because cryolite helps to extract aluminum profitably.

Step by step solution

01

Cryolite

The compound cryolite is sodium aliminium fluoride $({Na}_{3} {AlF}_{6})$ . It is added to bauxite in aluminum smelting.

02

Explanation

- The high melting point of aluminum oxide is $2030^{°} C$ . The Hall-Héroult process makes

it difficult to refine aluminum.

- When cryolite is added, the melting point of the mixture becomes $1000^{°} C$ .

- Cryolite can also act as a solvent. It increases the conductivity of the solution of molten

bauxite.

-Therefore, cryolite helps to extract aluminum profitably.

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Most popular questions from this chapter

lodine is the only halogen that occurs in a positive oxidation state, in impurities within Chile saltpeter, ${NaNO}_{3}$ .

(a) Is this mode of occurrence consistent with iodine's location in the periodic table? Explain.

(b) In the production of $I_{2},I {O_{3}}^{-}$ reacts with $HS {O_{3}}^{-}$ :

$I {O_{3}}^{-} (aq) + HS {O_{3}}^{-} (aq) \to HS {O_{4}}^{-} (aq) + S {O_{4}}^{2 -} {(aq) +H}_{2} {O(I) +I}_{2} (s)$

[unbalanced] Identify the oxidizing and reducing agents.

(c) If $0.78 mol %$ of an ${NaNO}_{3}$ deposit is ${NaIO}_{3}$ , how much $I_{2}$ (in g) can be obtained from $1.000$ ton (2000. Ib) of the deposit?

Question: Chemosynthetic bacteria reduce ${CO}_{2}$ by “splitting” $H_{2} S (g)$ instead of the $H_{2} O (g)$ used by photosynthetic organisms. Compare the free energy change for splitting $H_{2} S$ with that for splitting $H_{2} O$ . Is there an advantage to using $H_{2} S$ instead of $H_{2} O$ ?

How are each of the following involved in iron metallurgy?

(a) slag; (b) pig iron; (c) steel; (d) basic-oxygen process?

How does acid rain affect the leaching of phosphate into groundwater from terrestrial phosphate rock? Calculate the solubility of ${Ca}_{3} {(PO}_{4})_{2}$ in each of the following: (a) Pure water, pH(Assume that $P {O_{4}}^{3 -}$ does not react with water.) (b) Moderately acidic rainwater, pH $4.5$ (Hint: Assume that all the phosphate exists in the form that predominates at this pH.)

Use equations to show how acid-base properties are used to separate ${Fe}_{2} O_{3}$ and ${TiO}_{2} {from Al}_{2} O_{3}$ in the Bayer process.

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