Cracking the SAT Chemistry Subject Test

Part IV

Practice SAT Chemistry Subject
Tests and Answers and Explanations

15 Practice SAT Chemistry Subject Test 1

16 Practice SAT Chemistry Subject Test 1: Answers and Explanations

17 Practice SAT Chemistry Subject Test 2

18 Practice SAT Chemistry Subject Test 2: Answers and Explanations

19 Practice SAT Chemistry Subject Test 3

20 Practice SAT Chemistry Subject Test 3: Answers and Explanations

Chapter 15

Practice SAT Chemistry Subject Test 1



Click here to download a PDF of the Practice SAT Chemistry Subject Test 1.

PRACTICE SAT CHEMISTRY SUBJECT TEST 1

You are about to take the first of three practice SAT Chemistry Subject Tests.

After answering questions 1–23, which constitute Part A, you'll be directed to answer questions 101–116, which constitute Part B. Then you will begin again at question 24. Questions 24–69 constitute Part C.

When you're ready to score yourself, refer to the scoring instructions and answer key on this page. Full explanations regarding the correct answers to all questions start on this page.

PRACTICE SAT CHEMISTRY

MATERIAL IN THE FOLLOWING TABLE MAY BE USEFUL IN ANSWERING THE QUESTIONS IN THIS EXAMINATION.

Click here to see full page view

CHEMISTRY SUBJECT TEST 1

Note: For all questions involving solutions and/or chemical equations, assume that the system is in pure water unless otherwise stated.

Part A

Directions: Each set of lettered choices below refers to the numbered statements or questions immediately following it. Select the one lettered choice that best fits each statement or answers each question, and then fill in the corresponding oval on the answer sheet. A choice may be used once, more than once, or not at all in each set.

Questions 1–4 refer to the following.

(A) Thermometer

(B) Conductivity tester

(C) Salt bridge

(D) Buret

(E) Graduated cylinder

1. May be used in combination with a calorimeter to compare the specific heats of two substances

2. Is used to measure the volume of a solid by water displacement

3. Useful for adding small quantities of acid into a base

4. Completes the circuit of an electrochemical cell

Questions 5–9 refer to the following.

(A) Nucleic acids

(B) Proteins

(C) Carbohydrates

(D) Lipids

(E) Electrolytes

5. Always amphoteric in nature

6. Found as both straight-chained and branched polymers

7. Deoxyribose in DNA nucleotides belongs to this family of biologically important molecules

8. Always ionic in nature

9. Tend not to be water soluble, and aggregate into droplets or molecular bilayers

Questions 10–13 refer to the following.

(A) Ag+ + Br → AgBr

(B)

(C)

(D) +

(E) 2HgO → 2Hg + O2

10. Represents the decomposition of a compound into its constituent elements

11. Represents alpha decay

12. Represents an oxidation-reduction reaction

13. Causes the neutron-to-proton ratio in a nucleus to be lowered

Questions 14–16 refer to the following.

14. Is the activation energy of the reverse reaction

15. Is the enthalpy change of the forward reaction

16. Represents energy of the activated complex

Questions 17–20 refer to the following.

(A) Hydrogen bonding

(B) Ionic bonding

(C) Metallic bonding

(D) Nonpolar covalent bonding

(E) Polar covalent bonding

17. Holds a sample of barium iodide, BaI2, together

18. Allows solids to conduct electricity

19. Attracts atoms of hydrogen to each other in an H2 molecule

20. Responsible for relatively low vapor pressure of water

Questions 21–23 refer to the following.

(A) Iron(III) chloride, FeCl3(s)

(B) Iodine, I2(s)

(C) Sodium hydroxide, NaOH(s)

(D) Sucrose, C12H22O11(s)

(E) Graphite, C(s)

21. Gives off a purplish vapor as it sublimes

22. Can conduct electricity in the solid state

23. Its dissolution in water is highly exothermic

PLEASE GO TO THE SPECIAL SECTION LABELED CHEMISTRY AT THE LOWER RIGHT-HAND CORNER OF THE ANSWER SHEET YOU ARE WORKING ON AND ANSWER QUESTIONS 101–116 ACCORDING TO THE FOLLOWING DIRECTIONS.

Part B

Directions: Each question below consists of two statements, I in the left-hand column and II in the right-hand column. For each question, determine whether statement I is true or false and whether statement II is true or false, and fill in the corresponding T or F ovals on your answer sheet.Fill in oval CE only if statement II is a correct explanation of statement I.

101.

102.

103.

104.

105.

106.

107.

108.

109.

110.

111.

112.

113.

114.

115.

116.

