CHEM 67013 | Course Paper

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What is the mass of 0.50 mol chromium(III) sulfide?

A.2.5 10“3 g

B.5.9 10“3 g

C.42 g

D.1.0 102 g

E.110 g

Which one of the following sets of ions are listed in order of lowest to highest hydration

energy?

A.H+ < Na+ < Mg2+

B.Mg2+ < Ca2+ < Ba2+

C.Mg2+ < Ba2+ < Ca2+

D.Ca2+ < K+ < Rb+

E.Rb+ < K+ < Ca2+

Which one of the following molecules is polar?

A.CCl4

B.SF4

C.SO3

D.Br2

E.BCl3

Which of the following gases has the greatest density at 35 C and 450 mm Hg?

A.CH4

B.Ar

C.N2

D.Cl2

E.C3H8

The dissolution of ammonium nitrate occurs spontaneously in water at 25 C. As

NH4NO3 dissolves, the temperature of the water decreases. What are the signs of DrH,

DrS, and DrG for this process?

A.DrH > 0, DrS < 0, DrG > 0

B.DrH > 0, DrS > 0, DrG > 0

C.DrH > 0, DrS > 0, DrG < 0

D.DrH < 0, DrS < 0, DrG < 0

E.DrH < 0, DrS > 0, DrG > 0

Which of the following statements is/are CORRECT?

1/ FM radio waves have longer wavelengths than visible radiation and AM radio waves

have shorter wavelengths than visible radiation.

2/ Magnetic resonance imaging (MRI) uses a mixture of x-rays and gamma rays.

3/ Exposure to ultraviolet (UV) radiation can lead to sunburns.

A.1 only

B.2 only

C.3 only

D.1 and 2

E.1, 2, and 3

Molecules must overcome a barrier called the activation energy if they are to react. The

highest energy point reached during the progress of a reaction is called the ____.

A.rate determining step

B.transition state

C.half-life

D.elementary step

E.intermediate state

What is a correct cell notation for a voltaic cell based on the reaction below?

Cu2+(aq) + Pb(s) + SO4

2″(aq) Cu(s) + PbSO4(s)

A.Pb(s) | PbSO4(s) || Cu2+(aq) || Cu(s)

B.Cu(s) | Cu2+(aq) || SO4

2″(aq) | PbSO4(s) | Pb(s)

C.Cu(s) | Cu2+(aq), SO4

2″(aq) | PbSO4(s) | Pb(s)

D.Cu(s) | Cu2+(aq), SO4

2″(aq) || PbSO4(s) || Pb(s)

E.Pb(s) | PbSO4(s) | SO4

2″(aq) || Cu2+(aq) || Cu(s)

Which of the following is a correct Lewis structure for nitrous acid, HNO2?

An aqueous solution contains 0.010 M Br“ and 0.010 M I“. If Ag+ is added until

AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I“? (Ksp of

AgBr = 5.4 10“13, Ksp of AgI = 8.5 10“17)

A.[Ag+] = 5.4 10“11 M, [I“] = 1.0 10“2 M

B.[Ag+] = 8.5 10“15 M, [I“] = 1.0 10“2 M

C.[Ag+] = 5.4 10“11 M, [I“] = 1.6 10“6 M

D.[Ag+] = 8.5 10“15 M, [I“] = 6.4 101 M

E.[Ag+] = 8.5 10“15 M, [I“] = 1.6 10“6 M

Elemental sodium is commercially produced by electrolysis of ____. A valuable

by-product, ____, is simultaneously produced during the electrolysis.

A.NaCl( ), Cl2(g)

B.NaH(g), H2(g)

C.NaCl(aq), NaOH(aq)

D.Na2O2( ), O2(g)

E.Na2S(s), S8(s)

For a reaction, A B + C, which of the following equations corresponds to the integrated

expression for a zero-order decomposition reaction?

Which of the following species will have a Lewis structure most like that of IF4

“?

A.XeF4

B.SO4

2″

C.PF4

D.SF4

E.IO4

“

Which atom is most likely to form a 2+ ion?

A.scandium

B.calcium

C.aluminum

D.oxygen

E.fluorine

Which of the following is/are physical properties of amorphous solids?

1/ Amorphous solids have well defined melting points.

2/ At the particulate level, amorphous solids do not have long range order.

3/ Polymeric materials never form amorphous solids.

A.1 only

B.2 only

C.3 only

D.1 and 3

E.2 and 3

What is the maximum number of hybridized orbitals formed by an oxygen atom?

A.1

B.2

C.3

D.4

E.6

The speed of sound at one atmosphere of pressure is 0.214 miles per second. What is

the speed of sound in units of meters per second? (1 km = 0.621 mile)

A.133 m/s

B.345 m/s

C.478 m/s

D.4.46 104 m/s

E.4.78 105 m/s

How many isomers exist for the following benzene derivative, C6H4ClBr?

