Adv. Bonding and States of Matter Test Review
1. A pressure of 700 kPa is equal to
a. 40.0 mm Hg
b. 401 mm Hg
mm Hg.
c. 1060 mm Hg
d. 5250 mm Hg
2. The average atmospheric pressure in Denver is 0.830 atm. What is this pressure in kPa?
a. 8.19 x 10-3 kPa
c. 100 kPa
b. 84.1 kPa
d. 102 kPa
3. When pressure, volume, and temperature are known, the ideal gas law can be used to calculate
a. the chemical formula
c. number of moles
b. the ideal gas constant
d. compressibility
4. 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
5. Which of the following is a property of gases?
a. gases have high density
c. gases have a definite shape
b. gases are fluid
d. gases are incompressibility
6. A 2.5 L sample of a gas has a mass of 1.56 g at STP. What is the molar mass?
a. 14.18 g/mol
c. 22.4 g/mol
b. 1.39 g/mol
d. 27.02 g/mol
7. If the volume remains constant, P1 and T1 represent the original pressure and temperature, and P2 and
T2 represent the new volume and pressure, what is the mathematical expression for Gay-Lussac’s Law?
a. T1/P1=T2/P2
c. P1/T1=P2/T2
b. P1T1=P2T2
d. T1/V1=T2/V2
8. According to Charles law, volume and temperature are
a. indirectly proportional
c. inverses
b. directly proportional
d. reciprocals
9. Temperature and volume changes at a constant pressure can be calculated using
a. Boyle’s Law
c. Dalton’s Law
b. Ideal Gas Law
d. Charles’ Law
10. A sample of gas has a volume of 2.32 L at 20 C. What would the volume be at 43 C, if the pressure
remains the same?
a. 2.1 L
c. 4.99 L
b. 2.5 L
d. 40 L
11. The density of a substance undergoes the smallest increase when the substance changes from a
a. liquid to a gas
c. liquid to a solid
b. gas to a liquid
d. none of the above
12. The greater the kinetic energy of the particles in a sample of matter
a. the higher the temperature is
c. the more heat the sample will absorb
b. the lower the temperature is
d. the less heat flows away from the sample
13. London Dispersion forces are considered a dipole-dipole force because it
a. affects all types of compounds
c. affects polar molecules
b. affects non-polar molecules
d. results from a temporary dipole
14. A hydrogen bond is an example of what intermolecular force?
a. Ionic
c. Metallic
b. dipole-dipole
d. London Dispersion
15. When an object feels cold to the touch it is because the object
a. has less heat
c. has no heat
b. particles have stopped moving
d. is a solid
16. What happens to the amount of kinetic energy during a phase change?
a. Kinetic Energy increases
c. Kinetic Energy increases or decreases
b. Kinetic Energy decreases
d. There is no change in kinetic energy
17. A solid will have
a. increased
b. the same
compressibility compared to a liquid
c. decreased
d. double
18. Which is an example of gas diffusion?
a. inflating a flat tire
b. the odor of perfume spreading throughout a room
c. a cylinder of oxygen stored under high pressure
d. All of the above
19. A carbonated beverage over ice contains
a. one
b. two
phases
c. three
d. four
20. The amount of heat that is required to melt one mole of solid at its melting point is
a. heat of vaporization
c. heat of sublimation
b. heat of fusion
d. heat of deposition
21. A volatile liquid can
a. freeze readily
b. react readily
c. condense readily
d. evaporate readily
22. 31.5 g of H2O is being melted at its melting point of 0 °C. Calculate the heat of fusion. (molar heat of
fusion of water is 6.009 kJ/mol)
a. 10.52kJ
c. 2.04 kJ
b. 6.05 kJ
d. 4.59 kJ
23. 80.1 g of H2O exists as a gas at 100 °C. How many kJ must be removed to turn the water into liquid at
100 °C? (The molar heat of vaporization of water is 40.79 kJ/mol)
a. 14.82 kJ
c. 180.91 kJ
b. 40.7 kJ
d. 35.46 kJ
Short Answer
24. Explain diffusion and effusion
25. What is the volume of a 0.76 mol sample of gas at 45 C and a pressure of .974 atm?
26. The standard molar heat of vaporization for water is 40.79 kJ/mol. How much energy would be
required to vaporize 5.00 mol H2O?
