Chapter 6, States of Matter: Gases, Liquids, and Solids 1.
Which two states of matter are the least compressible?
Ans. 2.
solids and liquids What device is used to measure atmospheric pressure?
Ans. 3.
barometer The pascal (Pa) is a unit for expressing what quantity?
Ans. 4.
pressure What experimental quantity measures force per unit area?
Ans. 5.
pressure State Boyle's Law.
Ans.
The volume of a gas is inversely proportional to the pressure, if the number of moles (or mass) and the temperature of the gas are kept constant. State Charles's Law.
6. Ans.
7. Ans. 8.
The volume of a gas is directly proportional to the absolute temperature, if the number of moles (or mass) and the pressure of the gas are kept constant. State Avogadro's Law. Equal volumes of any ideal gas, at the same temperature and pressure, contain the same number of moles. What law predicts the expansion of a balloon when helium is added?
Ans. 9.
Avogadro's Consider 1.00 L of air in a patient's lungs at 37.0°C and 1.00 atm pressure. What volume would this air occupy if it were at 25.0°C under a pressure of 5.00 × 102 atm (a typical pressure in a compressed air cylinder)?
Ans. 10.
19.2 × 10-3 L If a gas sample is at STP (Standard Temperature and Pressure), what are its temperature and pressure?
Ans. 11.
temperature = 0.0°C or 273 K, pressure = 1.00 atm. Calculate the density of oxygen gas (O2) at STP, in g/L. [Use molar mass: O2, 32.0 g/mol]
Ans. 12.
1.43 g/L What is the volume (L) occupied by a mole of an ideal gas, if the pressure is 626 mmHg and the temperature is 25.0°C?
Ans. 13.
29.7 L Who found that a mixture of gases exerts a total pressure that is the sum of the pressures that each gas would exert if each were present alone under similar conditions?
Ans.
Dalton
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Chapter 6, States of Matter: Gases, Liquids, and Solids 14.
An gas sample is prepared in which the components have the following partial pressures: nitrogen, 555 mmHg; oxygen, 149 mmHg; water vapor, 13 mmHg; argon, 7 mmHg. What is the total pressure of this mixture?
Ans. 15.
724 mmHg What is the name of the theory which deals with particle behavior in the gas phase?
Ans. 16.
kinetic molecular theory Choose the best one from each pair in the following sentence: The closest approach to ideal gas behavior will be shown by (NH3 or H2?) at (low or high?) pressure and (low or high?) temperature.
Ans. 17.
H2, low, high What is meant by viscosity?
Ans. 18.
It is the resistance of a liquid to flow. What experimental quantity is a measure of the attractive forces between molecules at the surface of a liquid?
Ans. 19.
surface tension What process is responsible for the formation of dew on the grass early in the morning?
Ans. 20.
condensation How can pure water be made to boil at a temperature above 100°C?
Ans. 21.
by raising the pressure to more than one atmosphere Who postulated the existence of temporary dipole attraction among nonpolar molecules?
Ans. 22.
Fritz London What are the general structural requirements for a compound to display hydrogen bonding?
Ans.
It must have hydrogen atoms bonded to small, electronegative atoms such as N, O or F. Why is hydrogen bonding more extensive in water than in hydrogen fluoride?
23.
Ans.
24. Ans.
Each water molecule has two δ+ sites and two δ- sites, all of which can be used for hydrogen bonding. The hydrogen fluoride has three δ- sites but only one δ+ site, and the shortage of the latter limits the number of hydrogen bonds which can form per molecule to half the number in water. Name the four main types of crystalline solid, and give an example of each. ionic solid, NaCl; covalent solid, diamond; molecular solid, ice; metallic solid, iron.
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Chapter 6, States of Matter: Gases, Liquids, and Solids 25.
A barometer measures
A. B. C. D. E. Ans. 26.
D Who invented the first barometer?
A. B. C. D. E. Ans. 27.
14.7 mm Hg 380 mm Hg 760 mm Hg 0.333 mm Hg 30 mm Hg
C Which one of the following pressures is NOT equal to one atmosphere?
A. B. C. D. E. Ans.
Boyle Charles Dalton Gay-Lussac Torricelli
E Express one standard atmosphere of pressure in units of mm Hg.
