1. Which type of intermolecular force is the strongest?b) c)
Answer: d d)

2. Which type of intermolecular force is the strongest?b) c)
Answer: d d)

3. List the following molecules in order of increasing boiling point:
n-propanol
dimethyl ether
diethyl ether
n-propanol < dimethyl ether < diethyl ether
diethyl ether < dimethyl ether < n-propanol
dimethyl ether < diethyl ether < n-propanol
dimethyl ether < n-propanol < diethyl ether
Answer: c

4. List the following molecules in order of increasing boiling point:
n-propanol
dimethyl ether
diethyl ether
n-propanol < dimethyl ether < diethyl ether
diethyl ether < dimethyl ether < n-propanol
dimethyl ether < diethyl ether < n-propanol
dimethyl ether < n-propanol < diethyl ether
Answer: c

5. Which of the following is the most viscous?a) b) c) d) e)
Answer: c

6. Which of the following is the most viscous?a) b) c) d) e)
Answer: c

7. A graph is prepared from the natural log of pressure versus the inverse of the temperature. The slope of the resulting line is –2996 K. What is the enthalpy of vaporization?
24.91 kJ/mol
−24.91 kJ/mol
245.9 kJ/mol
–245.9 kJ/mol
Answer: a

8. A graph is prepared from the natural log of pressure versus the inverse of the temperature. The slope of the resulting line is –2996 K. What is the enthalpy of vaporization?
24.91 kJ/mol
−24.91 kJ/mol
245.9 kJ/mol
–245.9 kJ/mol
Answer: a

9. Temperature (K) Pressure (torr)
The vapor pressure of nitrogen is tabulated below as a function of temperature. Calculate the heat of vaporization of nitrogen.
Temperature (K)
Pressure (torr) 65
130.5 70
289.5 75
570.8 80
1028 85
1718
5.92 kJ/mol
9.90 × 10–2 J/mol
64.2 J/mol
1.75 × 10–5 J/mol
5.85 × 10–2 kJ/mol
Answer: a

10. Temperature (K) Pressure (torr)
The vapor pressure of nitrogen is tabulated below as a function of temperature. Calculate the heat of vaporization of nitrogen.
Temperature (K)
Pressure (torr) 65
130.5 70
289.5 75
570.8 80
1028 85
1718
5.92 kJ/mol
9.90 × 10–2 J/mol
64.2 J/mol
1.75 × 10–5 J/mol
5.85 × 10–2 kJ/mol
Answer: a

11. A 29. 0 g sample of acetone is heated from a solid at −94. 8°C to −50
A 29.0 g sample of acetone is heated from a solid at −94.8°C to −50.0°C. How much energy is required for this change?
Melting point
−94.8°C
ΔHfus
5.69 kJ/mol s
2.15 J/g·K
Molar mass
58.01 g/mol
2.80 kJ
5.64 kJ
6.18 kJ
2.96 kJ
7.84 kJ
Answer: b

12. A 29. 0 g sample of acetone is heated from a solid at −94. 8°C to −50
A 29.0 g sample of acetone is heated from a solid at −94.8°C to −50.0°C. How much energy is required for this change?
Melting point
−94.8°C
ΔHfus
5.69 kJ/mol s
2.15 J/g·K
Molar mass
58.01 g/mol
2.80 kJ
5.64 kJ
6.18 kJ
2.96 kJ
7.84 kJ
Answer: b

13. How much energy is required to vaporize 32
How much energy is required to vaporize g of ethanol at its boiling point, if its Hvap is 40.7 kJ/mol?
28.9 kJ
3.83 kJ
6.30 kJ
17.6 kJ
7.60 kJ
Answer: a

14. How much energy is required to vaporize 32
How much energy is required to vaporize g of ethanol at its boiling point, if its Hvap is 40.7 kJ/mol?
28.9 kJ
3.83 kJ
6.30 kJ
17.6 kJ
7.60 kJ
Answer: a

15. More than one phase is present.
A sample is at the temperature and pressure indicated by point a on the phase diagram below. What phase is present after the temperature is increased to the critical temperature at constant pressure?
gas
liquid
solid
More than one phase is present.
Answer: a

16. More than one phase is present.
A sample is at the temperature and pressure indicated by point a on the phase diagram below. What phase is present after the temperature is increased to the critical temperature at constant pressure?
gas
liquid
solid
More than one phase is present.
Answer: a

17. What phases are present at point f on the given phase diagram?
gas and liquid
gas and solid
liquid and solid
gas, liquid, and solid
Answer: c

18. What phases are present at point f on the given phase diagram?
gas and liquid
gas and solid
liquid and solid
gas, liquid, and solid
Answer: c

19. Liquid Solid P (atm) Gas Temp (°F)
Considering the following phase diagram for UF6, which of the following conditions is true?
Liquid
At 1 atm, UF6 boils.
UF6 melts at 1 atm.
At 1 atm, UF6 sublimes.
UF6 does not boil until it reaches the critical temperature.
Solid
1 atm
Answer: c
P (atm)
Gas
Temp (°F)

20. Liquid Solid P (atm) Gas Temp (°F)
Considering the following phase diagram for UF6, which of the following conditions is true?
Liquid
At 1 atm, UF6 boils.
UF6 melts at 1 atm.
At 1 atm, UF6 sublimes.
UF6 does not boil until it reaches the critical temperature.
Solid
1 atm
Answer: c
P (atm)
Gas
Temp (°F)

21. nonbonding atomic solid. network covalent solid.
Diamond is a/an
molecular solid.
ionic solid.
metallic atomic solid.
nonbonding atomic solid.
network covalent solid.
Answer: e

22. nonbonding atomic solid. network covalent solid.
Diamond is a/an
molecular solid.
ionic solid.
metallic atomic solid.
nonbonding atomic solid.
network covalent solid.
Answer: e