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2nd Session Pre-Test Chemistry Mr R

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
All of the following are homogeneous mixtures except
a.
soil.
c.
gasoline.
b.
a sugar-water solution.
d.
a salt-water solution.
 

 2. 
An endothermic dissolution process
a.
absorbs energy as heat and has positive enthalpy of solution.
b.
releases energy as heat and has positive enthalpy of solution.
c.
absorbs energy as heat and has negative enthalpy of solution.
d.
releases energy as heat and has negative enthalpy of solution.
 

 3. 
As temperature increases, solubility of solids in liquids
a.
always increases.
c.
usually increases.
b.
always decreases.
d.
usually decreases.
 

 4. 
What is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg water? (molar mass of KNO3 = 101.11 g/mol)
a.
0.315 m
c.
1.02 m
b.
0.779 m
d.
1.14 m
 

 5. 
The hydrogen ion
a.
has a charge of 2+.
c.
has a negative charge.
b.
is a proton.
d.
is a bare electron.
 

 6. 
Nonvolatile solutes
a.
depress freezing point and elevate boiling point.
b.
elevate freezing point and depress boiling point.
c.
depress both freezing point and boiling point.
d.
elevate both freezing point and boiling point.
 

 7. 
Actual freezing-point depressions of electrolyte solutions are slightly lower than the calculated values because of
a.
ion repulsion.
b.
more complete ionization than is expected.
c.
ion attraction.
d.
higher-than-expected effective concentration.
 

 8. 
Acetic acid is found in
a.
lemons.
c.
sour milk.
b.
vinegar.
d.
apples.
 

 9. 
Which of the following is chlorous acid?
a.
HClO
c.
HClO3
b.
HClO2
d.
HClO4
 

 10. 
An electron-pair acceptor is a(n)
a.
Brønsted-Lowry base.
c.
Lewis base.
b.
Lewis acid.
d.
Arrhenius acid.
 

 11. 
If [H3O+] = 1.7 ´ 10–3 M, what is the pH of the solution?
a.
1.81
c.
2.42
b.
2.13
d.
2.77
 

 12. 
What process measures the amount of a solution of known concentration required to react with a measured amount of a solution of unknown concentration?
a.
autoprotolysis
c.
neutralization
b.
hydrolysis
d.
titration
 

 13. 
An acid-base titration determines the volumes of two solutions that
a.
are chemically equivalent.
c.
have equal mass.
b.
have equal molarity.
d.
have equal molality.
 

 14. 
What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
a.
0.200 M
c.
0.320 M
b.
0.280 M
d.
0.500 M
 

 15. 
Which of the following best describes temperature?
a.
energy as heat absorbed or released in a chemical or physical change
b.
a measure of the average kinetic energy of the particles in a sample of matter
c.
energy in the form of heat
d.
energy of change
 

 16. 
What units are used to measure energy as heat?
a.
joules/mole or kilojoules/mole
c.
joules or kilojoules
b.
kelvins or degrees Celsius
d.
None of the above
 

 17. 
A reaction is spontaneous if mc017-1.jpg is
a.
zero.
c.
positive.
b.
negative.
d.
greater than DH.
 

 18. 
What is the value of mc018-1.jpg at 200 K for a reaction in which mc018-2.jpg= –150 kJ/mol and mc018-3.jpg = +2.00 kJ/(mol·K)?
a.
–250 kJ/mol
c.
+250 kJ/mol
b.
–450 kJ/mol
d.
+450 kJ/mol
 

 19. 
Which branch of chemistry studies reaction mechanisms?
a.
thermochemistry
c.
chemical kinetics
b.
thermodynamics
d.
calorimetry
 

 20. 
For most reactions, particles must
a.
collide.
c.
be at rest.
b.
be properly oriented.
d.
collide in the proper orientation.
 

 21. 
Reaction rate depends upon
a.
both collision frequency and efficiency.
b.
average kinetic energy.
c.
collision efficiency.
d.
average potential energy.
 

 22. 
A sample of a substance burns more rapidly in pure oxygen than in air. Which factor is most responsible for this high rate of reaction?
a.
the pressure of the reactants
c.
concentration of the reactants
b.
temperature
d.
surface area exposed to air
 

 23. 
The letter k in a rate law stands for
a.
a proportionality constant.
c.
temperature.
b.
concentration.
d.
reaction rate.
 

 24. 
In the rate law for the following equation, R=k[A]n[B]m, the units for [A] and [B] are
a.
g-1s-1.
c.
M.
b.
M-1s-1.
d.
Ms-1.
 

 25. 
What symbol in a chemical equation indicates equilibrium?
a.
mc025-1.jpg
c.
mc025-3.jpg
b.
mc025-2.jpg
d.
None of the above
 

 26. 
In the equation mc026-1.jpg, what represents the concentrations of the reactants?
a.
[Y] and [Z]
c.
mc026-2.jpg
b.
[W] and [X]
d.
mc026-3.jpg
 

 27. 
In the equation, mc027-1.jpgwhat represents the concentrations of the products?
a.
[Y] and [Z]
c.
mc027-2.jpg
b.
[W] and [X]
d.
mc027-3.jpg
 

 28. 
If a soluble product forms, a reaction may run to completion
a.
if the product is only slightly ionized.
b.
if the product is highly soluble.
c.
if the product is not gaseous.
d.
under no circumstances.
 

