Multiple
Choice
Identify the letter of the choice that best completes the statement or answers the
question.
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1.
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What is the most common
oxidation number of combined oxygen?
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2.
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The algebraic sum of the
oxidation numbers of the atoms in a compound a. | is always
zero. | c. | is always –1. | b. | is always
+1. | d. | can be any whole number. | | | | |
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3.
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What are the oxidation numbers
in the ion SO32–? a. | S = +6, O =
–2 | c. | S = +4, O = –2 | b. | S = +1, O =
–1 | d. | S = 0, O = –1 | | | | |
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4.
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A species whose oxidation
number decreases in a reaction is a. | oxidized. | c. | electrolyzed. | b. | reduced. | d. | autooxidized. | | | | |
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5.
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Pure water
contains a. | water molecules only. | b. | hydronium ions only. | c. | hydroxide ions
only. | d. | water molecules, hydronium ions, and hydroxide
ions. | | |
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6.
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What is the concentration of
H3O+ in pure water? a. | 10–7
M | c. | 55.4 M | b. | 0.7 M | d. | 107 M | | | | |
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7.
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What is the product of
H3O+ and OH– concentrations in water? a. | 10–28 | c. | 10–7 | b. | 10–14 | d. | 55.4 | | | | |
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8.
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Which expression represents the
pH of a solution? a. | log[H3O+] | c. | log[OH–] | b. | –log[H3O+] | d. | –log[OH–] | | | | |
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9.
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If [H3O+]
of a solution is greater than [OH–], the solution a. | is always acidic. | c. | is always neutral. | b. | is always basic. | d. | might be acidic, basic, or neutral. | | | | |
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10.
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The pH scale in general use
ranges from a. | 0 to 1. | c. | 0 to 7. | b. | –1 to
1. | d. | 0 to 14. | | | | |
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11.
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The pH of an acidic solution
is a. | less than 0. | c. | greater than 7. | b. | less than 7. | d. | greater than 14. | | | | |
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12.
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Acids taste a. | sweet. | c. | bitter. | b. | sour. | d. | salty. | | | | |
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13.
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Acetic acid is found in
significant quantities in a. | lemons. | c. | sour milk. | b. | vinegar. | d. | apples. | | | | |
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14.
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Acids generally release
H2 gas when they react with a. | nonmetals. | c. | active metals. | b. | semimetals. | d. | inactive metals. | | | | |
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15.
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Acids make litmus paper
turn a. | red. | c. | blue. | b. | yellow. | d. | black. | | | | |
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16.
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Bases feel a. | rough. | c. | slippery. | b. | moist. | d. | dry. | | | | |
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17.
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The name of a binary
acid a. | has no prefix. | c. | ends with the suffix -ous. | b. | begins with the prefix bi-. | d. | begins with the prefix
hydro-. | | | | |
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18.
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Which of the following is
perchloric acid? a. | HClO | c. | HClO3 | b. | HClO2 | d. | HClO4 | | | | |
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19.
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An acid having the suffix
-ic produces an anion having the a. | suffix
-ate. | c. | prefix hydro-. | b. | suffix
-ite. | d. | suffix -ous. | | | | |
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20.
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A substance that ionizes
(dissociates) nearly completely in aqueous solutions and produces H3O+ is
a a. | weak base. | c. | weak acid. | b. | strong
base. | d. | strong acid. | | | | |
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21.
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How many moles of ions are
produced by the dissociation of 1 mol of NH4Br?
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22.
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When solutions of two ionic
compounds are combined and a solid forms, the process is called a. | hydration. | c. | solvation. | b. | precipitation. | d. | dissociation. | | | | |
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23.
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The formula for the hydronium
ion is a. | H+. | c. | H3O–. | b. | H2O+. | d. | H3O+. | | | | |
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24.
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Which of the following is a
homogeneous mixture? a. | water | c. | whole-wheat
bread | b. | a sugar-water solution | d. | sugar | | | | |
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25.
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All of the following are
homogeneous mixtures EXCEPT a. | sodium
chloride. | c. | gasoline. | b. | a sugar-water
solution. | d. | a salt-water solution. | | | | |
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26.
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Which of the following is an
electrolyte? a. | sodium chloride | c. | water | b. | sugar | d. | glass | | | | |
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27.
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The rule like dissolves like is
used to predict a. | solubility. | c. | reactivity. | b. | equilibrium. | d. | phase. | | | | |
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28.
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At pressures greater than 760
mm Hg, water will boil at a. | a temperature higher than
100ûC. | c. | 100ûC. | b. | a temperature lower than
100ûC. | d. | 4ûC. | | | | |
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29.
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As the atmospheric pressure on
the surface of a liquid decreases, its boiling point a. | decreases. | c. | remains unchanged. | b. | increases. | d. | shows no
correlation. | | | | |
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30.
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What is the boiling point of
water at standard pressure? a. | 100ûC | c. | 212ûC | b. | 112ûC | d. | 200ûC | | | | |
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31.
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At about what temperature does
water reach its maximum density?
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32.
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What is the mass of 1 mL of
water at its temperature of maximum density? a. | 1 mg | c. | 1 g | b. | 1.5 mg | d. | 1.5 g | | | | |
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33.
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Solids have a definite volume
because a. | the particles do not have a tendency to change
positions. | b. | the particles are far apart. | c. | they can be easily compressed. | d. | the energy of the particles is high. | | |
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34.
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The electronegativity
difference between oxygen and hydrogen results in the water molecule being a. | flammable. | c. | ionically bonded. | b. | polar. | d. | linear. | | | | |
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35.
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What is the freezing point of
water at standard pressure?
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36.
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Equal volumes of diatomic gases
under the same conditions of temperature and pressure contain the same number of a. | protons. | c. | molecules. | b. | ions. | d. | Dalton's "ultimate
particles." | | | | |
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37.
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Knowing the mass and volume of
a gas at STP allows one to calculate the a. | identity of the
gas. | c. | condensation point of the gas. | b. | molar mass of the gas. | d. | rate of diffusion of the gas. | | | | |
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38.