RETURN TO THE SECTION OF YOUR ANSWER SHEET YOU STARTED FOR CHEMISTRY AND ANSWER QUESTIONS 24–69.

Part C

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 then fill in the corresponding oval on the answer sheet.

24. What is the number of protons and neutrons in an atom with mass number 89 and atomic number 39?

(A) 50 protons and 50 neutrons

(B) 50 protons and 39 neutrons

(C) 39 protons and 89 neutrons

(D) 39 protons and 50 neutrons

(E) 39 protons and 39 neutrons

…C4H10(g) +…O2(g) →…CO2(g) +…H2O(l)

25. When the above equation is balanced using the lowest whole-number terms, the coefficient of CO2 is

(A) 2

(B) 4

(C) 8

(D) 10

(E) 13

26. Which of the following is closest in mass to a proton?

(A) Alpha particle

(B) Positron

(C) Neutron

(D) Electron

(E) Hydrogen molecule

27. What is the approximate percentage composition by mass of the element oxygen in the compound HClO4?

(A) 16%

(B) 32%

(C) 50%

(D) 64%

(E) 75%

28. If two atoms that differ in electronegativity combine by chemical reaction and share electrons, the bond that joins them will be

(A) metallic

(B) ionic

(C) a hydrogen bond

(D) nonpolar covalent

(E) polar covalent

29. When the temperature of a 20-gram sample of water is increased from 10°C to 30°C, the heat transferred to the water is

(A) 600 calories

(B) 400 calories

(C) 200 calories

(D) 30 calories

(E) 20 calories

30. What is the oxidation state of chromium, Cr, in the compound potassium dichromate, K2Cr2O7?

(A) +1

(B) +2

(C) +3

(D) +6

(E) +12

31. An aqueous solution with pH 5 at 25°C has a hydroxide ion (OH) concentration of

(A) 1 10–11 molar

(B) 1 10–9 molar

(C) 1 10–7 molar

(D) 1 10–5 molar

(E) 1 10–3 molar

2H2O(g) → 2H2(g) + O2(g)

32. The volume of water vapor required to produce 44.8 liters of oxygen by the above reaction is

(A) 11.2 liters

(B) 22.4 liters

(C) 44.8 liters

(D) 89.6 liters

(E) 100.0 liters

33. When 190 grams of MgCl2 are dissolved in water and the resulting solution is 500 milliliters in volume, what is the molar concentration of MgCl2 in the solution?

(A) 2.0 M

(B) 4.0 M

(C) 8.0 M

(D) 12.0 M

(E) 16.0 M

34. When a fixed amount of gas has its Kelvin temperature doubled and its pressure doubled, the new volume of the gas is

(A) four times greater than its original volume

(B) twice its original volume

(C) unchanged

(D) one-half its original volume

(E) one-fourth its original volume

35. In 12.4 hours, a 100 gram sample of an element decays so that its mass is 25 grams. What is the approximate half-life of this radioactive substance?

(A) 1.6 hours

(B) 3.1 hours

(C) 6.2 hours

(D) 24.8 hours

(E) 49.6 hours

36. In the equation Q → + , the species represented by Q is

(A)

(B)

(C)

(D)

(E)

37. A compound with a molecular weight of 56 amu has an empirical formula of CH2. What is its molecular formula?

(A) C2H2

(B) C2H4

(C) C4H8

(D) C4H10

(E) C6H12

38. The change in heat energy for a reaction is best expressed as a change in

(A) enthalpy

(B) absolute temperature

(C) specific heat

(D) entropy

(E) kinetic energy

…NF3(g) +…H2O(g) →…HF(g) +…NO(g) +…NO2(g)

39. When the equation for the reaction above is balanced, how many moles of NF3 would be required to react completely with 6 moles of H2O?

(A) 0.5 mole

(B) 1 mole

(C) 2 moles

(D) 3 moles

(E) 4 moles

40. Which characteristic is associated with bases?

(A) React with metal to produce hydrogen gas

(B) Donate an unshared electron pair

(C) Always contain the hydroxide ion in their structure

(D) Taste sour

(E) Formed by the reaction of a nonmetal oxide and water

41. An element has the following properties: shiny, brittle, poor electrical conductivity, and high melting point. This element can be best classified as a(n)

(A) alkali metal

(B) halogen

(C) metalloid

(D) transition metal

(E) noble gas

42. Which of the following forward processes produces a decrease in entropy?

I. H2O(g) → H2O(l)

II. Fe2+ (aq) + S2– (aq) → FeS(s)

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

(A) I only

(B) III only

(C) I and II only

(D) II and III only

(E) I, II, and III

43. Which of the following will raise the boiling point of a sample of water?

(A) Heat the water

(B) Mix gasoline into the water

(C) Bring the water sample to a higher altitude

(D) Place the water sample on a magnetic stirrer

(E) Dissolve table sugar into the water

44. Elements H and J lie in the same period. If the atoms of H are smaller than the atoms of J, then compared to atoms of J, atoms of H are most likely to