A. B. C. D. E. Ans. 28.
the pressure of a gas sample in a container the difference in pressure between two gas samples the difference in pressure between a gas sample and atmospheric pressure atmospheric pressure the pressure of an ideal gas
76 cm Hg 14.7 lb/in2 30 inches of Hg 101 kPa 76 torr
E
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Chapter 6, States of Matter: Gases, Liquids, and Solids 29. A
B
E
C
D
0 0
Pressure (atm )
In the graph shown above, which line is the best representation of Boyle's Law behavior of a gas?
A. Ans. 30.
C
D.
E.
D
E
Boyle Charles Dalton Gay-Lussac Torricelli
3.00 L 1.50 L 0.667 L 0.500 L 0.333 L
E A given mass of oxygen at room temperature occupies a volume of 500.0 mL at 1.50 atm pressure. What pressure must be applied to compress the gas to a volume of only 150.0 mL?
A. B. C. D. E. Ans.
C.
A A sample of oxygen occupies 1.00 L. If the temperature remains constant, and the pressure on the oxygen is tripled, what is the new volume?
A. B. C. D. E. Ans. 32.
B
E Who formulated the relationship between the volume and the pressure of a gas?
A. B. C. D. E. Ans. 31.
B.
A
500 atm 150 atm 5.00 atm 1.50 atm 0.500 atm
C
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Chapter 6, States of Matter: Gases, Liquids, and Solids 33.
Who formulated the relationship between the volume and temperature of a gas?
A. B. C. D. E. Ans. 34.
B A balloon filled with helium has a volume of 1.00 × 103 L at 20°C. What would be the balloon's volume at 30°C, if the pressure surrounding the balloon remains constant?
A. B. C. D. E. Ans. 35.
Boyle Charles Dalton Gay-Lussac Torricelli
6.7 × 102 L 9.70 × 102 L 1.03 × 103 L 1.11 × 103 L 1.50 × 103 L
C
0 0
Temperature (K)
Who discovered the gas law represented in the figure above?
A. B. C. D. E. Ans. 36.
B What is the volume occupied by one mole of helium at 0°C and 1 atm pressure?
A. Ans.
Boyle Charles Dalton Gay-Lussac Torricelli
1.0 L
B.
22.4 L
C.
4.0 L
D.
40.0 L
B
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E.
12.2 L
Chapter 6, States of Matter: Gases, Liquids, and Solids 37.
A helium-filled weather balloon is launched from the ground where the pressure is 752 mmHg and the temperature is 21°C. Under these conditions its volume is 75.0 L. When it has climbed to an altitude where the pressure is 89 mmHg and the temperature is 0°C, what is its volume?
A. Ans. 38.
C. D. E.
9.56 L
D.
588 L
E.
682 L
2.24 2.67 2.81 31.9 1.71
mol mol mol mol × 103 mol
absorbing visible radiation absorbing ultraviolet radiation absorbing infrared radiation storing solar energy trapping sunlight during photosynthesis
There are no forces between gas particles. Gas particles occupy a negligible volume compared with the volume of their container. The average kinetic energy of the gas particles is proportional to the absolute temperature. Gas particles lose energy only when they collide with the walls of the container. Gas particles are in constant, random motion.
D What quantity is directly proportional to the kinetic energy of the particles in a gas?
A. B. C. D. E. Ans.
C.
C Which of the following statements conflicts with the kinetic molecular theory of gases?
A. B.
Ans. 41.
8.24 L
B Carbon dioxide acts as a greenhouse gas by
A. B. C. D. E. Ans. 40.
B.
D How many moles of gas are there in a gas-filled balloon which has a volume of 67.0 L at a pressure of 742 mmHg and a temperature of 25.0°C?
A. B. C. D. E. Ans. 39.
0.00 L
distance between molecules absolute temperature atomic mass formula mass volume of the individual particles.
B
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Chapter 6, States of Matter: Gases, Liquids, and Solids 42.
Of the following gases, which will behave most like an ideal gas?
A. Ans. 43.
NH3
D.
CH3Cl
E.
CO
vapor pressure surface tension resistivity viscosity compressibility
equal proportional zero lower higher
increases with increasing temperature is unaffected by temperature is higher for nonpolar substances than for polar ones is lowered by surfactants is the same as viscosity
D What is the term that describes a liquid changing to a vapor at a temperature less than its boiling point?
A. B. C. D. E. Ans.
C.
