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Student’s name:___________________________________

Student’s ID:______________________________________

Mock Final Exam

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1. Which of the following statements is incorrect?

A. The condensation of steam on a mirror is an example of a physical change.

B. The burning of a piece of charcoal to a white powder is an example of a physical change.

C. Evaporation of water from a fish tank is evidence of a physical change.

D. The fact that sulfur is a yellow powder is a physical property.

E. The fact that copper conducts electricity is a physical property.

2. Which of the following is not an example of a physical property?

A. The boiling point of acetone is 56C.

B. Sand is more dense than water.

C. Helium is a gas at room temperature.

D. Copper gets a greenish coating on it when exposed to moist air.

E. Water is colorless.

3. Which of the following is not normally a part of scientific inquiry?

A. observations

B. philosophizing

C. theories

D. hypotheses

E. laws

4. Which of the following is the correct formula for the nitrite ion?

A. N2

B. NO2–

C. NO3–

D. N23–

E. N3–

5. Which combination of formula and name is incorrect?

A. Na+ = sodium ion

B. Ca2+ = calcium ion

C. N2– = nitride ion

D. F = fluoride ion

E. O2= oxide ion

6. Which of the following combinations of formula and name is incorrect?

A. hydroxide ion = OH–

B. nitrate ion = NO3–

C. sulfide ion = SO32–

D. nitrite ion = NO2–

E. sulfate ion = SO42–

7. Based on common charges, which formula for an ionic compound is incorrect?

A. CaCl

B. NaF

C. SrO

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D. MgS

E. K3P

8. Based on common charges, which formula for an ionic compound is incorrect?

A. LiCO3

B. NaBr

C. CaO

D. SrS

E. MgCl2

9. Which of the following formulas for a compound containing the Cr2+ ion is incorrect?

A. CrClO4

B. CrSO4

C. CrO

D. CrS

E. CrCl2

10. What is the correct formula for the compound chromium(III) sulfide?

A. CrS

B. Cr3S

C. CrS3

D. Cr3S2

E. Cr2S3

11. Write and balance the equation for the combination reaction that occurs when sulfur dioxide gas, SO2, reacts with oxygen

gas.

A. 3SO2(g) + 2O2(g) 3SO3(g)

B. SO2(g) + O2(g) SO3(g)

C. SO2(g) + O2(g) SO4(g)

D. 2SO2(g) + 2O2(g) 2SO3(g)

E. 2SO2(g) + O2(g) 2SO3(g)

12. When copper metal is placed into a silver nitrate solution, a single-displacement reaction occurs, forming a copper(II)

compound. Write a balanced equation to describe this reaction.

A. Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)

B. Cu(s) + Ag(NO3)2(aq) CuNO3(aq) + AgNO3(aq)

C. Cu(s) + Ag(NO3)2(aq) Cu(NO3)2(aq) + Ag(s)

D. 2Cu(s) + Ag(NO3)2(aq) 2Cu(NO3)2(aq) + Ag(s)

E. Cu(s) + AgNO3(aq) CuNO3(aq) + Ag(aq)

13. When copper metal is placed in a solution of platinum(II) chloride, will a reaction occur? If so, what is the balanced

equation for the reaction?

A. Cu(s) + Pt2Cl(aq) CuCl(aq) + 2Pt(aq)

B. Yes. Cu(s) + PtCl2(aq) CuCl(aq) + PtCl(aq)

C. No reaction will occur.

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D. Yes. Cu(s) + Pt2Cl(aq) CuCl(aq) + Pt(aq)

E. Yes. Cu(s) + PtCl2(aq) CuCl2(aq) + Pt(s)

14. Which of the following ionic compounds would be expected to be insoluble in water?

A. Li2SO4

B. AgI

C. Ca(CH3CO2)2

D. NaCl

E. KOH

15. Consider the reaction Ca(OH)2(aq) + 2HCl(aq) CaCl2(aq) + 2H2O(l). The driving force that causes the reaction to go to

completion is:

