®SAT II Chemistry Subject Test OFFICIAL TESTS & PRACTICE TESTS Page 1 of 136 TABLE OF CONTENTS 4 Princeton Practice Test 1 CHAPTER 1 17 CHAPTER 2 Princeton Practice Test 2 32 CHAPTER 3 Princeton Practice Test 3 44 CHAPTER 4 Barron’s Practice Test 1 56 Barron’s Practice Test 2 CHAPTER 5 68 Barron’s Practice Test 3 CHAPTER 6 80 CHAPTER 7 Barron’s Practice Test 4 92 CHAPTER 8 McGraw-Hill’s Practice Test 1 104 McGraw-Hill’s Practice Test 2 CHAPTER 9 114 CHAPTER 10 McGraw-Hill’s Practice Test 3 125 CHAPTER 11 McGraw-Hill’s Practice Test 4 Page 2 of 136 Page 3 of 136 ® Practice Test 1 SAT II Chemistry Princeton Page 4 of 136 . Page 5 of 136 . Page 6 of 136 . Page 7 of 136 . Page 8 of 136 . Page 9 of 136 . Page 10 of 136 . Page 11 of 136 . Page 12 of 136 . Page 13 of 136 . Page 14 of 136 . Page 15 of 136 . Page 16 of 136 . ® Practice Test 2 SAT II Chemistry Princeton Page 17 of 136 . Page 18 of 136 . Page 19 of 136 . Page 20 of 136 . Page 21 of 136 . Page 22 of 136 . Page 23 of 136 . 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Page 72 of 136 . Page 73 of 136 . Page 74 of 136 . Page 75 of 136 . Page 76 of 136 . Page 77 of 136 Page 78 of 136 Page 79 of 136 ® Practice Test 4 SAT II Chemistry Barron’s Page 80 of 136 . Page 81 of 136 . Page 82 of 136 . Page 83 of 136 . Page 84 of 136 . Page 85 of 136 . Page 86 of 136 . Page 87 of 136 . Page 88 of 136 . Page 89 of 136 . Page 90 of 136 . Page 91 of 136 . ® Practice Test 1 SAT II Chemistry McGraw-Hill’s Page 92 of 136 . assume that the system is in pure water. An atom of the same element that differs by the num- ber of neutrons 3. Will migrate through a salt bridge to the anode half cell GO ON TO THE NEXT PAGE Page 93 of 136 . Part A Directions: Each of the following sets of lettered choices refers to the numbered formulas or statements immediately below it. Cannot be broken down chemically 4. for all statements involving chemical equations and/or solutions. more than once. Then fill in the corresponding oval on the answer sheet.PRACTICE TEST 1 199 PRACTICE TEST 1 Time: 60 minutes Note: Unless otherwise stated. Each choice in a set may be used once. Questions 1– 4 (A) Anions (B) Cations (C) Element (D) Isotope (E) Atom 1. For each numbered item. choose the one lettered choice that fits it best. or not at all. A positive ion 2. Sodium salt 7. Yields hydroxide ions as the only negative ions in solution 9. Proton donor GO ON TO THE NEXT PAGE Page 94 of 136 . Used to detect radioactivity 11. Mercury Questions 8–10 (A) Arrhenius acid (B) Arrhenius base (C) Lewis acid (D) Lewis base (E) Brønsted-Lowry acid 8. Chlorine 14. Electron pair acceptor 10. Potassium permanganate 6.200 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued Questions 5–7 Questions 11–14 (A) Calorimeter (A) Purple solution (B) Geiger Counter (B) Brown-orange liquid (C) Burette (C) Green gas (D) Funnel (D) Silver-gray liquid (E) Bunsen burner (E) Yellow-orange when burned in a flame 5. Used to deliver acids and bases in a titration 12. Can be lined with moist filter paper to catch insoluble solids 13. A reaction is nonspontaneous 23. Group 10 20. and gas phases 21. Oxidation number of calcium in calcium phosphate Questions 18–21 (A) Alkali metals (B) Alkaline earth metals (C) Transition metals (D) Halogens (E) Noble or inert gases 18. Group 1 19. Oxidation number of O in H2O2 16. liquid. and randomness 24. Will form chlorides with the formula of MCl2 GO ON TO THE NEXT PAGE Page 95 of 136 .PRACTICE TEST 1 201 PRACTICE TEST—Continued Questions 15–17 Questions 22–25 (A) E° is positive (A) 1+ (B) ∆S is negative (B) 1− (C) ∆G is positive (C) 0 (D) Keq is greater than 1 (D) 2+ (E) Ka is very large (E) 3+ 15. Indicates a strong acid 22. Oxidation number of F in HF 17. Contains elements in the solid. disorder. Oxidation number of O in O3 25. Less chaos. Bromine has an atomic mass of 79. −273 degrees Celsius is also known as BECAUSE C = K + 273. 106.9 BECAUSE about 50% of all bromine atoms are 79Br and the other 50% are 81Br. 103. 102. SAMPLE: EX 1. 108. absolute zero 104. SAMPLE ANSWER I II CE* EX 1 F F I II 101.202 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued PLEASE GO TO THE SPECIAL SECTION AT THE LOWER LEFT-HAND CORNER OF YOUR ANSWER SHEET LABELED “CHEMISTRY” AND ANSWER QUESTIONS 101–115 ACCORDING TO THE FOLLOWING DIRECTIONS. 107. Part B Directions: Each question below consists of two statements. the volume of the volume is considered to be an inverse gas will decrease. The burning of a piece of paper is a BECAUSE once burned. As you go from left to right across the BECAUSE as you go from left to right across the periodic periodic table the elements tend to table the elements tend to lose electrons. relationship 105. become more metallic in character GO ON TO THE NEXT PAGE Page 96 of 136 . determine whether statement I in the left- most column is true or false and whether statement II in the rightmost column is true or false. Fill in the oval labeled “CE” only if statement II correctly explains statement I. Methane is defined as a compound BECAUSE methane can be broken down chemically. Fill in the corresponding T or F ovals on the answer sheet provided. the chemical properties of the paper physical change remain the same. The nucleus of an atom has a BECAUSE the only positive particles positive charge found in the atom’s nucleus are protons. A liquid can boil at different BECAUSE the atmospheric (or surrounding) pressure can temperatures vary. For each question. Excited tungsten atoms will give off light BECAUSE as the excited electrons return to their ground state energy they emit energy in the form of light. The relationship between pressure and BECAUSE as pressure increases on a gas. The bonds found in a molecule of N2 are BECAUSE there is an equal sharing of electrons between the nonpolar covalent nitrogen atoms. The empirical formula of C6H12O6 is BECAUSE the empirical formula shows the lowest ratio of the CH2O elements present in the molecular formula. 111. 113. Ethane is considered to be a saturated BECAUSE ethene has a triple bond. hydrocarbon GO ON TO THE NEXT PAGE Page 97 of 136 . F2 → 2F1− + 2e− is a correctly written half BECAUSE this half reaction must demonstrate proper reaction conservation of mass and charge. 115. electricity 112. A solution of NaCl will conduct BECAUSE NaCl will not form ions in solution. Cl1− is the conjugate base of HCl BECAUSE a conjugate base is formed once a Brønsted-Lowry acid accepts a proton.PRACTICE TEST 1 203 PRACTICE TEST—Continued 109. 110. Increasing the concentration of reactants BECAUSE more reactants lowers the activation energy of a will cause a reaction to proceed faster reaction. 114. 05 mL (D) Methane (E) Potassium bromide mL of base used 28.75 M neutral. Which of the following would not be attracted or 30. (C) The pH is 6 and the solution is acidic. What will be the products of the following double (D) 0.00 M (A) Ammonium nitrate and barium nitrate (B) Barium nitrate and ammonium phosphate 32.0 × 10−6 M and the solution is basic.0 × 10−8 M and the solution is Acid: initial burette reading 14. Beta particle (B) 2. 26.6 × 10−10 (A) I only (D) 4.00 M NaOH to (E) I.15 mL (A) The pH is 8 and the solution is acidic.0 × 10−6 M? Acid: final burette reading 44. Which substance below is resonance stabilized by molarity of the solution of HCl? delocalized pi electrons? (A) Benzene (B) Hydrochloric acid Base: final burette reading 21. What is the 27. Which of the following is not a synthetic polymer? (C) Barium phosphate and sodium nitrate (A) Polyvinyl chloride (D) Ammonium nitrate and barium phosphate (B) Plastic (E) Ammonium nitrite and barium nitrate (C) Polystyrene (D) Polyethylene (E) Cellulose GO ON TO THE NEXT PAGE Page 98 of 136 . Neutron (C) 6. and III find the unknown molarity of a solution of HCl. The student records the data as shown below.10 M replacement? (NH4)3PO4 + Ba(NO3)2 → (E) 2. Select the one answer that is best in each case and then fill in the corresponding oval on the answer sheet provided. (B) The [H1+] = 1. (E) The [H1+] = 1.05 mL (C) Hydrogen gas Base: initial burette reading 6.7 × 10−8 III.9 × 10−3 (B) II only (E) 5.25 M 29. mL of acid used (D) The [H1+] = 1.2 × 10−4 (C) I and II only (D) I and III only 31.0 × 10−14 M and the solution is (A) 0. Which of the following is true about a solution that has [OH1−] = 1. Which Ka value is that of an acid that is the weakest deflected while traveling through an electric field? electrolyte? I. (B) 0. Gamma ray (A) 1.204 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued Part C Directions: Each of the multiple-choice questions or incomplete sentences below is followed by five answers or comple- tions.7 × 10−7 II.15 mL basic. II.50 M (C) 0. A student performs a titration using 1. 