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A 1.00 L sample of a gas has a
mass of 0.716 g at STP. What is the molar mass of the gas? a. | 0.716 g/mol | c. | 7.16 g/mol | b. | 1.60 g/mol | d. | 16.0 g/mol | | | | |
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39.
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Which is a common unit for the
ideal gas constant R?
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40.
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What instrument measures
atmospheric pressure? a. | barometer | c. | vacuum pump | b. | manometer | d. | torrometer | | | | |
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41.
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A pressure of 745 mm Hg
equals a. | 745 torr. | c. | 1 pascal. | b. | 1 torr. | d. | 745 pascal. | | | | |
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42.
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Suppose the temperature of the
air in a balloon is increased. If the pressure remains constant, what quantity must
change? a. | volume | c. | compressibility | b. | number of molecules | d. | adhesion | | | | |
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43.
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Who developed the concept that
the total pressure of a mixture of gases is the sum of their partial
pressures? a. | Charles | c. | Kelvin | b. | Boyle | d. | Dalton | | | | |
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Water Vapor
Pressure
Temperature (ûC) | Pressure (mm
Hg) | 0 |
4.6 | 5 |
6.5 | 10 |
9.2 | 15 |
12.8 | 20 |
17.5 | 25 |
23.8 | 30 |
31.8 | 35 |
42.2 | 40 |
55.3 | 50 |
92.5 | | |
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44.
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A sample of nitrogen is
collected by water displacement at 730.0 mm Hg and 20ûC. What is the partial pressure of the
nitrogen? a. | 17.5 mm Hg | c. | 717.2 mm Hg | b. | 712.5 mm
Hg | d. | 747.5 mm Hg | | | | |
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45.
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Which branch of chemistry deals
with the mass relationships of elements in compounds and the mass relationships among reactants and
products in chemical reactions? a. | qualitative
analysis | c. | chemical kinetics | b. | entropy | d. | stoichiometry | | | | |
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46.
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The coefficients in a chemical
equation represent the a. | masses, in grams, of all reactants and
products. | b. | relative numbers of moles of reactants and
products. | c. | number of atoms in each compound in a
reaction. | d. | number of valence electrons involved in the
reaction. | | |
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47.
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For the reaction 2H2
+ O2→ 2H2O, how many moles of water
can be produced from 6.0 mol of oxygen? a. | 2.0 mol | c. | 12 mol | b. | 6.0 mol | d. | 18 mol | | | | |
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48.
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In the reaction A + B
→ C + D, if the quantity of B is insufficient to react with all of
A, a. | A is the limiting reactant. | c. | there is no limiting
reactant. | b. | B is the limiting reactant. | d. | no product can be
formed. | | | | |
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49.
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After the correct formula for a
reactant in an equation has been written, the a. | subscripts are adjusted to balance the
equation. | b. | formula should not be changed. | c. | same formula must appear as the product. | d. | symbols in the formula must not appear on the product side of the
equation. | | |
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50.
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In writing an equation that
produces hydrogen gas, the correct representation of hydrogen gas is
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51.
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What is the small whole number
that appears in front of a formula in a chemical equation? a. | a subscript | c. | a ratio | b. | a
superscript | d. | a coefficient | | | | |
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52.
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Which of the following is a
formula equation for the formation of carbon dioxide from carbon and oxygen? a. | Carbon plus oxygen yields carbon dioxide. | b. | C + O2 →
CO2 | c. | CO2 → C +
O2 | d. | 2C + O →
CO2 | | |
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53.
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In an equation, the symbol for
a substance in water solution is followed by a. | (1). | c. | (aq). | b. | (g). | d. | (s). | | | | |
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54.
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A chemical formula written over
the arrow in a chemical equation signifies a. | a
byproduct. | c. | a catalyst for the reaction. | b. | the formation of a gas. | d. | an impurity. | | | | |
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55.
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Which equation is NOT
balanced? a. | 2H2 + O2 →
2H2O | b. | 4H2 + 2O2
→ 4H2O | c. | H2 + H2 + O2 →
H2O + H2O | d. | 2H2 + O2
→ H2O | | |
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56.
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The equation AX → A + X is the general equation for a a. | synthesis reaction. | c. | combustion reaction. | b. | decomposition reaction. | d. | single-replacement reaction. | | | | |
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57.
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In what kind of reaction does
one element replace a similar element in a compound? a. | single-replacement reaction | c. | decomposition
reaction | b. | double-replacement reaction | d. | ionic reaction | | | | |
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58.
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The equation AX + BY
→ AY + BX is the general equation for a a. | synthesis reaction. | c. | single-replacement reaction. | b. | decomposition reaction. | d. | double-replacement reaction. | | | | |
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59.
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The equation A + X → AX is the general equation for a(n) a. | combustion reaction. | c. | synthesis reaction. | b. | ionic reaction. | d. | double-replacement reaction. | | | | |
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60.
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The decomposition of a
substance by an electric current is called a. | electrolysis. | c. | ionization. | b. | conduction. | d. | transformation. | | | | |
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61.
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When heated, a metal carbonate
decomposes into a metal oxide and a. | carbon. | c. | oxygen. | b. | carbon dioxide. | d. | hydrogen. | | | | |
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62.
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Group 1 metals react with water
to produce metal hydroxides and a. | metal
hydroxides. | c. | oxygen. | b. | hydrochloric
acid. | d. | hydrogen. | | | | |
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63.
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An element in the activity
series can replace any element a. | in the periodic
table. | c. | above it on the list. | b. | below it on the
list. | d. | in its group. | | | | |
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64.
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Which reaction does NOT
occur? a. | 2HF + Cl2 →
F2 + 2HCl | c. | Fe + CuCl2 →
FeCl2 + Cu | b. | 2Na + ZnF2 → 2NaF + Zn | d. | 2HCl + Mg → MgCl2 +
H2 | | | | |
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65.
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What is the formula for zinc
fluoride?
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66.
