Chemsitry States of Matter Multiple Choice017074

CHEMISTRY LTF® DIAGNOSTIC TEST

STATES OF MATTER

1

TEST CODE: 017074

Directions: Each group of questions below consists of five lettered answers followed by a list of numbered phrases or sentences. For each numbered phrase or sentence select the one answer that is most closely related to it and fill in the corresponding oval on the answer sheet. Each answer may be used once, more than once or not at all in each group.

Questions 1-3 refer to the following diagram showing 1.0 L containers filled with gases at 25ºC and 1.0 atm pressure.

H2 He O2 CH4 SO2

A) B) C) D) E)

1. The container whose gas is involved in the formation of acid rain.

2. The container with the greatest number of atoms.

3. The sample containing gases that have the slowest average velocity.

Questions 4-7 refer to the following choices

A) NaHCO3(s)B) C6H12O6(s)C) Cu(s)D) Cdiamond

E) CO2(s)

4. The substance that can be classified as a covalent network solid.

5. The substance, that when dissolved in water, will conduct a current of electricity.

6. The substance that contains both ionic and covalent bonding.

7. The substance that conducts electricity in its solid state.

2

Directions: Each of the questions or incomplete statements below is followed by five suggested answers or completions. Select the one that is best in each case and fill in the corresponding oval on the answer sheet.

8. Determine the density of a sample of oxygen gas which exerts a pressure of 2 atm at 400 K.

A) 1 g/LB) 2 g/LC) 4 g/LD) 8 g/LE) 30 g/L

9. A student was given two separate yet identical containers, under the same set of conditions, filled with different gases. The density of the gas in container A was 2.24 g/L. The density of the gas in container B was 4.48 g/L. Gas B was eventually identified as pure sulfur dioxide gas. Determine the molar mass of gas A.

A) 4 g/molB) 8 g/molC) 16 g/molD) 32 g/molE) 64 g/mol

10. Which expression gives the molar mass of a gas if 18.0 grams of the gas occupies 3.00 L at 2.32 atm and 27ºC.

A)

18.03.00

× 0.082 × 300

2.32

B)2.32

18.03.00

× 0.082 × 300

C)

18.03.00

× 0.082 × 27

2.32

D)2.32 × 0.082 × 300

18.03.00

E)18.0 × 0.082 × 3 × 27

2.32

3

11. Which of the following would behave least like an ideal gas?

A) SO2

B) H2

C) O2

D) N2

E) He

12. Which of the following gases has the greatest density at standard temperature and pressure?

A) Argon B) XenonC) HeliumD) NitrogenE) Carbon dioxide

13. Under which conditions do gases behave most ideally? Pressure Temperature Number of Molecules

A) Low Low FewB) High High ManyC) High High FewD) High Low ManyE) Low High Few

4

Questions 14 and 15 refer to the spherical monatomic molecule pictured below having no dipole moment. The dot indicates the location of the nucleus in all of the diagrams.

14. The molecule is placed near a water molecule and experiences a dipole-induced dipole intermolecular force as a result. Which of the following best represents this interaction?

A)

δ+δ+ δ−δ−

B)

δ+δ+ δ−δ−

C)

δ− δ+δ+ δ−

D)

δ+δ− δ−δ+

E)

δ+δ− δ−δ−

5

15. The molecule is placed near an identical molecule and experiences an induced dipole-induced dipole (London dispersion) intermolecular force. Which of the following best represents this interaction?

A)

δ−δ− δ+δ+

B)

δ+δ+ δ−δ−

C)

δ+δ+ δ−δ−

D)

δ+δ− δ−δ+

E)

δ−δ− δ+δ+

6

16. All of the following exhibit hydrogen bonding EXCEPTA) HFB) NH3

C) H2OD) C2H6 E) C2H5OH

Questions 17 and 18 refer to the following graph.

17. Which of the following statements best account for the general trend represented by the graph?

I. Boiling point increases as group number of the hydride increases. II. Boiling point increases as the number of electrons in the molecule increases. III. Boiling point increases as the number of hydrogen atoms in the molecule increases.

A) I only B) II onlyC) III onlyD) I and II onlyE) I, II and III

18. Which of the following statements best accounts for the difference in boiling points between water and methane?

A) Methane is nonpolar molecule.B) Water exhibits hydrogen bonding.C) Methane exhibits hydrogen bonding.D) Water has a higher molar mass than methane.E) At room temperature, methane is a gas and water is a liquid.