E Surface tension
A. B. C. D. E. Ans. 46.
HF
D At the membrane barrier in lung tissue between the blood and the surrounding atmosphere, what is the relationship between the partial pressure of atmospheric oxygen to that of the oxygen present in the blood?
A. B. C. D. E. Ans. 45.
B.
A What is the experimental quantity that serves as a measure of resistance to flow of a liquid?
A. B. C. D. E. Ans. 44.
H2
evaporation sublimation dissociation condensation supercooling
A
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Chapter 6, States of Matter: Gases, Liquids, and Solids 47.
Which one of the following substances with their structures shown, will NOT display hydrogen bonding? H
H O N
H
H
H
O
F H
H
H
H
H
C
H
H
C
H
C O
H
C
H
A. NH3
A. Ans. 48.
E T
B.
A
F
B. HF
B
C. H2O
C.
D. ethanol
C
H
H
H
E. diethyl ether
D.
E.
D
E
Gases and liquids are both highly compressible.
49.
Ans. T F
F The density of a gas is proportional to its molecular weight.
50.
Ans. T F
T Dalton's Law states that the volume of a gas varies directly with the absolute temperature.
51.
Ans. T F
F Approximately 99% of the total pressure of dry air is due to molecules of N2 and O2.
52.
Ans. T F
T The average energy of an ideal gas molecule depends on the molecular weight of the gas.
53.
Ans. T F
F Polar gases are more ideal than nonpolar ones.
54.
Ans. T F
F As temperature increases, so does viscosity.
55.
Ans. T F
F Glycerol has a lower viscosity than ethanol.
56.
Ans. T F
F The surface tension of water is reduced by the addition of soap.
57.
Ans. T F
T The boiling point of a liquid is dependent on the atmospheric pressure.
58.
Ans. T F
T The boiling point of a liquid increases with increasing altitude.
Ans.
F
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Chapter 6, States of Matter: Gases, Liquids, and Solids 59.
T
F
60.
Ans. T F
T All compounds containing both oxygen and hydrogen will exhibit hydrogen bonding.
61.
Ans. T F
F Ionic compounds tend to have higher melting points than molecular compounds.
62.
Ans. T F
T Covalent solids are soft and readily soluble in many solvents.
63.
Ans. T F
F Metals conduct electricity well due to the mobility of the metal ions in the solid.
Ans.
F
Polar compounds generally have higher boiling points than nonpolar compounds of similar molecular weight.
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Chapter 7, Reactions and Solutions 1.
Classify the following reaction as precipitation, acid-base or oxidation-reduction: Ce4+(aq) + Fe2+(aq) → Ce3+(aq) + Fe3+(aq)
Ans. 2.
oxidation-reduction Classify the following reaction as precipitation, acid-base or oxidation-reduction: H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(aq)
Ans. 3.
acid-base Classify the following reaction as precipitation, acid-base or oxidation-reduction: Na2S(aq) + CuSO4(aq) → Na2SO4(aq) + CuS(s)
Ans. 4.
precipitation Complete the products and balance the following equation for an acidbase reaction: HCl(aq) + KOH(aq)
Ans. 5.
HCl(aq) + KOH(aq) → KCl(aq) + H2O(l) Complete the products and balance the following equation for a precipitation reaction: FeSO4(aq) + NaOH(aq)
Ans. 6.
FeSO4(aq) + 2NaOH(aq) → Fe(OH)2(s) + Na2SO4(aq) Write a balanced equation for the reaction between zinc metal and iron(III) ions to form zinc(II) ions and iron(II) ions (Symbols: zinc = Zn; iron = Fe).
Ans. 7.
Zn(s) + 2Fe3+(aq) → Zn2+(aq) + 2Fe2+(aq) Name the two products formed when octane (C8H18) burns completely in excess oxygen gas.
Ans. 8.
carbon dioxide and water Classify the following reaction as decomposition, combination, singlereplacement or double-replacement: 2H2O(l) → 2H2(g) + O2(g)
Ans. 9.
decomposition Classify the following reaction as decomposition, combination, singlereplacement or double-replacement: H2SO4(aq) Ba(OH)2(aq) → BaSO4(s) + 2H2O(g)
Ans. 10.
double-replacement Classify the following reaction as decomposition, combination, singlereplacement or double-replacement: Mg(s) + 2HCl(aq) → MgCl2(g) + H2(g)
Ans.
single-replacement
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