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What is the oxidation number of
oxygen in most compounds?
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67.
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What is the oxidation number of
an uncombined element?
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68.
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A formula that shows the
simplest whole-number ratio of the atoms in a compound is the a. | molecular formula. | c. | structural formula. | b. | ideal formula. | d. | empirical formula. | | | | |
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69.
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A molecular compound has the
empirical formula XY3. Which of the following is a possible molecular
formula?
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70.
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The molecular formula for
vitamin C is C6H8O6. What is the empirical formula? a. | CHO | c. | C3H4O3 | b. | CH2O | d. | C2H4O2 | | | | |
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71.
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A chemical bond resulting from
the electrostatic attraction between positive and negative ions is called a(n) a. | covalent bond. | c. | charged bond. | b. | ionic bond. | d. | dipole bond. | | | | |
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72.
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The chemical bond formed when
two atoms share electrons is called a(n) a. | ionic
bond. | c. | Lewis structure. | b. | orbital
bond. | d. | covalent bond. | | | | |
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73.
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If the atoms that share
electrons have an unequal attraction for the electrons, the bond is called a. | nonpolar. | c. | ionic. | b. | polar. | d. | dipolar. | | | | |
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74.
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A bond that is less than 5%
ionic is considered a. | polar
covalent. | c. | nonpolar covalent. | b. | ionic. | d. | metallic. | | | | |
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75.
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A neutral group of atoms held
together by covalent bonds is a a. | molecular
formula. | c. | compound. | b. | chemical
formula. | d. | molecule. | | | | |
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76.
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An octet is equal
to
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77.
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The elements of the ____ group
satisfy the octet rule without forming compounds. a. | main | c. | alkali metal | b. | noble gas | d. | alkaline-earth metal | | | | |
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78.
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In SI, the frequency of
electromagnetic radiation is measured in a. | nanometers. | c. | hertz. | b. | quanta. | d. | joules. | | | | |
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79.
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The distance between two
successive peaks on a wave is its a. | frequency. | c. | quantum number. | b. | wavelength. | d. | velocity. | | | | |
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80.
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A line spectrum is produced
when an electron moves from one energy level a. | to a higher energy
level. | b. | to a lower energy level. | c. | into the nucleus. | d. | to another position in the same
sublevel. | | |
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81.
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If electrons in an atom have
the lowest possible energies, the atom is in the a. | ground
state. | c. | excited state. | b. | inert
state. | d. | radiation-emitting state. | | | | |
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82.
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How many quantum numbers are
needed to describe the energy state of an electron in an atom?
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83.
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The p orbitals are
shaped like a. | electrons. | c. | dumbbells. | b. | circles. | d. | spheres. | | | | |
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84.
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If 8 electrons completely fill
a main energy level, what is n?
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85.
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The atomic sublevel with the
next highest energy after 4p is
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86.
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The element with electron
configuration 1s2 2s2 2p6 3s2
3p2 is a. | Mg (Z =
12). | c. | S (Z = 16). | b. | C (Z =
6). | d. | Si (Z = 14). | | | | |
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87.
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What is the electron
configuration for nitrogen, atomic number 7? a. | 1s2
2s2 2p3 | c. | 1s2
2s3 2p1 | b. | 1s2 2s3
2p2 | d. | 1s2 2s2 2p2
3s1 | | | | |
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88.
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According to the law of
definite proportions, any two samples of KCl have a. | the same
mass. | c. | the same melting point. | b. | slightly different molecular
structures. | d. | the same ratio of elements. | | | | |
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89.
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Who was the schoolmaster who
studied chemistry and proposed an atomic theory? a. | John
Dalton | c. | Robert Brown | b. | Jons
Berzelius | d. | Dmitri Mendeleev | | | | |
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90.
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Who discovered the nucleus by
bombarding gold foil with positively charged particles and noting that some particles were widely
deflected? a. | Rutherford | c. | Chadwick | b. | Dalton | d. | Bohr | | | | |
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91.
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A nuclear particle that has
about the same mass as a proton, but with no electrical charge, is called a(n) a. | nuclide. | c. | electron. | b. | neutron. | d. | isotope. | | | | |
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92.
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Protons within a nucleus are
attracted to each other by a. | nuclear
forces. | c. | their energy levels. | b. | opposite
charges. | d. | electron repulsion. | | | | |
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93.
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An atom is electrically neutral
because a. | neutrons balance the protons and electrons. | b. | nuclear forces stabilize the charges. | c. | the numbers of protons and electrons are equal. | d. | the numbers of protons and neutrons are equal. | | |
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94.
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Most of the volume of an atom
is occupied by the a. | nucleus. | c. | electron cloud. | b. | nuclides. | d. | protons. | | | | |
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95.
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Atoms of the same element that
have different masses are called a. | moles. | c. | nuclides. | b. | isotopes. | d. | neutrons. | | | | |
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96.
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All atoms of the same element
have the same a. | atomic mass. | c. | mass number. | b. | number of neutrons. | d. | atomic number. | | | | |
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97.
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In determining atomic mass
units, the standard is the a. | C-12 atom. | c. | H-1 atom. | b. | C-14 atom. | d. | O-16 atom. | | | | |
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98.
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An atom of potassium has 19
protons and 20 neutrons. What is its mass number?
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99.
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The number of atoms in 1 mol of
carbon is a. | 6.022 ×
1022. | c. | 5.022 ×
1022. | b. | 6.022 ×
1023. | d. | 5.022 ×
1023. | | | | |
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100.
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The mass of two moles of oxygen
atoms (atomic mass 16 amu) is a. | 16 g. | c. | 48 g. | b. | 32 g. | d. | 64 g. | | | | |
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101.
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The mass of 2.50 mol of calcium
atoms (atomic mass 40.08 amu) is approximately a. | 10.0 g. | c. | 100 g. | b. | 42.5 g. | d. | 250 g. | | | | |
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102.
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The SI standard units for
length and mass are a. | centimeter and
gram. | c. | centimeter and kilogram. | b. | meter and
gram. | d. | meter and kilogram. | | | | |
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103.
