CHM 2046C Module 7II:
Chapter 13 Sample Multiple Choice Test #1

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1. One mole of propan-2-ol, C3H7OH, is placed in a 250 cm3 flask. Another mole of propan-2-ol is placed in a 1000 cm3 flask. Both flasks are sealed and maintained at the same temperature. The vapor pressure of propan-2-ol in the 250 cm3 flask at 24°C is 40 mm Hg. In the 1000 cm3 flask the vapor pressure in mm Hg is

a.

10.

b.

20.

c.

40.

d.

80.

e.

160.

 

2. The vapor pressure of a liquid increases with an increase of temperature. Which of the following statements best explains this increase?

a.

The average kinetic energy of molecules is greater, thus more molecules can enter the gaseous state.

b.

The number of gaseous molecules above the liquid remains constant, but these molecules have greater average kinetic energy.

c.

The faster moving molecules in the liquid exert a greater pressure.

d.

All the molecules have greater kinetic energies.

e.

The intermolecular forces between the molecules becomes less at higher temperature.

 

3. The normal boiling point of a liquid

a.

is 100°C at 1 atm pressure.

b.

is the temperature at which the vapor pressure is 1 atm.

c.

is the temperature at which liquid and vapor are in equilibrium.

d.

is the temperature at which the vapor pressure equals the external pressure.

e.

is the temperature at which there is a continuous formation of gaseous bubbles in the liquid.

 

4. The data for the equilibrium pressure of any liquid as a linear function of temperature can best be represented by plotting

a.

ln P versus t.

b.

ln P versus T.

c.

ln P versus 1/T.

d.

P versus t.

e.

P versus T.

5. All of the following indicate very strong intermolecular forces of attraction in a liquid EXCEPT

a.

a very high boiling point.

b.

a very high vapor pressure.

c.

a very high critical temperature.

d.

a very high viscosity.

e.

a very high heat of vaporization.

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6. Which compound should have the highest vapor pressure at room temperature?

a.

C4H10

b.

C5H12

c.

C6H14

d.

C7H16

e.

C8H18

 

7. Which of the following compounds shows an abnormal boiling point due to hydrogen bonding?

a.

CH3NH2

b.

CH3OCH3

c.

CH3SH

d.

CH3Cl

e.

HCl

 

8. Of the following substances, the one expected to have the highest critical temperature is

a.

CH3OH.

b.

CH3Cl.

c.

CH4.

d.

C2H6.

e.

C3H8.

 

9. What compound should have the lowest vapor pressure at room temperature?

a.

SiH4

b.

Si2H6

c.

Si2Cl6

d.

Si3H8

e.

Si4H10

10. Which of the following would be expected to have the highest heat of vaporization?

 

a.

CH3CH2CH3

b.

CH3OCH3

c.

CH3CHO

d.

CH3CH2NH2

e.

CH3CH2F

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11. The lines in the diagram represent values of pressure and temperature at which two phases may be present in equilibrium. Which one of the following descriptions of the lines SX, RX, and XZ is the correct one?

a.

SX = solid-liquid, RX = solid-gas, XZ = gas-liquid

b.

SX = solid-gas, RX = solid-liquid, XZ = gas-liquid

c.

SX = solid-liquid, RX = gas-liquid, XZ = solid-gas

d.

SX = gas-liquid, RX = solid-gas, XZ = solid-liquid

e.

SX = gas-liquid, RX = solid-liquid, XZ = solid-gas



12. From a consideration of the phase diagram below, a change from point N to point M corresponds to

a.

sublimation.

b.

vaporization.

c.

condensation.

d.

liquefaction.

e.

freezing.



 

13. The process which is represented by the equation, K(s) --> K(g), is

a.

fusion.

b.

melting.

c.

sublimation.

d.

vaporization.

e.

condensation.

 

14. The heat of fusion of a compound equals

a.

heat of vaporization plus heat of crystallization.

b.

heat of fusion plus heat of vaporization.

c.

heat of sublimation minus heat of vaporization.

d.

heat of vaporization minus heat of fusion.

e.

heat of ionization plus heat of crystallization.

 

15. Which of the following as solids has a crystal structure containing discrete (or separate) molecules?

a.

potassium

b.

glass

c.

quartz

d.

carborundum, SiC

e.

hydrogen

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16. A solid has a very high melting point, it is very hard, and its liquid is nonconducting. The solid is

a.

an ionic solid.

b.

a covalent solid.

c.

a metallic solid.

d.

an atomic solid.

e.

a molecular solid.

 

17. Which of the following compounds would be expected to have the highest melting point?

a.

LiCl

b.

NaCl

c.

MgCl2

d.

BaCl2

e.

BCl3

18. What is the simplest formula of a solid containing A, B, and C atoms in a cubic lattice in which the A atoms occupy the corners, the B atoms, the body-centered position and the C atoms, the faces of the unit cell?

a.

ABC

b.

ABC3

c.

ABC6

d.

A8BC6

e.

A4BC3

 

19. A crystalline compound consists of two types of atoms, X and Y. It crystallizes in a cubic lattice with one X atom at the body center Y atoms at the corners of the unit cell. The simplest formula of this compound is

a.

XY8.

b.

X2Y.

c.

XY.

d.

XY2.

e.

X8Y.

 

20. Tungsten crystallizes in a cubic lattice with two atoms of W per unit cell. It could be classified as

a.

a body-centered cubic structure.

b.

a face-centered cubic structure.

c.

a simple cubic structure.

d.

a cubic closest packing structure.

e.

a hexagonal closest packing structure.

 

21. The oxide ions in Na2O form a face-centered cubic lattice and the sodium ions occupy all the tetrahedral holes. The oxide ions occupy the faces and the corners of the unit cell. How many sodium ions are in one unit cell?

a.

2

b.

4

c.

6

d.

8

e.

12



 

 

 

22. Titanium dioxide crystallizes in a noncubic crystal system (a tetragonal system). In this structure, two of the O2- ions are within the interior of the cell, two are in the top face, and two in the bottom face of the cell. Ti4+ ions are at the corners and the center of the cell. How many oxide ions are there per unit cell?

a.

1

b.

2

c.

3

d.

4

e.

6



23. Silver crystallizes in the face-centered cubic system. If the edge of the unit cell is 0.407 nm, what is the radius of a silver atom in nm?

a.

0.144

b.

0.176

c.

0.206

d.

0.288

e.

0.352


24. Solid nickel has a cubic unit cell. The edge of the cubic cell is 3.0 x 10-8 cm. Which of the cubic unit cells described below would give nickel its highest density?

 

a.

A simple cubic cell.

b.

A body-centered cubic cell.

c.

A face-centered cubic cell.

d.

The density would be identical for all of the cells above if the edge of each cell was 3.0 x 10-8 cm.

e.

Cannot determine since the size of the nickel atom is not given.



25. Which of the following substances is most likely to exist as a solid at room temperature?

a.

NF3

b.

PF5

c.

SF6

d.

BF3

e.

BaF2

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