0 grams.4 liters (C) N2 (D) 44.0 M (C) 40% (C) 1. 34.5 liters of solution? (A) 25% (A) 19. (B) 154 grams/mole (C) The bonding gives the molecule a tetrahedral (C) 67 grams/mole shape. 37.01 × 1023 mole- 2H2(g) + O2(g).33 M (E) 75% (E) 1. (D) 83 grams/mole (D) The bonds between the atoms are ionic bonds.75 M (D) 53% (D) 0.25 grams (molar mass = 180)? of NaCl dissolved to make 1. CH2O? (A) The carbon atom is sp hybridized.) reaction at equilibrium? 2W(aq) + X(l) ←→ 3Y(aq) + 2Z(s) (A) [ Z ] [ Y ] 2 3 [W] [X]2 (B) [ W2] [ X3] 2 [Z] [Y] (C) [ Y ]3 [ W ]2 (D) [ Z ][ Y ] Figure 1 [ W ][ X ] (A) Evaporation (E) [ W ][ X ] (B) Deposition [ Z ][ Y ] (C) Condensation (D) Freezing 38. A sample of a gas at STP contains 3.5 M (B) 33% (B) 3.6 liters (E) NO GO ON TO THE NEXT PAGE Page 99 of 136 . Which process is represented by the arrow on the fol. What is the molarity of a solution that has 29.6 liters (A) CO2 (B) 11. 35.0 M 36.8 liters (D) CO (E) 89. How many liters of hydrogen gas can cules and has a mass of 22. This gas is most be produced by the breakdown of 72 grams of water? likely (A) 5.2 liters (B) O2 (C) 22. Which statement best describes the bonding found in (E) Sublimation formaldehyde. What is the percent composition of oxygen in C6H12O6 39. The following reaction occurs at STP: 2H2O(l) → 40. What is the molar mass of Ca3(PO4)2? (B) There are three sigma bonds and one pi bond (A) 310 grams/mole present. What is the mass-action expression for the following lowing phase diagram? (See Figure 1. (E) 115 grams/mole (E) All of the bonds are nonpolar bonds.PRACTICE TEST 1 205 PRACTICE TEST—Continued 33. The organic reaction: C2H6 + Cl2 → HCl + C2H5Cl is (B) 180 grams best described as (C) 540 grams (A) a substitution reaction (D) 3 grams (B) an addition reaction (E) 90 grams (C) an esterification (D) a dehydration synthesis (E) a fermentation GO ON TO THE NEXT PAGE Page 100 of 136 .0 × 10−6 (B) +50 kcal (B) 9.206 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 41. Which fraction would be used to find the new volume 47. Enough CaSO4(s) is dissolved in water at 298 K to produce a saturated solution. Which of the following statements is not true about of a gas at 760 torr under its new pressure at 900 torr acid rain? if the temperature is kept constant? (A) Acid rain will erode marble statues. Which mole sample of the solids below is best for (A) HCl(aq) + NaOH(aq) → melting a 500-gram sheet of ice on a sidewalk? (B) KBr + NaCl → (A) NaCl (C) AgNO3 + MgCl2 → (B) CaCl2 (D) CaCl2 + KI → (C) KBr (E) NaNO3 + HC2H3O2 → (D) AgNO3 (E) NaC2H3O2 44.7 (D) Acid rain creates holes in the ozone layer. (A) 54 grams 45. (A) 900 / 760 (B) Acid rain can change the pH of lakes and (B) 1. Which of the following reactions forms a salt that will precipitate out of solution? 48. how many grams C6H12O6 (molar (C) 2NO2(g) ←→ N2O4(g) mass is 180 grams/mole) can be made? Assume an (D) H2(g) + I2(g) ←→ 2HI(g) unlimited supply of carbon dioxide for the plant to (E) 2W(g) + X(g) ←→ 3Y(g) + 2Z(s) consume as well. (D) 658. If 54 grams of water are con- (B) N2(g) + 3H2(g) ←→ 2NH3(g) sumed by the plant.18 streams. (C) 760 / 900 (C) Acid rain can be formed from carbon dioxide. The Ksp value for (2W + 3X → 2Z + 2Y ∆H = −150 kcal) CaSO4 will be (A) −550 kcal (A) 6. 43.0 × 10−3 (E) +250 kcal (E) 3.0 × 10−3M. Which system at equilibrium will not be influenced by a change in pressure? 49. (E) 798. The concentration of (W + X → 2Y ∆H = −200 kcal) Ca2+ ions is found to be 3. What is the value of ∆H for the reaction: X + 2Y → 2Z? 46.7 / 798.0 × 10−3 (D) −350 kcal (D) 9.7 / 658.0 × 10−3 42.7 (E) Acid rain can be formed from the gases SO2 and SO3. Given this reaction that occurs in plants: 6CO2 + (A) 3O2(g) ←→ 2O3(g) 6H2O → C6H12O6 + 6O2.0 × 10−6 (C) −50 kcal (C) 6. The point of equilibrium (A) Pouring all liquids. II. which of the following state- (A) there will be an excess of 20.) (E) The volume that gas molecules occupy is mini- mal compared to the volume in which the gas is contained.202 × 1024 molecules. (E) None of the above statements is correct. II. 52. A triple beam balance (A) II only (A) A (B) III only (B) B (C) I and III only (C) C (D) II and III only (D) D (E) I. (A) The average kinetic energy of gas molecules is (D) The sample of helium will occupy 44. Which of the following statements is not part of the (C) The sample of hydrogen gas will occupy kinetic molecular theory? 44. and III (E) E GO ON TO THE NEXT PAGE Page 101 of 136 .8 liters and the sample of helium will con- (D) the sulfur will be the limiting factor in the tain 6. Which of the following will not be changed by the 54. when 20. Tongs Figure 2 III. between gas molecules. liquid phases existing at the same time? (See Figure 2. Which pieces of labo- B ratory equipment would be used to help determine A this percentage? I. and III (E) Knowing where the fire extinguisher and eye- wash stations are located 51.7 grams of lead ments is true? (Assume STP. II. A student is performing an experiment where a blue C salt is being heated to dryness in order to determine the percent of water in the salt.02 × 1023 molecules. The diagram shows a solid being heated from below (D) Gas molecules travel in a continuous. E D Temperature 53.2 grams (C) the lead and sulfur will react completely with.PRACTICE TEST 1 207 PRACTICE TEST—Continued 50.02 × 1023 molecules. thermometers. A crucible and cover Time II. Which of the following is considered to be a danger- addition of a catalyst to a reaction at equilibrium? ous procedure in the laboratory setting? I.4 grams of sulfur 55. Which line segment shows the gas and motion. especially acids and bases.8 liters and the sample of helium will con- tain 1.35 grams of lead 22. ∆H over the sink III. 56. The potential energy of the products (B) Wearing goggles (A) I only (C) Pushing glass tubing. (C) Collisions between gas molecules are perfectly elastic.4 liters and the sample of helium will con- tain 3.02 × 1023 molecules.7 grams of lead are reacted with 6. and the sample of hydrogen gas will contain (B) Attractive and repulsive forces are present 6. each in separate containers.) (B) the sulfur will be in excess by 3. (A) The sample of hydrogen gas will occupy out any excess reactants 44. According to the reaction Pb(s) + S(s) → PbS(s). reaction (B) The sample of hydrogen gas will occupy (E) there will be an excess of 10.8 liters proportional to temperature. Given a 4-gram sample of each H2(g) and He(g). or glass (B) II only thistle tubes through a rubber cork (C) I and II only (D) Pointing the mouth of a test tube that is being (D) II and III only heated away from you and others (E) I. random its freezing point. The heat of reaction. When Uranium-238 undergoes one alpha decay and II. II. the resulting isotope is III.0820 L iatm K i mol ) between its molecules. and III 59. ( 0 . Sublimation then one beta decay. (C) Charles / relationship between temperature and III. II.05 atm )( 2. Which of the following situations demonstrate(s) an (E) I. How many moles of electrons are transferred in the (D) NH3 following reaction? Ce3+ + Pb → Ce + Pb4+ (E) H2 (A) 14 (B) 12 (C) 7 (D) 24 (E) 3 GO ON TO THE NEXT PAGE Page 102 of 136 .0 L )( 295K ) while C20H42 has the least.0 liters at (B) CaF2—calcium difluoride 22°C and a pressure of 1. and III increase in entropy? I. Dissolving a salt into water 58. Which of the following statements is/are correct 62. (E) There are more Van der Waals (dispersion) 65. BF3 is trigonal planar in shape. (B) C20H42 has a greater amount of hydrogen bond. (D) (1.0 L ) (D) PCl3—potassium trichloride (A) ( 0.0 L ) ing than CH4 or C8H18. (B) Rutherford / nucleus II. (A) CO—monocarbon monoxide empty soda bottle that has a volume of 2.0820 L iatm K i mol ) ( 22 C ) (E) TiF4—tin(IV) fluoride (B) ( 0. (E) ( 0. Which compound is matched up with its correct name? 64.05 atm ) ( 2. Heating up a liquid (A) Th-234 (A) I only (B) U-234 (B) I and II only (C) Pa-234 (C) II and III only (D) Th-230 (D) I and III only (E) Ra-226 (E) I. Which of the gases listed below would not be collected (C) ∆H(+) and ∆S(+) at a low temperature via water displacement? (D) ∆H(−) and ∆S(−) at a high temperature (A) CO2 (E) ∆G(+) (B) CH4 (C) O2 66. while C8H18 is a liquid and C20H42 is a solid? (C) (1.05 atm )( 2. CH4 is trigonal pyramidal in shape. 