A. formation of water.

B. formation of a soluble salt.

C. formation of a precipitate.

D. formation of an insoluble gas.

E. formation of an element.

16. When aqueous solutions of K2CO3 and CaCl2 are mixed, what is the correct formula for the precipitate that forms?

A. ClCO3(s)

B. KCl(s)

C. K2Cl2(s)

D. CaCO3(s)

E. K2Ca(s)

17. Complete and balance the equation for the reaction that occurs when H2SO4(aq) and NaOH(aq) are mixed.

A. H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)

B. H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + H2O(l)

C. 2H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)

D. H2SO4(aq) + NaOH(aq) NaSO4(aq) + H2O(l)

E. H2SO4(aq) + NaOH(aq) NaSO4(aq) + H2(g)

18. Sterno, or “canned heat,” contains methanol, CH3OH, and is used for heating containers of food. Write a balanced equation

to represent the combustion reaction that occurs when methanol burns in air.

A. CH3OH(l) + O2(g) CO2(g) + H2O(g)

B. 2CH3OH(l) + 6O2(g) 2CO2(g) + 4H2O(g)

C. 2CH3OH(l) + 3O2(g) 2CO2(g) + 4H2O(g)

D. 2CH3OH(l) + O2(g) C2O2(g) + H2(g)

E. CH3OH(l) + O2(g) CH4O3(g)

19. Would an aqueous solution of CH3OH contain ions? If so, indicate the formulas of the ions in the solution.

A. Yes. CH4+(aq) + Oˉ(aq)

B. Yes. CH3ˉ(aq) + OH+(aq)

C. Yes. CH3+(aq) + OHˉ(aq)

D. Yes. CH42+(aq) + O2ˉ(aq)

E. No, this substance would not form ions in solution.

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20. Would an aqueous solution of KOH contain ions? If so, indicate the formulas of the ions in the solution.

A. Yes. K+(aq) + O2ˉ(aq) + H+(aq)

B. No, this substance would not form ions in solution.

C. Yes. K+(aq) + H2O(l)

D. Yes. K+(aq) + OHˉ(aq)

E. Yes. Kˉ(aq) + OH+(aq)

21. Write and balance a net ionic equation for the reaction between hydrochloric acid and potassium hydroxide.

A. H+(aq) + OHˉ(aq) H2O(l)

B. H+(aq) + O2ˉ(aq) OHˉ(aq)

C. HCl(aq) + KOH(aq) KCl(aq) + H2O(l)

D. Clˉ(aq) + OH+(aq) OHCl(aq)

E. K+(aq) + Clˉ(aq) KCl(aq)

22. Identify the spectator ion in the following reaction: Zn(s) + Cu(NO3)2(aq) Cu(s) + Zn(NO3)2(aq)

A. Cu2+(aq) and NO3–(aq)

B. Zn2+(aq) and Cu2+(aq)

C. Zn2+(aq) and NO3–(aq)

D. NO3–(aq) only

E. There are no spectator ions.

23. Given that 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g), if 4.5 moles of NH3 react with sufficient oxygen, how many moles of

H2O should form?

A. 4.0

B. 4.5

C. 6.0

D. 6.8

E. 5.5

24. Given the balanced equation 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g), if 82.0 g of NH3 react with sufficient oxygen, how

many grams of NO should form?

A. 145 g

B. 5.80 x 102 g

C. 46.5 g

D. 186 g

E. 11.6 g

25. When a 0.525 g piece of zinc is placed in a solution of copper(II) sulfate, copper metal and zinc sulfate are formed. Balance

the equation for the reaction, and determine the mass of copper(II) sulfate that would react with this quantity of

zinc. ___ Zn(s) + ___CuSO4(aq) ___ZnSO4(aq) + ___Cu(s) (unbalanced)

A. 65.4 g

B. 0.641 g

C. 1.28 g

D. 2.56 g

E. 159 g

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26. If you have eight bicycle wheels and five frames, how many bikes could you build (assuming that each bike requires one

frame and two wheels), and what would be left over?

A. Four bikes could be built, and nothing would be left over.

B. Four bikes could be built, and one frame would be left over.

C. Five bikes could be built, and three wheels would be left over.

D. Five bikes could be built, and nothing would be left over.

E. Three bikes could be built, and two frames would be left over.

27. Phosphorus trichloride can be made by the following reaction: P4(s) + 6Cl2(g) 4PCl3(l) What is the maximum amount of

phosphorus trichloride that can be formed if 10 molecules of P4 are mixed with 36 molecules of chlorine?