7

19. What type of attractive forces are being overcome when liquid oxygen boils at 90 K?A) Ionic bondsB) Covalent bondsC) Hydrogen bondsD) Dipole-dipole forcesE) Induced dipole-induced dipole (dispersion) forces

20. Which of these statements is true regarding the boiling of water at the top of a mountain?

A) The water will boil at 100oC.B) The water will boil at a temperature less than 100oC.C) The water will boil at a temperature greater than 100oC.D) The elevation of the mountain has no effect on the boiling point of water.E) The elevation of the mountain will affect the boiling point, but it is impossible to predict

whether it will be greater than or less than 100oC without the actual height of the mountain.

21. A slush of liquid water and ice is at equilibrium at 0ºC when a small amount of heat is removed so that more ice is formed. The system will experience

A) an increase in temperature since the formation of ice from water is an exothermic processB) a change in vapor pressure above the mixture of ice and waterC) a small decrease in temperature since the formation of ice produces a colder systemD) a large decrease in temperature since more ice will formE) no change in temperature

22. When a substance is converted from a liquid to a gas at its normal boiling point, which of the following are correct?

I. The potential energy of the system increases. II. The distance between the molecules increases. III. The vapor pressure of the liquid is less than 1 atm.

A) I onlyB) II onlyC) I and II onlyD) II and III onlyE) I, II and III

23. The temperature and pressure at which all three states of matter can exist in equilibrium is called the

A) critical pointB) boiling pointC) triple pointD) equilibrium pointE) flash point

8

24. Which of the following transformations is known as sublimation?

A) liquid to gasB) gas to liquidC) solid to liquidD) solid to gasE) gas to solid

Questions 25 and 26 refer to the following phase diagram.

25. If a substance is at position A and the temperature is increased at constant pressure until the substance is at point B, which of these statements are correct?

I. The substance melts. II. The substance changes from solid to liquid. III. The substance is a gas when heating is complete.

A) I onlyB) II onlyC) III onlyD) I and II onlyE) I, II and III

9

26. At which of the lettered points on the phase diagram is more than one phase present in equilibrium?

I. D II. E III. F IV. G A) II onlyB) III onlyC) I and III onlyD) I, II, III onlyE) I, II, III and IV

10

Questions 27 and 28 refer to a heating curve of a pure substance. Heat is being added to 100. grams of the substance at a constant rate.

27. Which of the following statements about the heating curve are true?

I. It takes more heat to vaporize the substance than to melt the substance. II. The solid has a higher specific heat than the liquid. III. Boiling occurs at a constant temperature. IV. Freezing is an exothermic process.

A) I and II onlyB) I, II, and III onlyC) I, II, and IV onlyD) I, III, and IV onlyE) I, II, III, and IV

28. How many joules of heat does it take to heat 100. g of the substance from 10ºC to 20ºC? (c = 4.2 J/g ºC)

A) 500 JB) 1000 JC) 2100 JD) 4200 JE) 5500 J

11

29. Which of the following processes are exothermic?

I. Freezing II. Melting III. Evaporating IV. Boiling V. Condensing

A) I and V only B) II, and IV only C) I, II, and III onlyD) I, III, and V onlyE) II, III, and V only

30. A 5.0 L sample of gas is heated from 15ºC to 30ºC. If the pressure remains constant, the volume would be expected to

A) doubleB) decrease to one halfC) decrease slightlyD) increase slightlyE) stay the same

31. A 10.0 L container is filled with 0.40 mol H2(g), 0.80 mol O2(g), and 0.80 mol SO2(g). If the total pressure inside the flask is 800. torr, what is the partial pressure of the H2(g)?

A) 120 torrB) 160 torrC) 220 torrD) 400 torrE) 800 torr

32. Which of the following refer only to ideal gases, and not real gases?

I. Gases contain particles that are in constant motion. II. Gas particles have no molecular volume. III. Gas particles exhibit no intermolecular forces.

A) I onlyB) II onlyC) I, and II onlyD) II and III onlyE) I, II, and III

12

33. Which of the following substances would you expect to have the highest boiling point?

A) ArB) O2

C) N2

D) CH4

E) C2H4

34. What would be the volume of the gas if the temperature were held constant and the external pressure on the gas is reduced to 400 torr?

A) 0.25 LB) 0.50 LC) 0.75 LD) 1.0 LE) 2.0 L

35. If the gas is confined in a rigid 0.50 L container, what would be the pressure if the temperature were increased to 127ºC?