27. Find the mass of 5.60 L of O2 at 1.75 atm and –23 C.
28. A mixture of three gases, A, B, and C, is at a total pressure of 6.11 atm. The partial pressure of gas
A is 1.68 atm; that of gas B is 3.89 atm. What is the partial pressure of gas C?
29. A sample of oxygen at 40 C occupies 820 mL. If this sample later occupies 1.25 L at 60 C and 1.40
atm, what was its original pressure?
30. What 5 conditions must be met for an ideal gas?
31. Explain why there is no change in temperature when water is continuously heated and boiled?
32. Explain what will happen to the potential and kinetic energy as a water sample is cooled to 0 C,
freezes, and continues cooling to –20 C.
33. Compare the kinetic and potential energies of three samples – 1 gas, 1 liquid, and 1 solid – all at 40
C.
34. What is the change in energy when a 400 mL sample of water goes from 88.2 C to 68.7 C?
35. What is the specific heat of a 100 g piece of metal cooled in the freezer to –20 C that cools a 500 mL
sample of water from 19.8 C to 17.6 C?
36. How can we boil water at a temperature much lower than 100 C? How can we boil water at a
temperature much higher than 100 C?
37. Why is the heat of vaporization typically much higher than the heat of fusion?
Answers
1. d
2. b
3. c
4. b
5. b
6. a
7. c
8. b
9. d
10. b
11. c
12. a
13. d
14. b
15. a
16. d
17. c
18. b
19. c
20. b
21. d
22. a
23. c
24. Diffusion is the spontaneous mixing of the particles of two substances caused by the random
motion. Effusion is a process by which gas particles pass through a tiny opening
25. V= (0.76 x 0.0821 x 318)/0.974 V= 20.37 L
26. (40.79 kJ/mol) x (5 mol) = 203.95 kJ
27. n= (1.75 x 5.60)/(0.0821 x 250) n= 0.477 mol O2
0.477 mol O2 x (32 g O2/1 mol O2) = 15.26 g O2
28. C= 6.11- (1.68 + 3.89) C= .54 atm
29. (P1 x 0.820)/313= (1.4 x 1.25)/333
P1 = 2.01 atm
30. a. gases consist of large numbers of tiny particles that are far apart relative to their size
b. collisions between gas particles and between particles and container walls are elastic collisions
(no loss of KE)
c. gas particles are in continuous, rapids, random motion (therefore they have KE)
d. there are no forces of attraction or repulsion between gas particles
e. the average KE of gas particles depends on the temperature of the gas
31. The energy being absorbed during boiling is breaking bonds between particles to create a gas.
This is a change in potential energy instead of kinetic (temperature)
32. As the water is cooled, kinetic energy is decreasing (with the temp) and potential is remaining
unchanged. At freezing, the kinetic is remaining constant and potential is decreasing as “bonds”
are formed between particles. After freezing – with continuing of cooling, the kinetic energy
starts decreasing again and the potential remains unchanged.
33. All three samples have the same kinetic energy as they are the same temperature. The gas has
the most potential as is has the potential to form more bonds. The liquid has the medium
amount of potential and the solid has the least amount of potential energy.
34. (4.18J/1g H2O 1C)(400 g H2O)(-19.5 C) = 32,604 J
35. Water - (4.18J/1g H2O 1C)(500 g H2O)(-2.2 C) = -4598 J
Metal – (+4598 J)/(100 g metal)(37.6 C) = .24 J/1 g metal 1 C
36. We can lower the pressure, then the water will boil at a lower temperature (phase diagram pg
381). Conversely, we can raise the pressure and the water will boil at a higher temperature
37. More “bonds” need to be broken to completely release a material as a gas.