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The symbol mm
represents a. | micrometer. | c. | milliliter. | b. | millimeter. | d. | meter. | | | | |
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104.
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The quantity of matter per unit
volume is a. | mass. | c. | inertia. | b. | weight. | d. | density. | | | | |
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105.
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A measure of Earth's
gravitational pull on matter is a. | density. | c. | volume. | b. | weight. | d. | mass. | | | | |
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106.
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The mass of a 5.00
cm3 sample of clay is 11 g. What is the density of the clay? a. | 0.45 g/cm3 | c. | 6 g/cm3 | b. | 2.2 g/cm3 | d. | 55 g/cm3 | | | | |
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107.
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30ûC
equals a. | –243.15 K. | c. | 243.15 K. | b. | 9.1 K. | d. | 303.15 K. | | | | |
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108.
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To two significant figures, the
measurement 0.0255 g should be reported as a. | 0.02 g. | c. | 0.026 g. | b. | 0.025 g. | d. | 2.5 × 102
g. | | | | |
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109.
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The number of significant
figures in the measurement 0.000 305 kg is
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110.
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The study of matter and changes
in matter best describes the science of a. | biology. | c. | microbiology. | b. | physics. | d. | chemistry. | | | | |
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111.
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The state of matter in which a
material has neither a definite shape nor a definite volume is the a. | gaseous state. | c. | elemental state. | b. | liquid state. | d. | solid state. | | | | |
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112.
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A vertical column of blocks in
the periodic table is called a(n) a. | group. | c. | property. | b. | period. | d. | octet. | | | | |
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113.
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The elements that border the
zigzag line in the periodic table are a. | inactive. | c. | metalloids. | b. | metals. | d. | nonmetals. | | | | |
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114.
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What is the symbol for the
silvery substance that coated (or was supposed to coat) the inside surface of the tube in the SILVER
mirror lab?
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115.
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The following footwear is
best in the laboratory. a. | sandals | b. | open-toed
shoes | c. | closed-toed shoes | d. | shoes appropriate for the weather | | | | | | | | |
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116.
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Oxidation is the ___?___ of
electrons? a. | gain | b. | loss | c. | destruction | | | | | | |
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117.
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What is the oxidation number of
a monatomic ion? a. | 0 | c. | its charge | b. | +1 | d. | its number of
electrons | | | | |
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118.
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What is the most common
oxidation number of combined hydrogen?
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119.
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What are the oxidation numbers
in the compound KCl? a. | K = 0, Cl =
0 | c. | K = +1, Cl = –1 | b. | K = –1, Cl =
+1 | d. | K = +2, Cl = –2 | | | | |
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120.
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What are the oxidation numbers
in the compound NO2? a. | N = +2, O =
–1 | c. | N = –2, O = +1 | b. | N = +2, O =
–2 | d. | N = +4, O = –2 | | | | |
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121.
|
In a reduction, atoms or
ions a. | increase their oxidation number. | b. | decrease their oxidation number. | c. | do not change their oxidation number. | d. | have a zero oxidation number after the reaction. | | |
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122.
|
A reaction in which products
can react to re-form reactants is a. | at
equilibrium. | c. | buffered. | b. | reversible. | d. | impossible. | | | | |
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|
123.
|
If [H3O+]
of a solution is less than [OH–], the solution a. | is always acidic. | c. | is always neutral. | b. | is always basic. | d. | might be acidic, basic, or neutral. | | | | |
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|
124.
|
What is the pH of a neutral
solution at 25ûC?
|
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|
125.
|
The pH of a basic solution
is a. | less than 0. | c. | greater than 7. | b. | less than 7. | d. | greater than 14. | | | | |
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126.
|
A water solution whose pH is
10 a. | is always neutral. | c. | is always acidic. | b. | is always basic. | d. | might be neutral, basic, or acidic. | | | | |
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127.
|
To calculate the pH of a
solution whose [OH–] is known, first calculate a. | [H3O+]. | c. | antilog[H3O+]. | b. | log[OH–]. | d. | [H2O]. | | | | |
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|
128.
|
What is the pH of a
10–5 M KOH solution?
|
|
|
129.
|
If [H3O+]
= 1.7 × 10–3 M, what is the pH
of the solution?
|
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|
130.
|
What is the pH of a solution
whose hydronium ion concentration is 5.03 ×
10–1 M? a. | 0.2984 | c. | 1.542 | b. | 0.5133 | d. | 5.031 | | | | |
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|
131.
|
Acids react
with a. | bases to produce salts and water. | c. | water to produce bases and
salts. | b. | salts to produce bases and water. | d. | neither bases, salts, nor
water. | | | | |
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132.
|
Bases taste a. | soapy. | c. | sweet. | b. | sour. | d. | bitter. | | | | |
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133.
|
Bases make litmus paper
turn a. | blue. | c. | yellow. | b. | red. | d. | black. | | | | |
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|
134.
|
A binary acid
contains a. | two hydrogen atoms. | c. | hydrogen and two other
elements. | b. | hydrogen and one other element. | d. | hydrogen and three other
elements. | | | | |
|
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|
135.
|
Which of the following is a
binary acid? a. | H2SO4 | c. | HBr | b. | CH3COOH | d. | NaOH | | | | |
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|
136.
|
Compared with acids that have
the suffix -ic, acids that have the suffix -ous contain a. | more hydrogen. | c. | less oxygen. | b. | more oxygen. | d. | the same amount of oxygen. | | | | |
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|
137.
|
What acid is produced in the
stomach? a. | hydrochloric acid | c. | nitric acid | b. | phosphoric acid | d. | sulfuric acid | | | | |
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|
138.
|
What acid is found in
vinegar? a. | acetic acid | c. | phosphoric acid | b. | nitric acid | d. | hydrochloric acid | | | | |
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|
139.