0820 L iatm K i mol )( 295K ) (C) There is more dipole-dipole interaction between molecules of greater mass.05 atm )( 2. Of the statements below.0820 L iatm K i mol ) (D) CH4 has the greatest intermolecular forces (1. (A) ∆H(+) and ∆S(−) (B) ∆H(−) and ∆S(+) 61.05 atm )( 2.05 atm? (C) CCl4—carbon tetrachloride (1. pressure (A) I only (D) Curie / radioactivity (B) II only (E) Mendeleyev / periodic table (C) III only (D) I and III only 63.208 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 57. Which set of conditions below guarantees that a reac- forces between nonpolar molecules that are tion will be spontaneous? greater in mass.0 L ) is a gas at STP. which best explains why CH4 (1. XeF6 is tetrahedral in shape.0 L )( 295K ) (A) C20H42 has the greatest ionic interaction ( 0.0820 L iatm K i mol )( 295K ) 60. Which scientist and discovery are not correctly paired? regarding molecular geometries? (A) Millikan / neutron I. How many moles of a gas are present in a closed. (E) Nitrogen dioxide has the highest density and the greatest rate of effusion. Which structure below demonstrates a violation of the octet rule? (See Figure 4. II. Methyl Orange—yellow (A) I only 760 mm Hg (B) II only (C) III only (D) I and III only (E) I. GO BACK AND CHECK YOUR WORK.) (A) H C C H (B) O Gas H C H 80 mm (C) OH O S O OH (D) H N H Figure 3 H (A) 80 mm Hg (E) H C C H (B) 160 mm Hg (C) 680 mm Hg H H (D) 840 mm Hg Figure 4 (E) The pressure cannot be determined. Phenolphthalein—pink sure of the gas? III. Litmus—blue that is 80 mm above its lowest level. 68. (C) Krypton has the lowest density and greatest rate of effusion. color if it were added to a base? est level of mercury inside the tube moved to a level I. A gas is confined in the manometer as shown. II. S T O P IF YOU FINISH BEFORE TIME IS CALLED. Page 103 of 136 . (B) Xenon has the greatest rate of effusion and the lowest density.) The stopcock is then opened and the high. and III 70. (See 69. What is the pres. (D) Ethane has the greatest rate of effusion and the lowest density.PRACTICE TEST 1 209 PRACTICE TEST—Continued 67. Which indicator is correctly paired up with its proper Figure 3. Which statement best describes the density and rate of effusion of the following gases? NO2 C2H6 Kr Xe F2 (A) Fluorine has the lowest density and the lowest rate of effusion. ® Practice Test 2 SAT II Chemistry McGraw-Hill’s Page 104 of 136 . For each numbered item. Phase A → Phase B 2. for all statements involving chemical equations and/or solutions. Each choice in a set may be used once. Then fill in the corresponding oval on the answer sheet. Phase A → Phase C 4.PRACTICE TEST 2 221 PRACTICE TEST 2 Time: 60 minutes Note: Unless otherwise stated. Questions 1–4 (A) Sublimation (B) Deposition (C) Vaporization (D) Condensation (E) Melting A B Pressure C Temperature Figure 1 1. Part A Directions: Each of the following sets of lettered choices refers to the numbered formulas or statements immediately below it. Phase C → Phase A 3. assume that the system is in pure water. choose the one lettered choice that fits it best. more than once. Phase B → Phase C GO ON TO THE NEXT PAGE Page 105 of 136 . or not at all. Ptotal = P1 + P2 + P3 + . 1 molecule of CH4 21. 9. PV = nRT 11. Aldehyde functional group Questions 19–22 Questions 9–11 (A) Boyle’s Law (B) Charles’ Law (A) 6. Forms ions with a 2+ charge 25. 88 grams of CO2(g) at STP 20.2 liters (D) Combined Gas Law (C) 58. Reacts most vigorously with water (E) 11H 13. Phenolphthalein in acid 8. Can be neutralized with a base 16.02 × 1023 molecules (C) Ideal Gas Equation (B) 11.0 moles Pressures (E) 5 atoms 19. Could be named 2-pentanone 17. P1V1 = P2V2 10.222 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued Questions 5–8 Questions 16 –18 (A) R—COOH (A) Blue (B) R—CHO (B) Red (C) R—CO—R (C) Pink/purple (D) R—COO—R (D) Colorless (E) R—CO—NH2 (E) Orange 5. Phenolphthalein in base 6. Has the greatest mass GO ON TO THE NEXT PAGE Page 106 of 136 . 32 grams of SO2 gas at STP P1V1 PV 22. . Is chemically inert 23. Litmus in acid 7. = 2 2 T1 T2 Questions 12–15 (A) Alkali metal Questions 23–25 (B) Alkaline earth metal (A) 4 He (C) Transition metal 2 (B) 0 e (D) Halogen 1− (E) Noble gas (C) γ (D) 10n 12. Has a charge of 2+ 14. Has the highest first ionization energy in its period 24. Has the lowest mass 15. Amide functional group 18. .5 grams/mole (E) Dalton’s Law of Partial (D) 2. point than that of 1m CaCl2(aq) 104. 1m NaCl(aq) will have a higher boiling BECAUSE 1 mole of NaCl yields 3 moles of ions in solution. Fill in the corresponding T or F ovals on the answer sheet provided. Powdered zinc reacts faster with acid BECAUSE powdered zinc has a greater surface area. NH3 can best be collected by water BECAUSE NH3 is a polar substance. SAMPLE: EX 1. than a larger piece of zinc 107. HCl is considered to be an acid BECAUSE HCl is a proton acceptor. Part B Directions: Each question below consists of two statements. Neutrons and protons are classified as BECAUSE neutrons and protons are both located in the princi- nucleons pal energy levels of the atom. 102. The element with an electron BECAUSE the element with an electron configuration of configuration of [He]2s1 has a larger [He]2s1 has a greater nuclear charge than fluorine. The double and single bonds in benzene BECAUSE benzene has delocalized pi electrons that stabilize are subject to resonance its structure. displacement GO ON TO THE NEXT PAGE Page 107 of 136 .PRACTICE TEST 2 223 PRACTICE TEST—Continued PLEASE GO TO THE SPECIAL SECTION AT THE LOWER LEFT-HAND CORNER OF YOUR ANSWER SHEET LABELED “CHEMISTRY” AND ANSWER QUESTIONS 101–115 ACCORDING TO THE FOLLOWING DIRECTIONS. determine whether statement I in the left- most column is true or false and whether statement II in the rightmost column is true or false. The nucleus of an atom has a BECAUSE the only positive particles positive charge found in the atom’s nucleus are protons. 105. Fill in the oval labeled “CE” only if statement II correctly explains statement I. SAMPLE ANSWER I II CE* EX 1 F F I II 101. 106. atomic radius than fluorine 103. For each question. 110. 115. 112. GO ON TO THE NEXT PAGE Page 108 of 136 . An exothermic reaction has a negative BECAUSE in an exothermic reaction the products have less value for ∆H potential energy than the reactants. AgCl is insoluble in water BECAUSE all chlorides are soluble in water except for those of silver. CH3CH2—OH and CH3—O—CH3 BECAUSE CH3CH2—OH and CH3—O—CH3 have the same are isomers molecular formula but different structures. the BECAUSE pressure and volume have a direct relationship. and lead. volume of the gas decreases 111. 113. The addition of H2 to ethene will form an BECAUSE ethane has as many hydrogen atoms bonded to the unsaturated compound called ethane carbon atoms as possible. mercury. 109. 