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Exam 21: Metallurgy and the Chemistry of Metals

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Question 1

True/False

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Beryllium, the first element in Group 2A, is the most metallic element in the group.

A) True
B) False

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Question 2

Multiple Choice

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The equilibrium 3Fe(s) + C(s) Fe₃C(s) is established in a solid solution.For such a solution, one can write an equilibrium constant expression in the usual way except that the concentrations that refer to solids in the solid solution are included.Determine the equilibrium constant for the formation of cementite from iron and carbon at 680°C.(Given: for this reaction at 25°C, $\Delta$ H° = 21 kJ/mol and $\Delta$ S° = 20.4 J/mol·K)

A) 0.75
B) 0.33
C) 3.1
D) 0.82
E) 1.2

F) A) and B)
G) A) and E)

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Question 3

Multiple Choice

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What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the reaction below to obtain chromium metal: Cr₂O₃(s) + 2Al(s) $\rarr$ 2Cr(l) + Al₂O₃(s)

The naturally occurring form of a metal that is concentrated enough to allow economical recovery of the metal is know as

Which of these ions is most likely to substitute for Ca²⁺ in the human body?

Which one of these metals would normally be obtained by electrolytic reduction?

The principal reducing agent in a blast furnace is

Calcium metal is produced by electrolysis of

For the reaction 3Fe(s) + C(s) Fe₃C(s) , $\Delta$ H° = 21 kJ/mol and $\Delta$ S° = 20.4 J/mol·K at 25°C.Estimate the minimum temperature above which the formation of cementite (Fe₃C) is favored.

How much energy (kJ) is released when 15.0g of Fe(l) is produced in the thermite reaction: 2Al(s) + Fe₂O₃(s) $\rarr$ Al₂O₃(s) + 2Fe(l) $\Delta$ H° = - 822.8 kJ/mol

How much energy (kJ) is released if 10.0g of Al(s) is reacted with excess Fe₂O₃(s) in the thermite reaction: 2Al(s) + Fe₂O₃(s) $\rarr$ Al₂O₃(s) + 2Fe(l) $\Delta$ H° = - 822.8 kJ/mol

Write two balanced chemical equations for the burning of magnesium in air.

Which one of these elements has seawater as its commercial source?

Potassium superoxide, KO₂(s), is used in the breathing systems of biohazard suits.Write separate chemical equations showing how KO₂(s)reacts with moisture and carbon dioxide in exhaled air to generate oxygen gas.

In n-type semiconductors

Bauxite (Al₂O₃·2H₂O)ore is the principal commercial source of aluminum metal.

The following reaction is used to produce titanium metal at high temperature. TiCl₄(g)+ 2Mg(l) $\rarr$ Ti(s)+ 2MgCl₂(l) Which element is oxidized and which is reduced?

Volatile impurities are removed from ores by means of

Write the chemical formula of pyrite.

Which of the following diagrams represents a semiconductor?