|
What is an Arrhenius
acid? a. | a chemical compound that increases the concentration of hydrogen ions in aqueous
solution | b. | a chemical compound that increases the concentration of hydroxide ions
in aqueous solution | c. | a chemical compound that decreases the
concentration of hydrogen ions in aqueous solution | d. | a chemical compound that decreases the concentration of hydroxide ions in aqueous
solution | | |
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|
140.
|
Which of the following is NOT a
strong acid? a. | HNO3 | c. | H2SO4 | b. | CH3COOH | d. | HCl | | | | |
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|
141.
|
A Brønsted-Lowry acid
is a. | an electron-pair acceptor. | c. | a proton acceptor. | b. | an electron-pair donor. | d. | a proton donor. | | | | |
|
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|
142.
|
Which compound is produced by a
neutralization? a. | H2O(l) | c. | Ca(OH)2(s) | b. | HNO3(aq) | d. | H3PO4(aq) | | | | |
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|
143.
|
Which of the following is a
pure substance? a. | water | c. | soil | b. | milk | d. | concrete | | | | |
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144.
|
Which of the following is a
heterogeneous mixture? a. | water | c. | whole-wheat
bread | b. | a sugar-water solution | d. | sugar | | | | |
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145.
|
A metal solution is
a(n) a. | colloid. | c. | suspension. | b. | alloy. | d. | electrolyte. | | | | |
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146.
|
To conduct electricity, a
solution must contain a. | nonpolar
molecules. | c. | ions. | b. | polar
molecules. | d. | free electrons. | | | | |
|
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|
147.
|
In the expression like
dissolves like, the word like refers to similarity in molecular a. | mass. | c. | energy. | b. | size. | d. | polarity. | | | | |
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|
148.
|
Compared with the particles in
a gas, the particles in a liquid a. | have more
energy. | c. | move around less. | b. | are
larger. | d. | are farther apart. | | | | |
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149.
|
The compressibility of a liquid
is generally a. | less than that of a gas. | c. | equal to that of a
gas. | b. | more than that of a gas. | d. | zero. | | | | |
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150.
|
What is
vaporization? a. | the process by which a liquid changes to a
gas | b. | the process by which a solid changes to a
gas | c. | both a and b | d. | neither a nor b | | |
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151.
|
Which term best describes the
process by which particles escape from the surface of a nonboiling liquid and enter the gas
state? a. | vaporization | c. | surface tension | b. | evaporation | d. | aeration | | | | |
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152.
|
What is the physical change of
a liquid to a solid by the removal of heat? a. | solidification | c. | freezing | b. | particle
arrangement | d. | both a and c | | | | |
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|
153.
|
Particles within a
solid a. | do not move. | c. | vibrate energetically. | b. | vibrate weakly about fixed positions. | d. | exchange positions
easily. | | | | |
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|
154.
|
If 0.5 L of
O2(g) reacts with H2 to produce 1 L of H2O(g), what is
the volume of H2O(g) obtained from 1 L of O2(g)? a. | 0.5 L | c. | 2 L | b. | 1.5 L | d. | Cannot be
determined | | | | |
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|
155.
|
In the equation C +
O2(g) → CO2(g), one volume of
O2 yields how many volumes of CO2?
|
|
|
156.
|
If gas A has a molar mass
greater than that of gas B and samples of each gas at identical temperatures and pressures contain
equal numbers of molecules, then a. | the volumes of gas A and gas B are
equal. | b. | the volume of gas A is greater than that of gas
B. | c. | the volume of gas B is greater than that of gas
A. | d. | their volumes are proportional to their molar
masses. | | |
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|
157.
|
At constant temperature and
pressure, gas volume is directly proportional to the a. | molar mass of the gas. | c. | density of the gas at STP. | b. | number of moles of gas. | d. | rate of diffusion. | | | | |
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|
158.
|
The standard molar volume of a
gas is all of the following except a. | the volume occupied by 1 mol of a gas at
STP. | b. | equal for all gases under the same
conditions. | c. | 22.4 L at STP. | d. | dependent upon the size of the molecules. | | |
|
|
|
159.
|
The standard molar volume of a
gas at STP is all of the following except a. | the volume occupied by 1 mol of the
gas. | b. | 22.4 g. | c. | 22.4 L. | d. | the volume occupied by one molar mass of the gas. | | |
|
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|
160.
|
At STP, the standard molar
volume of a gas of known volume can be used to calculate the a. | number of moles of gas. | c. | gram-molecular weight. | b. | rate of diffusion. | d. | gram-molecular volume. | | | | |
|
|
|
161.
|
What is the molar mass of gas
at STP? a. | density of the gas multiplied by the mass of 1
mol | b. | density of the gas divided by the mass of 1
mol | c. | density of the gas multiplied by 22.4 L | d. | density of the gas divided by 22.4 L | | |
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|
|
162.
|
A 1.00 L sample of a gas has a
mass of 1.7 g at STP. What is the molar mass of the gas? a. | 0.076 g/mol | c. | 38 g/mol | b. | 13.2 g/mol | d. | 170 g/mol | | | | |
|
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|
163.
|
All of the following equations
are statements of the ideal gas law except
|
|
|
164.
|
Calculate the approximate
volume of a 0.600 mol sample of gas at 15.0ûC and a pressure of 1.10 atm. a. | 12.9 L | c. | 24.6 L | b. | 22.4 L | d. | 129 L | | | | |
|
|
|
165.
|
What is the approximate volume
of gas in a 1.50 mol sample that exerts a pressure of 0.922 atm and has a temperature of
10.0ûC? a. | 13 L | c. | 37.8 L | b. | 14.2 L | d. | 378 L | | | | |
|
|
|
166.
|
In the reaction 2C +
O2(g) → 2CO(g), what is the volume ratio
of O2 to CO?
|
|
|
167.
|
In the reaction
H2(g) + Cl2(g) → 2HCl,
what is the volume ratio of Cl2 to HCl?
|
|
|
168.
|
The equation for the production
of methane is C + 2H2(g) →
CH4(g). How many liters of hydrogen are needed to produce 20 L of
methane? a. | 2.0 L | c. | 22.4 L | b. | 20 L | d. | 40 L | | | | |
|
|
|
169.