114.224 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 108. As pressure on a gas increases. pure water can boil at a BECAUSE water boils when the vapor pressure of the water is temperature less than 273 K equal to the atmospheric pressure. Pure water has a pH of 7 BECAUSE the number of H1+ ions is equal to the number OH1− ions. ∆S will be positive in value as BECAUSE vaporization increases the order of the molecules vaporization occurs entering the gas phase. At 1 atm. What is the empir- lowest freezing point? ical formula of this compound? (A) NaC2H3O2 (A) C2H4 (B) NaCl (B) CH4 (C) MgCl2 (C) CH3 (D) CH3OH (D) CH2 (E) C6H12O6 (E) CH 27. II. Cl2 + 2NaBr → Br2 + 2NaCl try? II. which one would require you to read a meniscus? 28. and III 31. 2K + 2H2O → H2 + 2KOH (B) CH4 (A) I only (C) CO2 (B) II only (D) H2S (C) III only (E) C2H2 (D) I and III only (E) I. Which of these equations is/are properly balanced? 30. A compound was analyzed and found to be composed solved in 1.0 (C) 8. Which compound below has a bent molecular geome- I. Select the one answer that is best in each case and then fill in the corresponding oval on the answer sheet provided. 26.0 moles of C3H8(g)? (D) 50 mL buret (A) 144. Which of these would (E) 22. One mole of each of the following substances is dis. Of the equipment listed below.8 + SCN−(aq) ←→ FeSCN2+(aq).0 kg of water. How many (B) 500 mL flask grams of water can be produced from the complete (C) Watch glass combustion of 2.0 (E) Trough (B) 82.4 shift the equilibrium to the left? (A) Adding FeCl3 to the reaction (B) Adding NH4SCN to the reaction (C) Increasing the pressure on the reaction (D) Adding a catalyst (E) Adding FeSCN2+(aq) to the reaction GO ON TO THE NEXT PAGE Page 109 of 136 .PRACTICE TEST 2 225 PRACTICE TEST—Continued Part C Directions: Each of the multiple-choice questions or incomplete sentences below is followed by five answers or com- pletions. Given the following reaction at equilibrium: Fe3+(aq) (D) 44. 29. Which solution will have the of 75% carbon and 25% hydrogen. 2Na + O2 → Na2O (A) H2SO4 III. Propane and oxygen react according to the equation: (A) 100 mL beaker C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g).0 32. water to make 1 liter of solution. (B) The percent by mass of oxygen is 45%.6 × 10−10 (D) 132 grams (B) 1. The Ksp value for AgCl (B) 64 grams will be (C) 28 grams (A) 2.5 moles according to the reaction: C(s) + O2(g) → CO2(g). The concentration of Ag1+ (A) 36 grams ions is found to be 1. which holds true for the ele- ments found in Na2HPO4? 36. of 36 grams of carbon with 64 grams of oxygen gas? duce a saturated solution. when added to enough (A) The total molar mass is 71 grams/mole. (D) D (B) All atoms of an element are identical.3 × 10−10 (E) 88 grams (C) 1.8 × 10−5 (E) 1. How much carbon dioxide can be formed from the reaction 37. Which unit is paired incorrectly? (B) H2O(l) (A) Torr and pressure (C) Ar(g) (B) Mass and grams (D) NaCl(aq) (C) Heat energy and kiloPascals (E) CH4(g) (D) Volume and milliliter (E) Temperature and Kelvin 40. Which amount of Pb(NO3)2. Which letter in the boxes below has a value of 7? Number of Number of Number of Mass Atomic Isotope Protons Neutrons Electrons Number Number 16 O A 13 C B E 23 Na C 10 B D (A) A 38. (E) E (C) The atoms of different elements have different chemical and physical properties. Carbon and oxygen react to form carbon dioxide (E) 0. Of the statements below.0 M? (C) The percent by mass of sodium is 16%. Each of the elements below is placed in water. geometric pattern? (A) NaC2H3O2(s) 35. Which statement below is inconsistent with the con- (B) B cept of isotopes? (C) C (A) Each element is composed of atoms.003 moles 41.3 × 10−5 (D) 1. Enough AgCl(s) is dissolved in water at 298 K to pro. (C) Cu (D) Au 39. tion with a molarity of 1. (A) 144 grams (D) The percent by mass of phosphorus is 44%. (A) Na (E) In a compound. will produce a solu. Which sample below has its atoms arranged in a reg- (E) Ne ular.3 × 10−5M. the kinds and numbers of atoms (B) Fe are constant. Which (D) The combining of elements leads to the forma- one will react violently with the water? tion of compounds.226 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 33. 34. (B) 331 grams (E) The percent by mass of hydrogen is 13%. (C) 317 grams (D) 0.8 × 10−10 GO ON TO THE NEXT PAGE Page 110 of 136 . Which of the following processes will decrease the (E) H in Na2HPO4 rate of a chemical reaction? I. Which electron configuration shows that of an excited electricity? atom? (A) KBr(l) (A) 1s22s22p63s1 (B) NaC2H3O2(s) (B) 1s22s22p63s23p63d1 (C) C6H12O6(aq) (C) 1s22s22p4 (D) CH3OH(aq) (D) 1s22s22p63s23p64s2 (E) NaCl(s) (E) 1s22s22p63s23p3 45. (B) I and II only (E) Reduction will occur at the cathode. What is the value for ∆H for the reaction: D + A + reaction 2NO(g) + Cl2(g) ←→ 2NOCl(g)? B → F? [ NO ][ Cl 2 ] (A + B → C ∆H = −390 kJ) (A) [ NOCl ] (D + 1⁄2B → E ∆H = −280 kJ) (F + 1⁄2B → C + E ∆H = −275 kcal) [ NOCl ] (B) [ NO ][ Cl 2 ] (A) −165 kJ (B) +385 kJ [ NO ]2 [ Cl 2 ] (C) −395 kJ (C) [ NOCl ]2 (D) −945 kJ (E) +400 kJ (D) [ NOCl ]2 [ NO ]2 [ Cl 2 ] 47. Of the substances below. A voltaic cell is set up and a chemical reaction pro. Decreasing the temperature by 25 K of bonding found between the atoms of that sub- III. Given the chemical reaction 3H2(g) + N2(g) ←→ ceeds spontaneously. and III (E) Cl2—polar covalent bonds 44. 50.PRACTICE TEST 2 227 PRACTICE TEST—Continued 42. I. the forward reaction can best be occur in this reaction? described as a(n) (A) The electrons will migrate through the wire. (A) II only (D) The anode will lose mass. which is best able to conduct 49. II. III. Stirring the reactants stance? (A) I only (A) CH4—covalent bonds (B) II only (B) CaO—ionic bonds (C) I and III only (C) Fe—metallic bonds (D) II and III only (D) H3O1+—coordinate covalent bonds (E) I. and III GO ON TO THE NEXT PAGE Page 111 of 136 . II. Which of the following will not 2NH3(g) + energy. Phase equilibrium anode half cell. Exothermic reaction (C) The cathode will gain mass. Using highly concentrated reactants 48. What is the correct mass-action expression for the 46. The oxidation state of the elements in the choices below will be 1− except for [ NOCl ]2 (A) F in HF (E) [ NO ]2 + [ Cl 2 ] (B) Cl in NaCl (C) O in H2O2 (D) F in NaF 43. (C) I and III only (D) II and III only (E) I. Which substance is not correctly paired with the type II. Synthesis reaction (B) The cations in the salt bridge will migrate to the II. (E) A conjugate pair will differ by an H1+ ion. If the initial reading of the (C) Na meniscus of the acid’s burette is 3.00 (E) I. s to p gas to that of helium gas? III.52°C (C) HCl (C) −3. A titration is set up so that 40. and III 53. Which of the following best describes the orbital over- gates and conjugate pairs? lap in a molecule of (A) HF and F1− are conjugate pairs.86°C (E) H2 (E) 3.86°C (B) HBr (B) −0.0 M HCl. Which of the following is not true regarding conju.72°C 54.50 (D) II and III only (E) 1. (B) NaC2H3O2 and C2H3O21− are conjugate pairs. H H (D) NH41+ is the conjugate acid of NH3. 56.15 mL (B) F2—Van der Waals (dispersion) forces (C) HCl—dipoles (D) CH4—dipoles (E) NaCl(aq)—molecule-ion attraction GO ON TO THE NEXT PAGE Page 112 of 136 .15 mL what will the (D) Li final burette reading be? (E) F2 (A) 20.00 (B) II only (C) 4. Which metal will not generate hydrogen gas when kcal. What will be the change in the freezing point of the ing between the molecules of the substance? water in a solution of 1 m NaCl(aq)? (A) CH4 (A) −1.41 (A) I only (B) 2. H C C H? (C) CO32− is the conjugate base of HCO31−.15 mL ing found between the molecules of that substance? (D) 23. Given the reaction: N2(g) +3H2(g) ←→ 2NH3(g) + 22 58. II. Which substance is the best oxidizing agent? (A) Fe 55. 