A. 4 molecules

B. 6 molecules

C. 12 molecules

D. 24 molecules

E. 46 molecules

28. What mass (in grams) of SF6 should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of

fluorine? S + 3F2 SF6

A. 24.0

B. 6.40

C. 11.1

D. 32.0

E. 16.0

29. If the theoretical yield for a reaction is 54.9 g, and 51.3 g of product are actually obtained, the percent yield is:

A. 0.934%

B. 93.4%

C. 107%

D. 3.60%

E. not enough information given

30. What is the ground-state electron configuration for the oxide ion?

A. 1s22s22p2

B. 1s22s22p4

C. 1s22s22p6

D. 1s22p6

E. 1s22p8

31. The electron configuration 1s22s22p63s23p6 applies to all of the following species except:

A. Cl-

B. Ar

C. Ca2+

D. Na+

E. K+

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32. Which element has the abbreviated ground-state electron configuration [Ar]4s23d8?

A. Co

B. Ni

C. Kr

D. Cu

E. Ca

33. Predict the molecular shape and give the approximate bond angles of the SO2 molecule.

A. linear, 180

B. trigonal planar, 120

C. tetrahedral, 109.5

D. trigonal pyramidal, 109.5

E. bent, 120

34. Which of the following molecules is a nonpolar molecule with polar bonds?

A. NF3

B. CH2Cl2

C. CF4

D. O3

E. CO

35. Which of the following molecules is polar?

A. CCl4

B. H2S

C. SO3

D. CO2

E. BeF2

36. Which of the following molecules or ions would exhibit resonance?

A. C2H2

B. Br2

C. CO32‾

D. CO

E. SiH4

37. How many equivalent resonance structures best represent(s) the NO2– ion?

A. 1

B. 2

C. 3

D. 4

E. It does not exhibit resonance.

38. If a 1.50 L gas sample is held at a constant temperature, and its pressure is changed from 2.30 atm to 3.60 atm, what will the

final volume be?

A. 1.50 L

B. 3.45 L

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C. 0.958 L

D. 8.28 L

E. 0.828 L

39. If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at

constant temperature?

A. 5.50 atm

B. 2.50 atm

C. 7.50 atm

D. 1.88 atm

E. 0.533 atm

40. If the temperature of a gas at a constant pressure is increased, the volume will

A. become smaller because of fewer collisions with the sides of the container.

B. become larger because of fewer collisions with the sides of the container.

C. become smaller because of more collisions with the sides of the container.

D. become larger because of more collisions with the sides of the container.

E. stay the same because temperature has no effect on pressure.

41. A given mass of gas in a rigid container is heated from 100oC to 500oC. Which of the following best describes what will

happen to the pressure of the gas?

A. The pressure will remain the same.

B. The pressure will decrease by a factor of five.

C. The pressure will increase by a factor of five.

D. The pressure will increase by a factor less than five.

E. The pressure will increase by a factor greater than five.

42. Given a fixed amount of gas in a rigid container (no change in volume), what pressure will the gas exert if the pressure is

initially 1.50 atm at 22.0oC, and the temperature is changed to 11.0oC?

A. 0.750 atm

B. 3.00 atm

C. 1.56 atm

D. 1.44 atm

E. 301 atm

43. Given a fixed amount of gas in a rigid container (no change in volume), what temperature will the gas have to be changed to

if the pressure is initially 3.50 atm at 22.0oC, and the desired final pressure is 1.75 atm?

A. 126oC

B. 11.0oC

C. 44.0oC

D. 148oC

E. 148oC

44. For which of the following changes is it not clear whether the volume of a particular sample of an ideal gas will increase or

decrease?

