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Practice Questions
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5.1 Intra- and Intermolecular Forces
 
5.2 Solids
 
5.3 Liquids
 
5.4 Gases
 
5.5 Phase Changes
 
5.6 The Gas Laws
 
5.7 Boyle’s Law
 
5.8 Charles’s Law
 
 
5.9 Avogadro’s Law
 
5.10 The Ideal Gas Law
 
5.11 Density of Gases
 
5.12 Dalton’s Law of Partial Pressures
 
5.13 Graham’s Law of Diffusion and Effusion
 
5.14 Solutions
 
5.15 Practice Questions
 
5.16 Explanations
 
Practice Questions
Statement I Statement II
1. Ice, unlike most substances, is denser than water in the liquid phase.   BECAUSE   In water, hydrogen bonds can form between the positively charged H atom on one water molecule and the slightly negatively charged O atom on a nearby water molecule.
2. Which of the following gases would be the densest at standard temperature and pressure?
(A) Helium
(B) Argon
(C) Carbon dioxide
(D) Xenon
(E) Nitrogen
3. In the laboratory, a sample of hydrogen is collected by water displacement. The sample of hydrogen has a volume of 25 mL at 24.0ºC and a barometric pressure for the day of 758 mmHg. What is the pressure of the dry gas at this temperature? (The vapor pressure of water at 24.0ºC is 22.4 mmHg.)
(A) 455 mmHg
(B) 470 mmHg
(C) 736 mmHg
(D) 758 mmHg
(E) 780 mmHg
4. Calculate the approximate amount of heat necessary to raise the temperature of 50.0 grams of liquid water from 10.0ºC to 30.0ºC. (The specific heat of water liquid is 4.18 J/gºC.)
(A) 20 J
(B) 80 J
(C) 100 J
(D) 200 J
(E) 4,180 J
5. Using the sketch of the phase diagram for water given above, determine which of the following statements is incorrect:
(A) The triple point is point A. This is the point at which all three phases are in equilibrium with one another.
(B) The line AB is the line representing the solid-liquid equilibrium line. Anywhere along this line the substance could melt or freeze.
(C) The slope of line AB is negative. This slope indicates that the solid is much denser than the liquid.
(D) Line AD represents the phase changes of sublimation and deposition.
(E) Line AC represents where the substance would condense and vaporize.
Statement I Statement II
6. Most ionic solids have high melting points.   BECAUSE   Ionic solids are made up of positive and negative ions held together by electrostatic attractions.
7. Which of the following best illustrates a graph of pressure versus volume for a gas at constant temperature?
(A)
(B)
(C)
(D)
(E)
8. Which of the following solutions would probably have the highest boiling point?
(A) 0.100 m KOH
(B) 0.100 m Na2SO4
(C) 0.100 m C6H12O6
(D) 0.200 m CaCl2
(E) 0.200 m CH3CH2OH
9. Which of the following must be measured in order to calculate the molality of a solution?
  I. Mass of the solute
 II. Mass of the solvent
III. Total volume of the solution
(A) I only
(B) I and III only
(C) II and III only
(D) I and II only
(E) I, II, and III
10. The molarity of a solution that is composed of 80.00 g of sodium hydroxide dissolved in 2.0 L of solution is
(A) 1.0 M
(B) 2.0 M
(C) 4.0 M
(D) 40.0 M
(E) 160.0 M
11. Which of the following substances would dissociate completely when placed into excess amounts of distilled water?
(A) C2H5OH
(B) HC2H3O2
(C) LiNO3
(D) Mg(OH)2
(E) All of these will dissociate completely in water
Statement I Statement II
12. The solubility of carbon dioxide in a soft drink decreases with a decrease in pressure.   BECAUSE   The solubility of a gas generally increases with an increase in temperature.
13. The molarity of a solution obtained when 50.0 mL of 6.0 M HCl is diluted to a final volume of 300.0 mL is
(A) 0.01 M
(B) 0.10 M
(C) 0.20 M
(D) 0.30 M
(E) 1.0 M
14. Which of the following solutes and solvents would be expected to form stable solutions?
(A) I only
(B) I and II only
(C) III only
(D) I, II, and III only
(E) I, II, and IV only
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