57. what is the value for ∆H for the reverse reaction placed in HCl(aq)? when 6 moles of NH3 are consumed to produce nitro- (A) Au gen gas and hydrogen gas? (B) Mg (A) +22 kcal (C) Ca (B) +66 kcal (D) Sr (C) −22 kcal (E) Zn (D) −66 kcal (E) +33 kcal 59. Figure 2 I.00 mL (B) 40.00 (C) I and III only (D) 0.15 mL (A) NH3—hydrogen bonding (E) 13. Which substance is not correctly paired with the bond- (C) 43. sp2 to sp2 (A) 1. What is the ratio of the rate of effusion of hydrogen II.0 M NaOH are (B) O2 titrated with 2.228 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 51.00 mL 60.0 mL of 1. Which substance below will exhibit hydrogen bond.72°C (D) H2O (D) 1. s to s 52. In 6. The modern periodic table is based upon 69.0-gram sample of 112Ag decays to cules. (B) There are no forces present between gas mole- 63. Wear goggles (D) HC2H3O2(aq) III. Which of the following would you not do in a labora- (A) NaCl(aq) tory setting? (B) C6H12O6(aq) I. 65.5 grams. (E) A pH of 10 is 100 times as basic. II. Which solution is not expected to conduct electricity? 67. ing the kinetic molecular theory? (D) All nitrates are insoluble in water.20 hours motion. 64. and III temperature. Which of the following statements about solubility is (C) III only correct? (D) I and III only (A) Gases decrease in solubility with an increase in (E) I. What is the pH of a 0. What is the half-life of 112Ag? (C) Collisions between gas molecules are perfectly (A) 1. How many times more basic is a solution with a pH of (A) atomic mass of the elements 10 than a solution with a pH of 8? (B) number of neutrons in the nucleus (A) A pH of 10 is two times as basic. random (C) 6. (B) 3.60 hours elastic. Which of the following reactions is not labeled cor- (B) one thousandth rectly? (C) one hundred (A) Fe + Cr3+ → Fe3+ + Cr (redox reaction) (D) one hundredth (B) KBr + H2O → HBr + KOH (hydrolysis) (E) one millionth (C) CH4 + 2O2 → CO2 + 2H2O (combustion) (D) CH4 + Cl2 → CH3Cl + HCl (addition) 66. (D) 12. Which of the following statements is not true regard- (C) PbI2 is soluble in water. 68. (B) NaCl is insoluble in water. Page 113 of 136 . Heat a stoppered test tube (E) NaOH(aq) (A) I only (B) II only 62. (D) oxidation states (C) A pH of 10 is 2.6 hours inversely proportional to temperature. (E) number of protons in the nucleus (D) A pH of 8 is 20 times as basic.means (A) one thousand 70. (C) number of isotopes of an element (B) A pH of 8 is two times as basic.4 hours (E) The average kinetic energy of gas molecules is (E) 18.20 hours. a 50. The prefix centi. (A) The volume that gas molecules occupy is negli- (E) Solubility depends solely upon the amount of gible compared to the volume within which the solvent used. 12.PRACTICE TEST 2 229 PRACTICE TEST—Continued 61. gas is contained.1 M acid solution where the acid (E) CO2 + H2O → H2CO3 (synthesis) has a Ka of 1 × 10−5? (A) 3 (B) 5 (C) 6 (D) 4 (E) 1 S T O P IF YOU FINISH BEFORE TIME IS CALLED.000 times as basic. GO BACK AND CHECK YOUR WORK. Pour acids and bases over a sink (C) KBr(aq) II.10 hours (D) Gas molecules travel in a continuous. ® Practice Test 3 SAT II Chemistry McGraw-Hill’s Page 114 of 136 . assume that the system is in pure water. or not at all. Then fill in the corresponding oval on the answer sheet. Demonstrates the relationship between pressure (x-axis) and volume (y-axis) in Boyle’s Law 2. Each choice in a set may be used once. choose the one lettered choice that fits it best. more than once. Shows the relationship between atomic number (x-axis) and atomic radius (y-axis) for the elements in period 2 GO ON TO THE NEXT PAGE Page 115 of 136 . Demonstrates the relationship between temperature (x-axis) and volume (y-axis) in Charles’ Law 4.PRACTICE TEST 3 241 PRACTICE TEST 3 Time: 60 minutes Note: Unless otherwise stated. Part A Directions: Each of the following sets of lettered choices refers to the numbered formulas or statements immediately below it. Questions 1–4 (A) (B) (C) (D) (E) Figure 1 1. Contains a triple point 3. for all statements involving chemical equations and/or solutions. For each numbered item. The electron configuration for potassium in the ground 25. Will form an ion with a 3–charge Questions 12–15 Questions 23–25 (A) 1s22s22p63s23p6 (A) milli- (B) 1s22s22p63s23p64s2 (B) kilo- (C) 1s22s22p63s23p64s1 (C) centi (D) 1s2 (D) micro- 2 2 6 1 (E) 1s 2s 2p 3p (E) nano- 12. The electron configuration for an excited atom 24. These two compounds have coordinate covalent bonds.242 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued Questions 5–8 Questions 16 –19 (A) Br2 and Hg (A) Sublimation (B) Cl2 and F2 (B) Deposition 1+ 1+ (C) NH4 and H3O (C) Vaporization (D) Fe and Co (D) Condensation (E) Diamond and graphite (E) Freezing 5. 10−9 13. The electron configuration for the noble gas with the highest first ionization energy GO ON TO THE NEXT PAGE Page 116 of 136 . Ends in -amine 21. Solid to gas 6. 10−6 14. Liquid to gas 8. Ends in -ol 22. Has 2 valence electrons 10. These two compounds are in the liquid phase at 293 K. Liquid to solid Questions 9–11 Questions 20 –22 (A) R—OH (A) Nitrogen (B) R—O—R (B) Oxygen (C) R—NH2 (C) Chlorine (D) R—COO—R (D) Neon (E) R—CO—R (E) Beryllium 9. Has 6 valence electrons 11. These two compounds are good oxidizing agents. 18. The electron configuration for calcium ion 23. These two compounds are allotropes of each other. Gas to solid 7. 103 state 15. Ends in -oate 20. 16. 19. 17. thin sheet of gold foil 102. decreases 107. According to the equation M1V1 = M2V2. SAMPLE ANSWER I II CE* EX 1 F F I II 101. Part B Directions: Each question below consists of two statements. 103. Fill in the oval labeled “CE” only if statement II correctly explains statement I. The nucleus of an atom has a BECAUSE the only positive particles positive charge found in the atom’s nucleus are protons. SAMPLE: EX 1. CCl4 is a polar molecule BECAUSE the dipole arrows for CCl4 show counterbalance and symmetry. 106. Fill in the corresponding T or F ovals on the answer sheet provided. 105.PRACTICE TEST 3 243 PRACTICE TEST—Continued PLEASE GO TO THE SPECIAL SECTION AT THE LOWER LEFT-HAND CORNER OF YOUR ANSWER SHEET LABELED “CHEMISTRY” AND ANSWER QUESTIONS 101–115 ACCORDING TO THE FOLLOWING DIRECTIONS. GO ON TO THE NEXT PAGE Page 117 of 136 . A molecule of ethyne is linear BECAUSE the carbon atoms in ethyne are sp hybridized. Alpha particles are able to pass through a BECAUSE the atom is mainly empty space. 104. determine whether statement I in the left- most column is true or false and whether statement II in the rightmost column is true or false. KNO3 will not dissolve in water BECAUSE all chlorides are soluble in water. BECAUSE as water is added to a solution the solution is as the volume increases the molarity diluted. HCl is an Arrhenius acid BECAUSE HCl will yield hydronium ions as the only positive ions in solution. Nitrogen has five valence electrons BECAUSE the electron configuration for nitrogen is 1s22s22p6. For each question. 114. The number 5. A 1m NaCl(aq) solution will freeze at a BECAUSE as a solute is added to a solvent. 115. alpha particle 111.244 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 108. 110. GO ON TO THE NEXT PAGE Page 118 of 136 . and food preservation. figures 113. DNA is a polymer BECAUSE DNA has many smaller units bonded to create longer chains. 4 2He is the correct symbol for an BECAUSE an alpha particle is a helium-3 nucleus. Radiation and radioisotopes can have BECAUSE radioisotopes and radiation can be used for radio beneficial uses dating. Adding more reactants will speed up a BECAUSE the reactants will collide less frequently. radiotracers. electronegativity 112. reaction 109. Fluorine has the highest value for BECAUSE fluorine has the greatest attraction for electrons.007 has three significant BECAUSE zeros between non-zero digits are significant. the boiling point temperature below 273 K increases while the freezing point decreases. Al3+ + 3e– → Al is a correctly balanced BECAUSE Al3+ + 3e– → Al correctly demonstrates conserva- oxidation reaction tion of mass and conservation of charge. Which of the following is not part of the Atomic Theory? 