A) 6.0 × 102 torr

B) 1.1 × 103 torr

C) 2.5 × 103 torr

D) 3.8 × 103 torr

E) 8.0 × 103 torr

Chemsitry States of Matter Multiple Choice017075

CHEMISTRY LTF® DIAGNOSTIC TEST

STATES OF MATTER

1

TEST CODE: 017075

Directions: Each group of questions below consists of five lettered answers followed by a list of numbered phrases or sentences. For each numbered phrase or sentence select the one answer that is most closely related to it and fill in the corresponding oval on the answer sheet. Each answer may be used once, more than once or not at all in each group.

Questions 1-4 refer to the following choices

A) NaHCO3(s)B) C6H12O6(s)C) Cu(s)D) Cdiamond

E) CO2(s)

1. The substance, that when dissolved in water, will conduct a current of electricity.

2. The substance that can be classified as a covalent network solid.

3. The substance that conducts electricity in its solid state.

4. The substance that contains both ionic and covalent bonding.

Questions 5-7 refer to the following diagram showing 1.0 L containers filled with gases at 25ºC and 1.0 atm pressure.

H2 He O2 CH4 SO2

A) B) C) D) E)

5. The container with the greatest number of atoms.

6. The sample containing gases that have the slowest average velocity.

7. The container whose gas is involved in the formation of acid rain.

2

Directions: Each of the questions or incomplete statements below is followed by five suggested answers or completions. Select the one that is best in each case and fill in the corresponding oval on the answer sheet.

8. Which expression gives the molar mass of a gas if 18.0 grams of the gas occupies 3.00 L at 2.32 atm and 27ºC.

A)

18.03.00

× 0.082 × 300

2.32

B)2.32

18.03.00

× 0.082 × 300

C)

18.03.00

× 0.082 × 27

2.32

D)2.32 × 0.082 × 300

18.03.00

E)18.0 × 0.082 × 3 × 27

2.32

3

Questions 9 and 10 refer to the following graph.

9. Which of the following statements best accounts for the difference in boiling points between water and methane?

A) Methane is nonpolar molecule.B) Water exhibits hydrogen bonding.C) Methane exhibits hydrogen bonding.D) Water has a higher molar mass than methane.E) At room temperature, methane is a gas and water is a liquid.

10. Which of the following statements best account for the general trend represented by the graph?

I. Boiling point increases as group number of the hydride increases. II. Boiling point increases as the number of electrons in the molecule increases. III. Boiling point increases as the number of hydrogen atoms in the molecule increases.

A) I only B) II onlyC) III onlyD) I and II onlyE) I, II and III

4

11. A slush of liquid water and ice is at equilibrium at 0ºC when a small amount of heat is removed so that more ice is formed. The system will experience

A) an increase in temperature since the formation of ice from water is an exothermic processB) a change in vapor pressure above the mixture of ice and waterC) a small decrease in temperature since the formation of ice produces a colder systemD) a large decrease in temperature since more ice will formE) no change in temperature

12. If the gas is confined in a rigid 0.50 L container, what would be the pressure if the temperature were increased to 127ºC?

A) 6.0 × 102 torr

B) 1.1 × 103 torr

C) 2.5 × 103 torr

D) 3.8 × 103 torr

E) 8.0 × 103 torr

13. A student was given two separate yet identical containers, under the same set of conditions, filled with different gases. The density of the gas in container A was 2.24 g/L. The density of the gas in container B was 4.48 g/L. Gas B was eventually identified as pure sulfur dioxide gas. Determine the molar mass of gas A.

A) 4 g/molB) 8 g/molC) 16 g/molD) 32 g/molE) 64 g/mol

14. Under which conditions do gases behave most ideally? Pressure Temperature Number of Molecules

A) Low Low FewB) High High ManyC) High High FewD) High Low ManyE) Low High Few

15. Which of the following would behave least like an ideal gas?

A) SO2

B) H2

C) O2

D) N2

E) He

5

16. What would be the volume of the gas if the temperature were held constant and the external pressure on the gas is reduced to 400 torr?

A) 0.25 LB) 0.50 LC) 0.75 LD) 1.0 LE) 2.0 L

17. Determine the density of a sample of oxygen gas which exerts a pressure of 2 atm at 400 K.

A) 1 g/LB) 2 g/LC) 4 g/LD) 8 g/LE) 30 g/L

18. A 10.0 L container is filled with 0.40 mol H2(g), 0.80 mol O2(g), and 0.80 mol SO2(g). If the total pressure inside the flask is 800. torr, what is the partial pressure of the H2(g)?

A) 120 torrB) 160 torrC) 220 torrD) 400 torrE) 800 torr

6

Questions 19 and 20 refer to the following phase diagram.