|
When hydrogen burns, water
vapor is produced. The equation is 2H2(g) + O2(g) → 2H2O(g). If 12 L of oxygen are consumed, what volume of water vapor
is produced?
|
|
|
170.
|
For the complete combustion of
100. L of CO, the volume of oxygen required is a. | 23.8 L | c. | 238 L | b. | 50.0 L | d. | 500. L | | | | |
|
|
|
171.
|
Iron oxide, FeO2, is
produced by the reaction Fe + O2 →
FeO2 (87.8 g/mol). How many grams of FeO2 can be produced from 50 L of
O2 at STP? a. | 19.5 g | c. | 50 g | b. | 37.8 g | d. | 196. g | | | | |
|
|
|
172.
|
What is the definition of
pressure? a. | | b. | | c. | pressure = force ×
area | d. | | | |
|
|
|
173.
|
Convert the pressure 0.840 atm
to mm Hg. a. | 365 mm Hg | c. | 638 mm Hg | b. | 437 mm Hg | d. | 780 mm Hg | | | | |
|
|
|
174.
|
Convert the pressure 1.30 atm
to kPa. a. | 2 kPa | c. | 132 kPa | b. | 115 kPa | d. | 245 kPa | | | | |
|
|
|
175.
|
Standard temperature is
exactly a. | 100ûC. | c. | 0ûC. | b. | 273ûC. | d. | 0 K. | | | | |
|
|
|
176.
|
Standard pressure is
exactly a. | 1 atm. | c. | 101.325 atm. | b. | 760 atm. | d. | 101 atm. | | | | |
|
|
|
177.
|
Pressure and volume changes at
a constant temperature can be calculated using a. | Boyle's
law. | c. | Kelvin's law. | b. | Charles's
law. | d. | Dalton's law. | | | | |
|
|
|
178.
|
A 180.0 mL volume of gas is
measured at 87.0ûC. If the pressure remains unchanged, what is the volume of the gas at
standard temperature? a. | 0.0 mL | c. | 136 mL | b. | 0.5 mL | d. | 410 mL | | | | |
|
|
|
179.
|
On a cold winter morning when
the temperature is –13ûC, the air pressure in an automobile tire is 1.5 atm. If the
volume does not change, what is the pressure after the tire has warmed to
15ûC? a. | –1.5 atm | c. | 3.0 atm | b. | 1.7 atm | d. | 19.5 atm | | | | |
|
|
|
180.
|
If V, P, and
T represent the original volume, pressure, and temperature in the correct units, and
V', P', and T' represent the new conditions, what is the combined gas
law?
|
|
|
181.
|
To correct for the partial
pressure of water vapor, the vapor pressure of H2O at the collecting temperature
is a. | divided by 22.4. | c. | subtracted from the total gas pressure. | b. | multiplied by 22.4. | d. | added to the total gas pressure. | | | | |
|
|
|
182.
|
If five gases in a cylinder
each exert 1 atm, what is the total pressure exerted by the gases? a. | 0.2 atm | c. | 1 atm | b. | 0.5 atm | d. | 5 atm | | | | |
|
|
|
183.
|
A balanced chemical equation
allows one to determine the a. | mole ratio of any two substances in the
reaction. | b. | energy released in the reaction. | c. | electron configuration of all elements in the reaction. | d. | mechanism involved in the reaction. | | |
|
|
|
184.
|
In the chemical reaction wA +
xB → yC + zD, a comparison of the number of moles of A to the number of
moles of C would be a(n) a. | mass
ratio. | c. | electron ratio. | b. | mole
ratio. | d. | energy proportion. | | | | |
|
|
|
185.
|
In the reaction
2Al2O3 → 4Al + 3O2, what is the mole
ratio of aluminum to oxygen?
|
|
|
186.
|
In the reaction 2H2
+ O2 → 2H2O, what is the mole ratio
of oxygen to water?
|
|
|
187.
|
In the equation
2KClO3 → 2KCl + 3O2, how many moles of
oxygen are produced when 3.0 mol of KClO3 decompose completely? a. | 1.0 mol | c. | 3.0 mol | b. | 2.5 mol | d. | 4.5 mol | | | | |
|
|
|
188.
|
For the reaction C +
2H2 → CH4, how many moles of
hydrogen are required to produce 10 mol of methane, CH4? a. | 2 mol | c. | 10 mol | b. | 4 mol | d. | 20 mol | | | | |
|
|
|
Element | Symbol | Atomic
mass | Bromine | Br | 79.904 | Calcium | Ca | 40.078 | Carbon | C | 12.011 | Chlorine | Cl | 35.4527 | Cobalt | Co | 58.933 20 | Copper | Cu | 63.546 | Fluorine | F | 18.998 4032 | Hydrogen | H | 1.007 94 | Iodine | I | 126.904 | Iron | Fe | 55.847 | Lead | Pb | 207.2 | Magnesium | Mg | 24.3050 | Mercury | Hg | 200.59 | Nitrogen | N | 14.006 74 | Oxygen | O | 15.9994 | Potassium | K | 39.0983 | Sodium | Na | 22.989 768 | Sulfur | S | 32.066 | | | |
|
|
|
189.
|
For the reaction 2H2
+ O2 → 2H2O, how many grams of water
are produced from 6.00 mol of hydrogen? a. | 2.00 g | c. | 54.0 g | b. | 6.00 g | d. | 108 g | | | | |
|
|
|
190.
|
For the reaction SO3
+ H2O → H2SO4, how many
grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid? a. | 80.0 g | c. | 240. g | b. | 160. g | d. | 320. g | | | | |
|
|
|
191.
|
In the chemical equation wA +
xB → yC + zD, if one knows the mass of A and the molar masses of A, B, C,
and D, one can determine a. | the mass of any of the reactants or
products. | b. | the mass of B only. | c. | the total mass of C and D only. | d. | the total mass of A and B only. | | |
|
|
|
192.