32.0 liters of with a molecular geometry that is described as trigo- solution nal planar with respect to other atoms present? (B) 360 grams of C6H12O6 dissolved to make I. Which of the following compounds will have an atom (A) 73 grams of HCl dissolved to make 2.029 J (D) the vapor pressure is reduced (E) the surrounding pressure is increased 28. Cyclopropane of solution (A) I only (D) 24 grams of LiOH dissolved to make 1. Which of the following transmutations demonstrate(s) hydrogen chloride.5 liters of solution II. 26. (E) HCl(aq) (E) The atom is mainly empty space.) II. CH2=CH2 (C) 94 grams of K2O dissolved to make 0.0 M? 29. When chlorine gas and hydrogen gas react to form 30. Pb-212 → Bi-212 (A) +245 kJ/mol III.PRACTICE TEST 3 245 PRACTICE TEST—Continued Part C Directions: Each of the multiple-choice questions or incomplete sentences below is followed by five answers or comple- tions. Select the one answer that is best in each case and then fill in the corresponding oval on the answer sheet pro- vided. BF3 1. (A) KCl(l) (B) All atoms of a given element are alike.75 liters III. Which sample has atoms that are arranged in a regular (A) Compounds are made up of combinations of geometric pattern? atoms. II. (B) NaC2H3O2(s) (C) All matter is composed of atoms. Which aqueous solution has a molarity of 1. and III 27. what will be the change of enthalpy beta decay? of the reaction? (Bond dissociation energies can be I. A liquid will boil when (A) 5.270 J (A) the liquid is hot (B) 355 J (B) a salt has been added to the liquid (C) 259 J (C) the vapor pressure of the liquid is equal to the (D) 151 J surrounding pressure (E) 22. II. Ra-228 → Ac-228 (B) +185 kJ/mol (A) I only (C) −185 kJ/mol (B) II only (D) −1105 kJ/mol (C) II and III only (E) +1105 kJ/mol (D) I and II only (E) I.25 liters (B) II only of solution (C) III only (E) 40 grams of HF dissolved to make 2. 33.50 liters of (D) I and II only solution (E) I. (C) Fe(l) (D) A chemical reaction involves the rearrangement (D) NaCl(aq) of atoms. and III GO ON TO THE NEXT PAGE Page 119 of 136 . Bi-212 → Po-212 found in Appendix 4 at the back of the book. How much heat is required to raise the temperature of 85 grams of water from 280 K to 342 K? 31. Sodium and chlorine react according to the following reaction: 2Na + Cl2 → 2NaCl. II.5 moles of NaCl 38.4 L of H2(g) at STP (D) Na is the limiting reagent and 2. (E) 207 grams of Pb GO ON TO THE NEXT PAGE Page 120 of 136 . (B) Na is the excess reagent and 2. If the reaction starts (A) MnO41− → Mn2+ + 4H2O with 5. II. 39.0 moles of Na and 3.7% (E) HClO4(aq) (C) 27. Hydronium ion concentration is greater than rusting of 446 grams of Fe according to the reaction: hydroxide ion concentration. The percent composition by mass of oxygen in BaSO4 (B) HF(aq) is (C) NaOH(aq) (A) 233. The quantity “one mole” will not be equal to will be produced. Of the following solutions. 4Fe + 3O2 → 2Fe2O3? (Assume an unlimited amount of oxygen gas. (D) AgNO3(aq) + KCl(aq) → (D) Ionic compounds are written as empirical for- (E) KBr(aq) + H2O(aq) → mulas.0 moles of NaCl (E) 2F1− + 2e− → F2 will be produced. (C) 64 grams of SO2(g) (E) Cl is the excess reagent and 2. (C) There will be an excess of 2. Which of the following half reactions is correctly bal- anced? 42. Litmus paper turns blue.0 moles of (B) 6.246 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 34. Which statement below is false regarding empirical ble precipitate? formulas? (A) HCl(aq) + KOH(aq) → (A) The empirical formula for butyne is C2H3.7% I. Which of the following indicate(s) a basic solution? (E) 13. Phenolphthalein turns pink. 41. (C) NaCl(aq) + CaCl2(aq) → (C) The empirical formula of CH2O is C6H12O6.0 moles of Cl2 then which (B) Cu + 2Ag1+ → 2Ag + Cu2+ statement below is true? (C) H2 + OH1− → 2H2O (D) Pb2+ + 2e− → Pb (A) Cl2 is the excess reagent and 5.) (A) I only (B) II only (A) 320 grams (C) III only (B) 223 grams (D) I and II only (C) 159 grams (E) I. be the weakest electrolyte? (A) HCl(aq) 40. (A) 22.0 moles of Na. Which double replacement reaction forms an insolu.7% 36. (E) The empirical and molecular formulas for 35.02 × 1023 carbon atoms NaCl will be produced.0 moles of NaCl (D) 36 grams of H2O will be produced. (B) KNO3(aq) + Na2SO4(aq) → (B) The empirical formula for ammonia is NH3. How many grams of Fe2O3 can be formed from the III.4% (D) 58.4% (D) KI(aq) (B) 66. which one is expected to methane are the same. and III (D) 480 grams (E) 640 grams 37. If the pressure on a gas is doubled. Given the reaction: 3H2(g) + N2(g) ←→ 2NH3(g) + (E) Carbon dioxide can be tested for with a lit heat energy. equilibrium in the direction opposite to that of the other four choices? 49. Which of the following demonstrate(s) ∆S(−)? I. Raking up leaves II. C D Potential Energy 45. (E) K eq = [ C][ D ] (C) Ammonia can be collected by water displace- [ A ][ B] ment. Which of the following statements about gas collec- [ D ]2 tion is false? (C) K eq = [ A ]2 [ B] (A) Carbon dioxide can be collected by an upward displacement of air. Boiling a liquid A B III. (E) Add hydrogen gas. which letter represents (A) Remove ammonia from the reaction. In which of the following pieces of glassware does a (B) D meniscus become of importance? (C) A (A) Watchglass (D) E (B) Burette (E) C (C) Beaker (D) Flask (E) Funnel GO ON TO THE NEXT PAGE Page 121 of 136 . Emptying a box of confetti onto the floor (A) I only (B) II only E (C) I and II only Time (D) I and III only (E) II and III only Figure 2 (A) B 46. tial energy of the reactants? (See Figure 2. (D) Add nitrogen gas. [ A ]2 [ B] (B) Ammonia can be tested for by placing red lit- (D) K eq = [ D ]2 mus paper at the mouth of the collection glass- ware. the volume of the 2A(g) + B(g) ←→ 3C(s) + 2D(g) is written as gas will be (A) doubled (A) K eq = [ A ] [ B] 2 (B) the same [ C ]3 [ D ]2 (C) halved (D) quartered [ C ]3 [ D ]2 (E) quadrupled (B) K eq = [ A ]2 [ B]2 48. Which of the following would drive the match. 44. (D) Hydrogen gas can be collected by water dis- placement. In the diagram shown below. The equilibrium constant expression for the reaction: 47.PRACTICE TEST 3 247 PRACTICE TEST—Continued 43. the potential energy of the products minus the poten- (B) Increase the temperature of the system.) (C) Increase the pressure on the system. (A) ( 2. (C) K(s) → K1+ + 1e– (E) Isotopes differ in their nuclear charge.3 moles )( 0. (D) Br2 → 2Br1− + 2e– (E) Br2 + 2e– → 2Br1− 57.248 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 50.1 atmospheres? increase in sulfate ions.3 moles )(1.14 V (C) ( 2. (A) Isotopes have the same number of protons. Which of the following pairs of substances can be broken down chemically? 52.0 mL of 1.00 mL (A) −1475 kcal (C) 23.00 mL (D) +325 kcal (E) +300 kcal 56. Which will not happen when sodium sulfate is added (A) Ammonia and iron to a saturated solution of PbSO4 that is at equilibrium? (B) Helium and argon [PbSO4(s) ←→ Pb2+(aq) + SO42−(aq)] (C) Methane and water (A) The solubility of the lead sulfate will decrease. (D) The Ksp value will change.5 M HCl. (B) 2Br1− → Br2 + 2e– (D) Isotopes differ in number of neutrons present.1 atm ) (A) H2 (E) ( 2. Which of the following molecules has polar bonds but is a nonpolar molecule? ( 2.0820 Liatm moliK ) (300 K ) (C) +1.3 moles )( 0. (A) K1+ + 1e– → K(s) (C) Isotopes differ in mass number.07 V (D) +1.3 moles ) (1.0820 Liatm moliK )(300 K ) 53.10 V ( 2. trolysis.00 mL (B) 35.1 atm ) (B) −1. 58.07 V (300 K ) (1. Which reaction occurs at the anode? (B) Isotopes have the same atomic number.1 atm ) (D) (300 K )( 0. What is the heat of reaction for A + B → F? 55.0 M? (A) +1.1 atm ) Zn2+ at 298 K if [Zn2+] = 0. A titration is set up so that 35. (D) Potassium and lithium (B) The concentration of lead ions will decrease.1 atm )(300 K ) (B) H2O ( 0.3 moles of an ideal gas at (E) The equilibrium will shift to consume the 300 K and a pressure of 1.0820 Liatm moliK ) 54. What is the volume of 2.0820 Liatm moliK K) (C) NH3 (D) NaCl (E) CO2 GO ON TO THE NEXT PAGE Page 122 of 136 .0820 Liatm moliK ) (E) −1.2 M and [Cu2+] = 4.10 V (B) (1.33 mL (C) −1025 kcal (E) 20.33 mL (B) +25 kcal (D) 58. (E) Water and carbon (C) The reaction will shift to the left. What is the voltage of the voltaic cell Cu / Cu2+ // Zn / (1.0 M NaOH are titrated with 1. How many milliliters of acid (A + B → 2C ∆H = +150 kcal) are needed to completely titrate this amount of base? (C → 2D + 2E ∆H = −450 kcal) (F → 4D + 4E ∆H = +725 kcal) (A) 15.3 moles )( 0. Which statement is inconsistent with the concept of isotopes of the same element? 