19. At which of the lettered points on the phase diagram is more than one phase present in equilibrium?

I. D II. E III. F IV. G A) II onlyB) III onlyC) I and III onlyD) I, II, III onlyE) I, II, III and IV

20. If a substance is at position A and the temperature is increased at constant pressure until the substance is at point B, which of these statements are correct?

I. The substance melts. II. The substance changes from solid to liquid. III. The substance is a gas when heating is complete.

A) I onlyB) II onlyC) III onlyD) I and II onlyE) I, II and III

7

Questions 21 and 22 refer to a heating curve of a pure substance. Heat is being added to 100. grams of the substance at a constant rate.

21. Which of the following statements about the heating curve are true?

I. It takes more heat to vaporize the substance than to melt the substance. II. The solid has a higher specific heat than the liquid. III. Boiling occurs at a constant temperature. IV. Freezing is an exothermic process.

A) I and II onlyB) I, II, and III onlyC) I, II, and IV onlyD) I, III, and IV onlyE) I, II, III, and IV

8

22. Which of the following processes are exothermic?

I. Freezing II. Melting III. Evaporating IV. Boiling V. Condensing

A) I and V only B) II, and IV only C) I, II, and III onlyD) I, III, and V onlyE) II, III, and V only

23. How many joules of heat does it take to heat 100. g of the substance from 10ºC to 20ºC? (c = 4.2 J/g ºC)

A) 500 JB) 1000 JC) 2100 JD) 4200 JE) 5500 J

24. When a substance is converted from a liquid to a gas at its normal boiling point, which of the following are correct?

I. The potential energy of the system increases. II. The distance between the molecules increases. III. The vapor pressure of the liquid is less than 1 atm.

A) I onlyB) II onlyC) I and II onlyD) II and III onlyE) I, II and III

25. Which of the following substances would you expect to have the highest boiling point?

A) ArB) O2

C) N2

D) CH4

E) C2H4

9

Questions 26 and 27 refer to the spherical monatomic molecule pictured below having no dipole moment. The dot indicates the location of the nucleus in all of the diagrams.

26. The molecule is placed near a water molecule and experiences a dipole-induced dipole intermolecular force as a result. Which of the following best represents this interaction?

A)

δ+δ+ δ−δ−

B)

δ+δ+ δ−δ−

C)

δ− δ+δ+ δ−

D)

δ+δ− δ−δ+

E)

δ+δ− δ−δ−

10

27. The molecule is placed near an identical molecule and experiences an induced dipole-induced dipole (London dispersion) intermolecular force. Which of the following best represents this interaction?

A)

δ−δ− δ+δ+

B)

δ+δ+ δ−δ−

C)

δ+δ+ δ−δ−

D)

δ+δ− δ−δ+

E)

δ−δ− δ+δ+

11

28. All of the following exhibit hydrogen bonding EXCEPTA) HFB) NH3

C) H2OD) C2H6 E) C2H5OH

29. A 5.0 L sample of gas is heated from 15ºC to 30ºC. If the pressure remains constant, the volume would be expected to

A) doubleB) decrease to one halfC) decrease slightlyD) increase slightlyE) stay the same

30. Which of the following refer only to ideal gases, and not real gases?

I. Gases contain particles that are in constant motion. II. Gas particles have no molecular volume. III. Gas particles exhibit no intermolecular forces.

A) I onlyB) II onlyC) I, and II onlyD) II and III onlyE) I, II, and III

31. Which of the following gases has the greatest density at standard temperature and pressure?

A) Argon B) XenonC) HeliumD) NitrogenE) Carbon dioxide

32. The temperature and pressure at which all three states of matter can exist in equilibrium is called the

A) critical pointB) boiling pointC) triple pointD) equilibrium pointE) flash point

12

33. Which of the following transformations is known as sublimation?

A) liquid to gasB) gas to liquidC) solid to liquidD) solid to gasE) gas to solid

34. What type of attractive forces are being overcome when liquid oxygen boils at 90 K?A) Ionic bondsB) Covalent bondsC) Hydrogen bondsD) Dipole-dipole forcesE) Induced dipole-induced dipole (dispersion) forces

35. Which of these statements is true regarding the boiling of water at the top of a mountain?

A) The water will boil at 100oC.B) The water will boil at a temperature less than 100oC.C) The water will boil at a temperature greater than 100oC.D) The elevation of the mountain has no effect on the boiling point of water.E) The elevation of the mountain will affect the boiling point, but it is impossible to predict

whether it will be greater than or less than 100oC without the actual height of the mountain.