A. increase the temperature and increase the pressure

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B. decrease the temperature and increase the pressure

C. increase the temperature and decrease the pressure

D. increase the temperature and keep the pressure constant

E. keep temperature constant and decrease the pressure

45. Calculate the number of moles and the mass of gas in 10.2 L of O2 at STP.

A. 0.455 mol, 7.28 g

B. 0.455 mol, 14.6 g

C. 228 mol, 7.14 g

D. 228 mol, 3648 g

E. 1.00 mol, 32.0 g

46. Calculate the density of NO2 in g/L at STP.

A. 22.41 g/L

B. 2.053 g/L

C. 1.031 x 103 g/L

D. 0.04462 g/L

E. 0.4871 g/L

47. If a 7.00 L container is filled with O2 to a pressure of 995 torr at 33.0C, calculate the mass of the oxygen in the container.

A. 11.7 g

B. 0.365 g

C. 277 g

D. 2.57 x 103 g

E. 0.0854 g

48. Under which conditions does sulfur trioxide (SO3) have the greatest molar volume?

A. high temperature and low pressure

B. low temperature and high pressure

C. high temperature and high pressure

D. low temperature and low pressure

E. The molar volume is always 22.414 L.

49. Rank the following substances in order of increasing average velocity, assuming they are all at the same temperature: O2,

CO2, Ar, He

A. O2 < CO2 < Ar < He

B. CO2 < Ar < O2 < He

C. Ar < O2 < CO2 < He

D. CO2 < O2 < Ar < He

E. He < O2 < Ar < CO2

50. What phase transition is occurring between points B and C on the heating curve?

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A. melting

B. condensation

C. evaporation

D. sublimation

E. deposition

51. What phase transition is occurring between points D and E on the cooling curve?

A. melting

B. freezing

C. evaporation

D. sublimation

E. deposition

52. Which of the following is not an attractive force that acts between the individual molecules of CH3OH?

A. London dispersion forces

B. dipole-dipole forces

C. hydrogen-bonding forces

D. covalent bonds

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E. none of these is correct

53. Which of the following molecules experience dipole-dipole forces?

A. NO2

B. CO2

C. CBr4

D. SO3

E. all of these choices are correct

54. Which of the following substances can participate in hydrogen bonding?

A. SiH4

B. CH2Cl2

C. H2O

D. PH3

E. C and D

55. Which of the following increases the solubility of a gas in solution?

A. increasing gas pressure and increasing temperature

B. increasing gas pressure and decreasing temperature

C. decreasing gas pressure and increasing temperature

D. decreasing gas pressure and decreasing temperature

E. adding more water

56. If the solubility of a solid substance is 18.2 g/100 g water, which of the following best describes what eventually forms after

10.0 grams of the substance is mixed with 50.0 grams of water?

A. a saturated solution with some undissolved solid

B. an unsaturated solution with some undissolved solid

C. a saturated solution with no undissolved solid

D. an unsaturated solution with no undissolved solid

E. a supersaturated solution

57. The rate of a reaction can be increased by all of the following except

A. increasing the temperature.

B. increasing the concentration of the reactants.

C. increasing the surface area of the reactants.

D. adding a catalyst.

E. increasing the volume of the reaction vessel.

58. According to collision theory, the increase in the rate constant with increasing temperature is due mostly to the fact that

A. the activation energy decreases with increasing temperature.

B. the fraction of the collisions having sufficient energy to react increases with increasing temperature.

C. the pressure of the reactants increases with increasing temperature.

D. the heat change for most reactions is negative.

E. the fraction of the collisions that have the proper orientation for reaction increases with increasing temperature.

59. The kinetics of a reaction is studied at 25C and at 50C. Which of the following statements is correct?

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A. The rate of the reaction at 50C will be lower than the rate at 25C, since the molecules will be moving too fast to collide

effectively.

B. The rate of the reaction at 50C will be twice that of the rate at 25C, since the temperature has doubled.

C. The rate of the reaction at 50C will be greater than the rate at 25C, since the activation energy will be lower at the higher

temperature.

D. The rate of the reaction at 50C will be greater than the rate at 25C, since a greater fraction of the molecules will possess

sufficient energy to react at the higher temperature.

E. None of these statements is correct.

60. Select the two Brønsted-Lowry acids in the following equation: HNO2(aq) + H2O(l) ⇌ NO2-(aq) + H3O+(aq)

A. HNO2 and H2O

B. HNO2 and NO2-

C. HNO2 and H3O+

D. H2O and H3O+

E. NO2- and H3O+