51. Molten KBr is allowed to undergo the process of elec. PRACTICE TEST 3 249 PRACTICE TEST—Continued 59. Substance X has three common isotopes: X-48, X-49, 63. As you go from left to right across a period on the and X-51. If the relative abundances of these isotopes periodic table there in a decrease in are 42%, 38%, and 20%, respectively, what is the (A) first ionization energy atomic mass of substance X? (B) nuclear charge (A) 49.33 (C) electronegativity (B) 48.62 (D) the ability to gain electrons (C) 50.67 (E) metallic character (D) 48.98 (E) 49.67 64. Which of the following statements is false? (A) H2 has just one sigma bond. 60. Which choice below would affect the rate of reaction (B) HCl has just one sigma bond. in the opposite way from the other four? (C) H—C≡≡C—H has four pi bonds and three (A) Cool the reaction down. sigma bonds. (B) Add a catalyst. (D) CH2==CH2 has five sigma bonds and one pi (C) Decrease the pressure. bond. (D) Use larger pieces of solid reactants. (E) H2O has two sigma bonds and two lone pairs. (E) Decrease the concentration of the reactants. 65. What is the correct formula for iron(III) sulfate? 61. One mole of an ideal gas at STP has its temperature (A) FeSO4 changed to 15°C and its pressure changed to 700 torr. (B) Fe2(SO4)3 What is the new volume of this gas? (C) Fe(SO4)3 (D) Fe3SO4 (A) ( 760 torr )( 22.4 L )( 288 K ) (E) Fe3(SO4)2 ( 273 K )( 700 torr ) (B) ( 273 K )( 700 torr ) 66. A solution has a pH of 6.0. What is the concentration of OH1− ions in solution? ( 760 torr )( 22.4 L )( 288 K ) (A) 6.0 × 10−14 M (C) ( 760 torr )( 22.4 L )( 273 K ) (B) 1.0 × 10−6 M (C) 1.0 × 10−14 M ( 288 K )( 700 torr ) (D) 6.0 × 10−8 M (D) ( 700 torr )( 22.4 L )( 287 K ) (E) 1.0 × 10−8 M ( 273 K )( 760 torr ) 67. Which of the following statements about bonding is (E) ( 760 torr )(1.0 L )( 288 K ) correct? ( 273 K )( 700 torr ) (A) Van der Waals forces exist between polar mole- cules. 62. Which reaction will not occur spontaneously? (B) Dipoles are the result of the equal sharing of electrons. (A) Au3+ + 3e– → Au (C) Cu(s) is a network solid. (B) Mg + 2H1+ → Mg2+ + H2 (D) Hydrogen bonds exist between the molecules of (C) F2 + 2e– → 2F1− HCl. (D) Li1+ + 1e– → Li (E) NaCl(aq) has attraction between the molecules (E) 2Na + Cl2 + 2e– → 2NaCl and the ions. GO ON TO THE NEXT PAGE Page 123 of 136 250 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 68. A radioactive substance decays from 100 grams to 70. Which statement below is incorrect regarding bal- 6.25 grams in 100 days. What is the half-life of this anced equations? radioactive substance? (A) C + O2 → CO2 is balanced and is a synthesis (A) 25 days reaction. (B) 6.25 days (B) CaCO3 → CaO + CO2 is balanced and is a (C) 12.5 days decomposition reaction. (D) 100 days (C) Na + Cl2 → NaCl is not balanced but demon- (E) 50 days strates a synthesis reaction. (D) KI + Pb(NO3)2 → PbI2 + KNO3 is balanced and 69. Which choice or choices demonstrate amphoterism? is a single replacement reaction. I. HCl + H2O → H3O1+ + Cl1− and (E) 2H2O → 2H2 + O2 is balanced and demonstrates H2O + NH3 → OH1− + NH41+ a redox reaction. II. HS1− + HCl → Cl1− + H2S and HS1− + NH3 → NH41+ + S2− III. HCl + NaOH → NaCl + H2O and NaCl + H2O → HCl + NaOH (A) I only (B) II only (C) III only (D) I and II only (E) I and III only S T O P IF YOU FINISH BEFORE TIME IS CALLED, GO BACK AND CHECK YOUR WORK. Page 124 of 136 ® Practice Test 4 SAT II Chemistry McGraw-Hill’s Page 125 of 136 Part A Directions: Each of the following sets of lettered choices refers to the numbered formulas or statements immediately below it. Questions 1–4 (A) The point of equilibrium (B) The triple point (C) The freezing point (D) The point where reactants first form products (E) The boiling point 1. and gas phases exist simultaneously 2. choose the one lettered choice that fits it best. The activated complex GO ON TO THE NEXT PAGE Page 126 of 136 . liquid. assume that the system is in pure water. more than once. Then fill in the corresponding oval on the answer sheet. or not at all. Vapor pressure of a liquid is equal to the pressure of the surround- ings 4. for all statements involving chemical equations and/or solutions. Each choice in a set may be used once. For each numbered item.PRACTICE TEST 4 263 PRACTICE TEST 4 Time: 60 minutes Note: Unless otherwise stated. A specific temperature and pressure where solid. Can be shifted by adding more reactants 3. Ne-19 → F-19 + X 14. Chlorine gas 17. Dispersion forces 11. Po-218 → At-218 + X 12. Hydrogen bonding spontaneous 21. 96. Contain elements in the solid.03 × 1023 molecules (B) Purple (B) 44. 0. Valence electrons are located in the f orbitals 24. Detects radioactive particles Questions 23–25 Questions 12–15 (A) Alpha particle (A) Halogens (B) Beta particle (B) Alkali metals (C) Gamma particle (C) Alkaline earth metals (D) Positron (D) Noble gases (E) Deuteron (E) Lanthanides 23.8 liters (C) Orange (C) 3. KMnO4 solution 18. Copper(II) sulfate solution 16.25 moles of O2 at STP 6.01 × 1023 atoms 5. 56 grams of N2 at STP 8. Dipoles 10. Tc-99 → Tc-99 + X 13. Requires an external current to make a redox reaction 20. Need to lose one electron to form a stable octet 25. liquid. Requires a salt bridge 22.0 grams (E) Blue (E) 3. and gas phases at STP GO ON TO THE NEXT PAGE Page 127 of 136 .264 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued Questions 5–8 Questions 16–19 (A) Red (A) 9. Will have the highest first ionization energies 15. 3.5 moles (D) Green (D) 6. Bromine liquid 19.0 moles of H2 at STP 7.0 grams of SO2 at STP Questions 9–11 Questions 20–22 (A) Voltaic cell (A) Water (B) Electrolytic cell (B) Hydrogen bromide (C) Geiger Counter (C) Iron (D) pH meter (D) Argon (E) Calorimeter (E) Sodium chloride 9. A reaction will be spontaneous if ∆H is BECAUSE ∆G will be negative when there is a decrease in negative and ∆S is positive enthalpy and an increase in entropy. An electrolytic cell makes a BECAUSE an electrolytic cell uses an external current to drive nonspontaneous redox reaction occur a redox reaction. gas to expand GO ON TO THE NEXT PAGE Page 128 of 136 . SAMPLE ANSWER I II CE* EX 1 F F I II 101. determine whether statement I in the left- most column is true or false and whether statement II in the rightmost column is true or false. 103. 106. Cl1− is the conjugate base of HCl BECAUSE a conjugate base is formed when an acid gains a proton. An increase in temperature will cause a BECAUSE temperature and volume have a direct relationship. Fill in the oval labeled “CE” only if statement II correctly explains statement I. An element’s nuclear charge is equal to BECAUSE the only charged particles in the nucleus are the number of protons in the nucleus neutrons.means “one thousandth. Fill in the corresponding T or F ovals on the answer sheet provided.PRACTICE TEST 4 265 PRACTICE TEST—Continued PLEASE GO TO THE SPECIAL SECTION AT THE LOWER LEFT-HAND CORNER OF YOUR ANSWER SHEET LABELED “CHEMISTRY” AND ANSWER QUESTIONS 101–115 ACCORDING TO THE FOLLOWING DIRECTIONS. 3.000 kilograms is equal to 3 grams BECAUSE the prefix kilo. 104. SAMPLE: EX 1.” 107. The maximum number of electrons BECAUSE the maximum number of electrons allowed in a allowed in the third principal energy principal energy level is dictated by the level is 18 equation 2n2. The nucleus of an atom has a BECAUSE the only positive particles positive charge found in the atom’s nucleus are protons. 102. For each question. 105. Part B Directions: Each question below consists of two statements. GO ON TO THE NEXT PAGE Page 129 of 136 . 114. Nitrogen gas will have a greater rate of BECAUSE lighter. Helium will have fewer dispersion forces BECAUSE as the mass of nonpolar atoms and molecules between its atoms than the other noble increases. less dense gases travel faster than heavier. Propane can be decomposed chemically BECAUSE propane is a compound that is made up of simpler elements. A catalyst will change the heat of BECAUSE a catalyst will lower the potential energy of the reaction activated complex in a reaction. 