(A) exist in a greater number of isotopes

(B) exist in a lesser number of isotopes

(C) exist in a greater number of oxidation states

(D) have a greater positive charge in their nuclei

(E) have a lesser positive charge in their nuclei

…Al(s) +…O2(g)…Al2O3(s)

45. When the equation representing the reaction shown above is completed and balanced and all coefficients are reduced to lowest whole-number terms, the coefficient of O2(g) is

(A) 1

(B) 2

(C) 3

(D) 4

(E) 6

46. Which of the following solids has a brilliant blue color?

(A) Ca(OH)2

(B) KCl

(C) NaBr

(D) Fe2O3

(E) CuSO4

47. Twenty-five percent of element X exists as 210X and 75 percent of it exists as 214X. What is the atomic weight of element X in amu?

(A) 85

(B) 211

(C) 212

(D) 213

(E) 214

48. A 600-milliliter container holds 2 moles of O2(g), 3 moles of H2(g), and 1 mole of He(g). Total pressure within the container is 760 torr. What is the partial pressure of O2?

(A) 127 torr

(B) 253 torr

(C) 380 torr

(D) 507 torr

(E) 760 torr

Fe(OH)3(s) Fe3+(aq) + 3OH(aq)

49. The ionic solid Fe(OH)3 is added to water and dissociates into its component ions, as shown above. The solubility product expression for the saturated solution is

(A) Ksp = [Fe3+] [OH]

(B) Ksp = [Fe3+] [3OH]

(C) Ksp = [Fe3+] [3OH]3

(D) Ksp = [Fe3+] [OH]3

(E) Ksp =

50. Which of the following electron configurations represents an atom of magnesium in an excited state?

(A) 1s22s22p6

(B) 1s22s22p63s2

(C) 1s22s22p53s23p2

(D) 1s22s22p63s13p1

(E) 1s22s22p63s13p2

51. All of the following when added to water will produce an electrolytic solution EXCEPT

(A) N2(g)

(B) HCl(g)

(C) KOH(s)

(D) NaI(s)

(E) CaCl2(s)

NH3 (aq) + H2CO3 (aq) NH4+(aq) + HCO3 (aq)

52. In the reaction represented above, NH4+ acts as a(n)

(A) indicator

(B) hydrate

(C) acid

(D) base

(E) salt

53. Which species has the ground state electron configuration 1s22s22p63s23p6?

(A) Sulfide ion, S2–

(B) Bromide ion, Br

(C) Neon atom, Ne

(D) Chromium ion, Cr3+

(E) Potassium atom, K

54. Which of the following species is amphoteric?

(A) Na3PO4

(B) HSO4

(C) KOH

(D) HNO3

(E) C2O2–4

55. An ideal gas has a volume of 10 liters at 20°C and a pressure of 750 mmHg. Which of the following expressions is needed to determine the volume of the same amount of gas at STP?

(A)

(B)

(C)

(D)

(E)

Questions 56–57 pertain to the phase diagram for substance Z below.

56. Substance Z is at 0.5 atm and 200 K. If the pressure on substance Z is steadily increased and its temperature is kept constant, what phase change will eventually occur?

(A) Condensation

(B) Freezing

(C) Melting

(D) Sublimation

(E) Vaporization

57. The normal boiling point of substance Z is closest to

(A) 100 K

(B) 200 K

(C) 300 K

(D) 400 K

(E) 500 K

58. The shape of a PCl3 molecule is described as

(A) bent

(B) trigonal pyramidal

(C) linear

(D) trigonal planar

(E) tetrahedral

59. What volume of 0.4 M Ba(OH)2 (aq) is needed to exactly neutralize 100 milliliters of 0.2 M HBr(aq)?

(A) 25 mL

(B) 50 mL

(C) 100 mL

(D) 200 mL

(E) 400 mL

60. Which of the following is true regarding the aqueous dissociation of HCN, Ka = 4.9 × 10–10 at 25°C?

I. At equilibrium, [H+] = [CN]

II. At equilibrium, [H+] > [HCN]

III. HCN(aq) is a strong acid.

(A) I only

(B) II only

(C) I and II only

(D) II and III only

(E) I, II, and III

61. Which of the following atoms has the largest second ionization energy?

(A) Silicon, Si

(B) Calcium, Ca

(C) Chlorine, Cl

(D) Iron, Fe

(E) Sodium, Na

Question 62 refers to the overall reaction and half-reactions with standard reduction potentials below.