|
A chemical reaction involving
substances A and B stops when B is completely used. B is the a. | excess reactant. | c. | primary reactant. | b. | limiting reactant. | d. | primary product. | | | | |
|
|
|
193.
|
A chemical reaction has NOT
occurred if the products have a. | the same mass as the
reactants. | b. | less total bond energy than the reactants. | c. | more total bond energy than the reactants. | d. | the same chemical properties as the reactants. | | |
|
|
|
194.
|
Which observation does NOT
indicate that a chemical reaction has occurred? a. | formation of a
precipitate | c. | evolution of heat and light | b. | production of a
gas | d. | change in total mass of substances | | | | |
|
|
|
195.
|
A solid produced by a chemical
reaction in solution that separates from the solution is called a. | a precipitate. | c. | a molecule. | b. | a
reactant. | d. | the mass of the product. | | | | |
|
|
|
196.
|
To balance a chemical equation,
it may be necessary to adjust the a. | coefficients. | c. | formulas of the products. | b. | subscripts. | d. | number of products. | | | | |
|
|
|
197.
|
How would oxygen be represented
in the formula equation for the reaction of methane and oxygen to yield carbon dioxide and
water?
|
|
|
198.
|
Which coefficients correctly
balance the formula equation NH4NO2(s)→ N2(g) + H2O(l)? a. | 1, 2, 2 | c. | 2, 1, 1 | b. | 1, 1, 2 | d. | 2, 2, 2 | | | | |
|
|
|
199.
|
Which coefficients correctly
balance the formula equation CaO + H2O →
Ca(OH)2? a. | 2, 1, 2 | c. | 1, 2, 1 | b. | 1, 2, 3 | d. | 1, 1, 1 | | | | |
|
|
|
200.
|
After the first steps in
writing an equation, the equation is balanced by a. | adjusting subscripts to the
formula(s). | b. | adjusting coefficients to the smallest whole-number
ratio. | c. | changing the products formed. | d. | making the number of reactants equal to the number of
products. | | |
|
|
|
201.
|
In what kind of reaction do two
or more substances combine to form a new compound? a. | decomposition reaction | c. | double-replacement reaction | b. | ionic reaction | d. | synthesis reaction | | | | |
|
|
|
202.
|
In what kind of reaction does a
single compound produce two or more simpler substances? a. | decomposition reaction | c. | single-replacement reaction | b. | synthesis reaction | d. | ionic reaction | | | | |
|
|
|
203.
|
The equation A + BX
→ AX + B is the general equation for a a. | double-replacement reaction. | c. | single-replacement
reaction. | b. | decomposition reaction. | d. | combustion
reaction. | | | | |
|
|
|
204.
|
The reaction 2Mg(s) +
O2(g) → 2MgO(s) is a a. | synthesis reaction. | c. | single-replacement reaction. | b. | decomposition reaction. | d. | double-replacement reaction. | | | | |
|
|
|
205.
|
The reaction 2HgO(s)
→ 2Hg(l) + O2(g) is a(n) a. | single-replacement reaction. | c. | ionic reaction. | b. | synthesis reaction. | d. | decomposition reaction. | | | | |
|
|
|
206.
|
The reaction
Cl2(g) + 2KBr(aq) →
2KCl(aq) + Br2(l) is a(n) a. | synthesis reaction. | c. | single-replacement reaction. | b. | ionic reaction. | d. | combustion reaction. | | | | |
|
|
|
207.
|
Oxides of active metals, such
as CaO, react with water to produce a. | metal
carbonates. | c. | acids. | b. | metal
hydrides. | d. | metal hydroxides. | | | | |
|
|
|
208.
|
An active metal and a halogen
react to form a(n) a. | salt. | c. | acid. | b. | hydroxide. | d. | oxide. | | | | |
|
|
|
209.
|
When a metal chlorate is
heated, it decomposes to yield a metal chloride and a. | a metal oxide. | c. | hydrogen. | b. | a metal
hydroxide. | d. | oxygen. | | | | |
|
|
|
210.
|
Some acids, such as carbonic
acid, decompose to nonmetal oxides and a. | water. | c. | oxygen. | b. | a salt. | d. | peroxide. | | | | |
|
|
|
211.
|
An insoluble gas that forms in
a double-replacement reaction in aqueous solution a. | bubbles out of
solution. | c. | disassociates into ions. | b. | forms a
precipitate. | d. | reacts with the water. | | | | |
|
|
|
212.
|
In a double-replacement
reaction, hydrogen chloride and sodium hydroxide react to produce sodium chloride. Another product
is a. | sodium hydride. | c. | water. | b. | potassium
chloride. | d. | hydrogen gas. | | | | |
|
|
|
213.
|
Active metals react with
certain acids, such as hydrochloric acid, to yield a metal compound and a. | oxygen. | c. | chlorine. | b. | hydrogen. | d. | sodium. | | | | |
|
|
|
214.
|
A precipitate forms in a
double-replacement reaction when a. | hydrogen gas reacts with a
metal. | c. | water boils out of the solution. | b. | positive ions combine with negative ions. | d. | a gas escapes. | | | | |
|
|
|
215.
|
Predict the product of the
following reaction: MgO + CO2 → a. | MgCO3 | c. | MgC + O3 | b. | Mg + CO3 | d. | MgCO2 + O | | | | |
|
|
|
216.
|
If chlorine gas is produced by
halogen replacement, the other halogen in the reaction must be a. | bromine. | c. | astatine. | b. | iodine. | d. | fluorine. | | | | |
|
|
|
217.
|
What is the balanced equation
when aluminum reacts with copper(II) sulfate? a. | Al + Cu2S → Al2S + Cu | c. | Al + CuSO4 →
AlSO4 + Cu | b. | 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu | d. | 2Al + Cu2SO4
→ Al2SO4 + 2Cu | | | | |
|
|
|
218.
|
What is the name of a list of
elements arranged according to the ease with which they undergo certain chemical
reactions? a. | reactivity list | c. | activity series | b. | reaction sequence | d. | periodic list | | | | |
|
|
|
219.