 29. 
Adding sodium acetate to an acetic acid, CH3COOH, solution
a.
increases pH and lowers [H+].
b.
increases pH and raises [H+].
c.
decreases pH and lowers [H+].
d.
decreases pH and raises [H+].
 

 30. 
The cation of the salt of a strong acid and a weak base is the
a.
hydronium ion.
c.
conjugate acid of the weak base.
b.
hydroxide ion.
d.
conjugate base of the strong acid.
 

 31. 
What is the solubility-product constant of barium carbonate, BaCO3? Its solubility is 0.0022 g/100 g H2O. The molar mass of BaCO3 is 197.34 g/mol.
a.
1.2 mc031-3.jpg 10–6
c.
2.2 mc031-5.jpg 10–8
b.
1.2 mc031-4.jpg 10–8
d.
4.4 mc031-6.jpg 10–10
 

 32. 
Calculate the ion product for mixing 50 mL of 0.015 M Ca(NO3)2 with 200 mL of 0.35 M NaOH. Ksp for Ca(OH)2 is 5.5 ´ 10–6. Does a precipitate form?
a.
8.5 ´ 10–7; no
c.
2.4 ´ 10–4; no
b.
8.5 ´ 10–7; yes
d.
2.4 ´ 10–4; yes
 

 33. 
In the reaction represented by the equation F2 + Mg mc033-1.jpg 2F– + Mg2+, which species is oxidized?
a.
F2
c.
Both (a) and (b)
b.
Mg
d.
Neither (a) or (b)
 

 34. 
After balancing the redox equation FeCl2 + KMnO4 + HCl ®
FeCl3 + MnCl2 + H2O + KCl, the coefficients, in order from left to right, are
a.
3, 1, 4, 3, 1, 2, 1.
b.
4, 2, 5, 4, 2, 3, 2.
c.
5, 1, 8, 5, 1, 4, 1.
d.
5, 1, 4, 5, 1, 4, 1.
 

 35. 
Which process deposits metal onto a surface?
a.
electrolysis
c.
autooxidation
b.
electroplating
d.
oxidation
 

 36. 
In a cell used to electroplate silver onto an object, Ag+ is
a.
oxidized at the anode.
c.
oxidized at the cathode.
b.
reduced at the anode.
d.
reduced at the cathode.
 

 37. 
Reactions that affect the nucleus of an atom are called
a.
fusions.
c.
radioactive decays.
b.
fissions.
d.
nuclear reactions.
 

 38. 
Balance the following equation: mc038-1.jpg+ ____ mc038-2.jpg mc038-3.jpg
a.
mc038-4.jpg
c.
mc038-6.jpg
b.
mc038-5.jpg
d.
mc038-7.jpg
 

 39. 
Balance the following equation: mc039-1.jpg+ ____ mc039-2.jpg mc039-3.jpg + mc039-4.jpg
a.
mc039-5.jpg
c.
mc039-7.jpg
b.
mc039-6.jpg
d.
mc039-8.jpg
 

 40. 
Which of the following particles has the same mass as an electron but a positive charge and is sometimes emitted from the nucleus during radioactive decay?
a.
beta particle
c.
positron
b.
alpha particle
d.
gamma ray
 

 41. 
A roentgen equals the amount of radiation that produces
a.
2 mc041-1.jpg 1018 ion pairs in 1 cm3 of dry air.
b.
2 mc041-2.jpg 1019 ion pairs in 1 cm3 of dry air.
c.
2 mc041-3.jpg 108 ion pairs in 1 cm3 of dry air.
d.
2 mc041-4.jpg 109 ion pairs in 1 cm3 of dry air.
 

 42. 
Radioactive nuclides cause molecules in air to
a.
ionize.
c.
condense.
b.
fluoresce.
d.
radiate.
 

 43. 
Each carbon atom in a molecule forms four single covalent bonds with other atoms in a(n)
a.
aromatic hydrocarbon.
c.
structural isomer.
b.
saturated hydrocarbon.
d.
geometric isomer.
 

 44. 
Which statement about London dispersion forces is correct?
a.
Their strength increases as the mass of the molecule increases.
b.
Their strength decreases as the mass of the molecule increases.
c.
Their strength increases as the mass of the molecule decreases.
d.
Their strength does not depend on the mass of the molecule.
 

 45. 
What is the general formula for ethers?
a.
R–O–R'
c.
R–COO–R'
b.
R–COOH
d.
R–CHO
 

 46. 
Which of the following compounds is used in cold creams, body lotions, and lipsticks?
a.
ethanol
c.
glycerol
b.
ethylene glycol
d.
methanol
 

 47. 
The monomer of both starch and cellulose is
a.
an amino acid.
c.
sucrose.
b.
glycogen.
d.
glucose.
 

 48. 
The two most abundant elements found in lipids are
a.
oxygen and carbon.
c.
carbon and hydrogen.
b.
hydrogen and oxygen.
d.
carbon and phosphorus.
 

 49. 
Energy is needed for
a.
catabolic reactions to occur.
c.
digestion to occur.
b.
anabolic reactions to occur.
d.
None of the above
 

 50. 
A gene is a sequence of DNA that holds the code for
a.
self-replication.
b.
the manufacture of a polypeptide.
c.
the manufacture of a carbohydrate.
d.
recombinant technology.
 



 
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