2Fe2+ + Cl2 → 2Fe3+ + 2Cl

Fe3+ + e → Fe2+; Eored = 0.77 volts

Cl2 + 2e → 2Cl; Eored = 1.36 volts

62. The standard potential difference of an electro-chemical cell using the overall reaction above is

(A) 0.18 volts

(B) 0.59 volts

(C) 1.05 volts

(D) 2.13 volts

(E) 2.90 volts

63. The reaction of zinc metal, Zn, and hydrochloric acid, HCl, produces which of the following?

I. H2(g)

II. Cl2(g)

III. Zn2+(aq)

(A) II only

(B) III only

(C) I and II only

(D) I and III only

(E) I, II, and III

Questions 64–66 refer to the following reaction.

2H2S(g) + 3O2(g) 2SO2(g) + 2H2O(g) + heat

64. For the above reaction, the equilibrium concentration of SO2(g) can be increased by

(A) adding neon gas

(B) increasing the temperature

(C) adding a catalyst

(D) increasing the concentration of H2O(g)

(E) increasing the concentration of O2(g)

65. Which of the following is increased by decreasing the volume of the reaction system?

I. Rate of reaction

II. Equilibrium concentration of reactants

III. Value of Keq

(A) I only

(B) III only

(C) I and II only

(D) II and III only

(E) I, II, and III

Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)

66. When 3 moles of Fe2O3 are allowed to completely react with 56 grams of CO according to the above equation, approximately how many moles of iron, Fe, are produced?

(A) 0.7

(B) 1.3

(C) 2.0

(D) 2.7

(E) 6.0

2Na2O2(s) + 2H2O(l) → 4NaOH(aq) + O2(g)

67. Sodium peroxide, Na2O2, and water react in the flask at 25°C according to the equation and in the diagram above. If water levels are equal inside and outside the beaker, then the gas pressure inside the beaker is equal to the

(A) pressure of oxygen gas collected

(B) vapor pressure of water at 25°C

(C) sum of pressure of oxygen gas collected and atmospheric pressure

(D) sum of vapor pressure of water at 25°C and atmospheric pressure

(E) sum of pressure of oxygen gas collected and vapor pressure of water at 25°C

68. Which of the following molecules has the strongest carbon-to-carbon bond?

(A) C2H2

(B) C2H4

(C) C2H6

(D) C3H8

(E) C4H10

N2O4(g) 2NO2(g)

The following concentration data were gathered for the above reaction at 5 minute intervals from the start of an experiment:

Time After Start of Experiment

[N2O4]

[NO2]

0 min (start)

0.00 M

0.50 M

5 min

0.10 M

0.33 M

10 min

0.20 M

0.20 M

15 min

0.25 M

0.15 M

20 min

0.28 M

0.13 M

25 min

0.28 M

0.13 M

69. If the experiment was carried out in a closed system at constant temperature, then during which time interval (from the start of the experiment) did the reaction most likely achieve equilibrium?

(A) 0 min (start) to 5 min

(B) 5 min to 10 min

(C) 10 min to 15 min

(D) 15 min to 20 min

(E) 20 min to 25 min

STOP

If you finish before time is called, you may check your work on this section only.
Do not turn to any other section in the test.

HOW TO SCORE THE PRINCETON REVIEW PRACTICE SAT CHEMISTRY SUBJECT TEST

When you take the real exam, the proctors will collect your test booklet and bubble sheet and send your answer sheet to New Jersey, where a computer looks at the pattern of filled-in ovals on your answer sheet and gives you a score. We couldn't include even a small computer with this book, so we are providing this more primitive way of scoring your exam.

Determining Your Score

STEP 1

Using the answer key on the next page, determine how many questions you got right and how many you got wrong on the test. Remember: Questions that you do not answer don't count as either right or wrong answers.

STEP 2

List the number of right answers here.

(A) ________

STEP 3

List the number of wrong answers here. Now divide that number by 4. (Use a calculator if you're feeling particularly lazy.)

(B) ________ ÷ 4 = (C) ________

STEP 4

Subtract the number of wrong answers divided by 4 from the number of correct answers. Round this score to the nearest whole number. This is your raw score.

A) ________ – (C) ________ = ________

STEP 5

To determine your real score, take the number from Step 4 above, and look it up in the left column of the Score Conversion Table on this page; the corresponding score on the right is your score on the exam.

ANSWERS TO THE PRINCETON REVIEW PRACTICE SAT CHEMISTRY SUBJECT TEST 1

THE PRINCETON REVIEW PRACTICE SAT CHEMISTRY SUBJECT TEST SCORE CONVERSION TABLE