|
A chemical formula includes the
symbols of the elements in the compound and subscripts that indicate a. | the number of moles in each element. | b. | how many atoms or ions of each type are combined in the simplest
unit. | c. | the formula mass. | d. | the charges on the elements or ions. | | |
|
|
|
220.
|
Changing a subscript in a
correctly written chemical formula a. | changes the number of moles represented by
the formula. | b. | changes the charges on the other ions in the
compound. | c. | changes the formula so that it no longer represents that
compound. | d. | has no effect on the formula. | | |
|
|
|
221.
|
The formula for carbon dioxide,
CO2, can represent a. | one molecule of carbon
dioxide. | c. | one molar mass of carbon dioxide. | b. | 1 mol of carbon dioxide molecules. | d. | all of the
above. | | | | |
|
|
|
222.
|
Which formula does NOT
represent a molecule? a. | H2O
(water) | c. | CO2 (carbon dioxide) | b. | NH3 (ammonia) | d. | NaCl (table salt) | | | | |
|
|
|
223.
|
What is the formula for the
compound formed by calcium ions and chloride ions? a. | CaCl | c. | CaCl3 | b. | Ca2Cl | d. | CaCl2 | | | | |
|
|
|
224.
|
What is the formula for tin(IV)
chromate? a. | Sn(CrO4)4 | c. | Sn2(CrO4)4 | b. | Sn2(CrO4)2 | d. | Sn(CrO4)2 | | | | |
|
|
|
225.
|
Name the compound
Ni(ClO3)2. a. | nickel
chlorate | c. | nickel chlorite | b. | nickel
chloride | d. | nickel peroxide | | | | |
|
|
|
226.
|
Name the compound
Zn3(PO4)2. a. | zinc potassium
oxide | c. | zinc phosphate | b. | trizinc
polyoxide | d. | zinc phosphite | | | | |
|
|
|
227.
|
Name the compound
KClO3. a. | potassium chloride | c. | potassium
chlorate | b. | potassium trioxychlorite | d. | hypochlorite | | | | |
|
|
|
228.
|
What is the name of
Sn3(PO4)4 under the Stock system of nomenclature? a. | stannous phosphate | c. | tin(III) phosphate | b. | tin(IV) phosphate | d. | tin(II) phosphate | | | | |
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229.
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Name the compound
SiO2. a. | silver oxide | c. | silicon dioxide | b. | silicon oxide | d. | monosilicon dioxide | | | | |
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230.
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Name the compound
N2O4. a. | sodium
tetroxide | c. | nitrous oxide | b. | dinitrogen
tetroxide | d. | binitrogen oxide | | | | |
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231.
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What is the formula for
dinitrogen trioxide?
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232.
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What is the formula for
diphosphorous pentoxide? a. | P2PeO5 | c. | P2O4 | b. | PO5 | d. | P2O5 | | | | |
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233.
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The oxidation number of
fluorine is a. | always 0. | b. | –1 in all
compounds | c. | +1 in all compounds. | d. | equal to the positive charge of all the metal ions in a
compound. | | |
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234.
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In a compound, the algebraic
sum of the oxidation numbers of all atoms equals a. | 0. | c. | 8. | b. | 1. | d. | the charge on the compound. | | | | |
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235.
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What is the oxidation number of
hydrogen in most compounds? a. | –1 | b. | 0 | c. | +1 | d. | It is equal to the algebraic sum of the oxidation numbers of the
nonmetals. | | |
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236.
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What is the oxidation number of
hydrogen in H2O?
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237.
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What is the oxidation number of
sulfur in H2SO4?
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238.
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The molar mass of an element is
the mass of one a. | atom of the element. | c. | gram of the
element. | b. | liter of the element. | d. | mole of the
element. | | | | |
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239.
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What is the formula mass of
(NH4)2SO4? a. | 114.09 amu | c. | 128.06 amu | b. | 118.34 amu | d. | 132.13 amu | | | | |
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240.
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The molar mass of
H2O is 18.015 g/mol. How many grams of H2O are present in 0.20
mol? a. | 0.2 g | c. | 35.9 g | b. | 3.6 g | d. | 89.9 g | | | | |
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241.
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The molar mass of LiF is 25.94
g/mol. How many moles of LiF are present in 10.37 g? a. | 0.3998 mol | c. | 2.500 mol | b. | 1.333 mol | d. | 36.32 mol | | | | |
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242.
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How many OH–
ions are present in 3.00 mol of Ca(OH)2? a. | 3.00 | c. | 3.61 × 1024 | b. | 6.00 | d. | 2.06 × 1023 | | | | |
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243.
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How many oxygen atoms are there
in 0.5 mol of CO2? a. | 6.02 ×
1023 | c. | 15.9994 | b. | 3.01 ×
1023 | d. | 11 | | | | |
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244.
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What is the percentage
composition of CF4? a. | 20% C, 80%
F | c. | 16.8% C, 83.2% F | b. | 13.6% C, 86.4%
F | d. | 81% C, 19% F | | | | |
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245.
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What is the percentage
composition of chlorine in NaCl? a. | 35.45% | c. | 60.7% | b. | 50% | d. | 64.5% | | | | |
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246.
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What is the empirical formula
for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen? a. | KClO2 | c. | K2Cl2O3 | b. | KClO3 | d. | K2Cl2O5 | | | | |
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Short
Answer
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247.
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Use the following equation to
explain acid rain: SO3(g) + H2O(l) → H2SO4(aq)
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Problem
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248.
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Find
[H3O+] for a soft drink whose pH is 3.20.
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Essay
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249.
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Write the balanced chemical
equation for the reaction bewteen water and sodium metal. Assume Na is a solid and the water
used is a liquid.
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250.
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Consider your time and efforts
relative to the study of chemistry. If you could magically change the past, what would you do
in order to be a better chemistry student? Your answer will not be counted wrong as long as you
make what Mr. Norris considers to be a respectable answer.
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