A.2

B.3

C.4

D.5

E.none

What is the pH of a solution that results from adding 250 mL of 0.50 M NaOH to 750

mL of 0.50 M HF? (Ka of HF = 7.2 10“4)

A.1.87

B.2.84

C.3.44

D.3.62

E.6.29

Which of the following species are likely to behave as oxidizing agents: Li(s), H2(g),

MnO4

“(aq), and Cl“(aq)?

A.Li(s) only

B.MnO4

“(aq) only

C.H2(g) and Cl“(aq)

D.Li(s) and MnO4

“(aq)

E.Cl“(aq) only

The pH of aqueous 0.50 M hypobromous acid, HBrO, is 4.45. What is the Ka of this

acid?

A.2.5 10“9

B.5.0 10“9

C.3.4 10“7

D.3.5 10“5

E.7.1 10“5

Metal hydrides are used to remove traces of water from nonpolar solvents. Write a

balanced chemical equation for the reaction of lithium hydride and water.

A.LiH2(s) + 2 H2O( ) Li(s) + 2 H3O+(aq)

B.2 LiH(s) + 2 H2O( ) 2 LiOH(s) + H2(g)

C.2 LiH(s) + H2O( ) Li2O(s) + 2 H2(g)

D.2 LiH(s) + H2O( ) Li2O(s) + 4 H+(aq)

E.LiH(s) + H2O( ) Li(s) + H3O+(aq)

The effect of adding a catalyst to a reaction is to

A.increase the number of collisions between reactants.

B.lower the activation energy of a reaction.

C.increase the equilibrium constant of a reaction.

D.decrease the yield of the products.

E.increase the enthalpy change of a reaction.

A buffer is prepared by combining 150 mL of 0.50 M NaOH and 250 mL of a 0.75 M

weak acid, HA. If the pH of the buffer is 5.50, what is the Ka of the acid?

A.1.3 10“11

B.1.3 10“6

C.2.1 10“9

D.3.2 10“6

E.4.7 10“6

Which group 1A metal is the strongest reducing agent?

A.Li

B.Na

C.K

D.Rb

E.Cs

Diagram 9-1

The molecular orbital diagram below may be used for the following problem(s). For

oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,

the diagram will still yield correct bond order and magnetic behavior for these

molecules.

Energy ________ s*2p

________ ________ p*2p

________ s2p

________ ________ p2p

________ s*2s

________ s2s

________ s*1s

________ s1s

Refer to Diagram 9-1. According to molecular orbital theory, which of the following

lists ranks the fluorine species in terms of increasing bond order?

A.F2

2+ < F2

2″ < F2

B.F2

2″ < F2 < F2

C.F2 < F2

2+ < F2

2″

D.F2 < F2

2″ < F2

E.F2

2+ < F2 < F2

2″

Which of the following is NOT a network solid?

A.elemental silicon, Si(s)

B.diamond, C(s)

C.buckminster fullerene, C60(s)

D.silicon dioxide, SiO2(s)

E.aluminum oxide, Al2O3(s)

What is the hybridization of the sulfur atom in sulfur tetrafluoride, SF4?

A.sp

B.sp2

C.sp3

D.sp3d

E.sp3d2

Aspirin (C9H8O4) is produced by the reaction of salicylic acid (M = 138.1 g/mol) and

acetic anhydride (M = 102.1 g/mol).

C7H6O3(s) + C4H6O3( ) C9H8O4(s) + C2H4O2( )

If you react 2.00 g C7H6O3 with 1.60 g C4H6O3, what mass of aspirin (M = 180.2

g/mol) can theoretically be obtained?

A.0.40 g

B.2.61 g

C.2.82 g

D.1.53 g

E.3.60 g

The Ksp of Ca(OH)2 is 5.5 10“5 at 25 C. What is the concentration of OH“(aq) in a

saturated solution of Ca(OH)2(aq)?

A.1.9 10“3 M

B.7.4 10“3 M

C.2.4 10“2 M

D.4.0 10“2 M

E.4.8 10“2 M

Which of the following combinations would be best to buffer an aqueous solution at a

pH of 9.0?

A.H3PO4 and H2PO4

“, Ka1 = 7.5 10“3

B.HNO2 and NO2

“, Ka = 4.5 10“4

C.CH3CO2H and CH3COO“, Ka = 1.8 10“5

D.H2PO4

“ and HPO4

2″, Ka2 = 6.2 10“8

E.NH4

+ and NH3, Ka = 5.7 10“10

What is the name of the following compound?

A.trans-acetylene

B.cis-1,3-pentadiene

C.trans-2,4-pentadiene

D.cis-4-methyl-1,3-butadiene

E.cis-4-methyl-1,3-butene

What is the mass of chlorine-35 relative to carbon-12?

A.0.657

B.0.522

C.1.52

D.2.92

E.23