109. Butene can be converted into butane BECAUSE the addition reaction of hydrogen gas to an alkene will form an alkane. NaCl is a basic salt BECAUSE hydrolysis of NaCl reveals the formation of NaOH and HCl. 111.266 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 108. 112. Isotopes have different atomic numbers BECAUSE isotopes must have different numbers of electrons. gases 110. effusion than oxygen gas more dense gases. A mixture of two different liquids can be BECAUSE different liquids have different boiling points. 115. dispersion forces increase. separated via distillation 113. mal compared to the volume within which the gas is contained. Which statement below best describes the molecule in kinetic molecular theory? question? (A) The average kinetic energy of gas molecules is (A) Water has a bent molecular geometry and one directly proportional to temperature.004 has five significant figures. random (D) Carbon dioxide is linear because it has one sin- motion. Nuclear waste (A) Zeros can be significant. the answer is determined by the (B) II only number of decimal places. Select the one answer that is best in each case and then fill in the corresponding oval on the answer sheet pro- vided.PRACTICE TEST 4 267 PRACTICE TEST—Continued Part C Directions: Each of the multiple-choice questions or incomplete sentences below is followed by five answers or comple- tions. (C) Collisions between gas molecules are perfectly (C) Methane has a trigonal planar molecular geom- elastic. (E) The volume that gas molecules occupy is mini. etry. Which statement regarding significant figures is false? I. Which of the following statements is not part of the 31. gle bond and one triple bond. When 58 grams of water is heated from 275 K to 365 K. (E) The carbon atoms in ethane are sp3 hybridized. the answer is determined by III. Excess exposure the number of significant figures. lone pair of electrons. geometry and two lone pairs of electrons. The following redox reaction occurs in an acidic solu- the water tion: Ce4+ + Bi → Ce3+ + BiO1+. (C) III only (D) When dividing. the answer is determined by the (D) I and II only number of decimal places.220 joules of heat (B) 2 (D) absorbs 242 joules of heat (C) 3 (E) releases 90 joules of heat (D) 6 (E) 9 27. GO ON TO THE NEXT PAGE Page 130 of 136 . 28. What is the coefficient (A) absorbs 21. 29. (B) Attractive and repulsive forces are present (B) Ammonia has a trigonal pyramidal molecular between gas molecules. 26. (E) I and III only (E) The number 50. (A) I only (C) When adding. (D) Gas molecules travel in a continuous.820 joules of heat before the Ce4+ when the equation is fully balanced? (B) absorbs 377 joules of heat (A) 1 (C) releases 5. Which of the following are uses for radiation and radioactivity that are of benefit to us? 30. Radioisotopes (B) When multiplying. II. II.268 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 32.0 m CaCl2 38.0 × 10−2 (B) 2.) The level of mercury for this compound? moves to a new height as can be seen in the diagram. what is the atmospheric pressure in this case? (C) CO2Cl2 (D) C2O2Cl Atmospheric (E) CCl2O Pressure 33. which would react with rain water (C) 750 torr to produce acid rain? (D) 815 torr I.5 m NaCl (E) 1.5 m C6H12O6 (E) I. Carbon dioxide 37. and 16. 36.7% Cl. Which process would have a positive value for the change in entropy? Gas I.0 × 10−7 (D) 3. 34.7% by mass.0 × 10−4 (E) 1. A sample of gas is trapped in a manometer and the stop- 71. Which aqueous solution is expected to have the high- (A) I only est boiling point? (B) II only (A) 1. and III (D) 2. (D) Carbon is 72% by mass. (E) Carbon is 20% by mass. A food fight in a school cafeteria (A) I only (B) II only (C) III only (D) II and III only Figure 1 (E) I and III only (A) 760 torr (B) 740 torr 35. (A) C2OCl If the pressure of the gas inside the manometer is 815 (B) COCl torr. (C) Hydrogen is 12% by mass. Which Ka value is that of a better electrolyte? (A) 1.0 m CH3OH (D) I and III only (C) 2. Of the gases below.0 × 10−12 (C) 5. The expansion of the universe 65 mm II. What is the empirical formula cock is opened.3% by mass.5 m FeCl2 (C) III only (B) 3. A compound was analyzed and found to be 12.1% C. Methane III. The condensation of a liquid III. (B) Oxygen is 53.0 × 10−6 GO ON TO THE NEXT PAGE Page 131 of 136 .2% O. CFCs (E) 880 torr II. (See Figure 1. Which statement is true about the percent composition by mass in C6H12O6? (A) Carbon is 6. Which sample is a homogeneous mixture? (A) KI(aq) (D) K eq = [ NO 2 Cl ]2 (B) Fe(s) [ Cl 2 ][ NO 2 ]2 (C) CO2(g) (D) NH3(l) [ NO 2 Cl ]2 (E) NaCl(s) (E) K eq = [ Cl 2 ]2 [ NO 2 ]2 GO ON TO THE NEXT PAGE Page 132 of 136 . How many grams of methane gas were burned if 67.2 M stance will have a decrease in its solubility? (A) NaCl What is the value of the equilibrium constant for this (B) KI reaction? (C) CaCl2 (A) 2.2 43. The following substances were all dissolved in 100 42. tions of the substances in question 41 are as follows: tions.PRACTICE TEST 4 269 PRACTICE TEST—Continued 39.48 (E) KNO3 (C) 0.83 to the reaction CH4(g) + 2O2(g) → CO2(g) + 2H2O(l).4 grams (D) N N 41. A closed system contains the following reaction at STP: Cl2(g) + 2NO2(g) ←→ 2NO2Cl(g). Which reaction below demonstrates the Lewis defini- [ Cl 2 ][ NO 2 ] tion of acids and bases? (A) HCl + NaOH → HOH + NaCl [ Cl 2 ][ NO 2 ]2 (B) K eq = (B) H2O + NH3 → OH1− + NH41+ [ NO 2 Cl ] (C) NH3 + BF3 → NH3BF3 (D) HI + KOH → H2O + KI [ Cl 2 ][ NO 2 ]2 (E) H+ + OH1− → H2O (C) K eq = [ NO 2 Cl ]2 45. rectly in Figure 2? tion? (Assume STP. If the solution is heated to 310 K.0357 (D) 20. the equilibrium concentra- grams of water at 290 K to produce saturated solu. At a particular temperature.1 (D) HCl (B) 0.5 M [Cl2] = 0. Methane undergoes a combustion reaction according (E) 208. Which Lewis structure below has been drawn incor- liters of carbon dioxide gas are produced in the reac. which sub- [NO2Cl] = 0.) (A) H H (A) 16 grams (B) 48 grams (B) H C N (C) 3 grams (C) H O (D) 132 grams H (E) 22.3 M [NO2] = 0.83 40. What is the (E) F B F F equilibrium constant expression for this reaction? Figure 2 [ NO 2 Cl ]2 (A) K eq = 44. How many pi bonds are there in a molecule of gas N— C—CH2—CH2—CO—NH—CH—CH2? (C) 12 grams of hydrogen gas and 56 grams of (A) 7 nitrogen gas (B) 4 (D) 102 grams of hydrogen gas and 34 grams of (C) 12 nitrogen gas (D) 10 (E) 6 grams of hydrogen gas and 2 grams of nitro- (E) 5 gen gas 49. the sum of the coefficients will be (B) K2O / potassium oxide (A) 4 (C) NO2 / nitrogen dioxide (B) 9. and III gen gas (B) 3 grams of hydrogen gas and 1 gram of nitrogen 48. Push a thermometer through a rubber stopper (D) II and III only III. Which solutions have a concentration of 1. Eat and drink in the laboratory (C) I and III only II.270 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 46.5 grams of potassium chloride dissolved to (C) CH3CH(Cl)CH3 and CH3CH2CH2Cl make 1 liter of solution (D) CH3COCH3 and CH3CH2CH2CHO III. When the equation: C2H6 + O2 → CO2 + H2O is com. 87 grams of lithium bromide dissolved to make (E) ClCH2CH2Br and BrCH2CH2Cl 1 liter solution (A) I only 47. 51.100 kJ (C) +2. 53. (A) FeCl2 / iron(II) chloride ficients. From the heats of reaction of these individual reactions: A + B → 2C ∆H = −500 kJ. 2D + 2A → F ∆H = +50 kJ Find the heat of reaction for F + 6B → 2E + 4C.350 kJ (D) −350 kJ (E) −2. II.450 kJ GO ON TO THE NEXT PAGE Page 133 of 136 . 74.5 (D) PCl3 / potassium trichloride (C) 19 (E) NH4Cl / ammonium chloride (D) 15. Which would you never do in a laboratory setting? (B) III only I. and III reaction (A) I only 52. Remove your goggles to take a better look at a (E) I.0 M? pound? I. D + 2B → E ∆H = −700 kJ. Which compound is not paired with its correct name? pletely balanced using the lowest whole number coef. According to the reaction 3H2 + N2 → 2NH3. how (B) II only many grams of hydrogen gas and nitrogen gas are (C) III only needed to make exactly 68 grams of ammonia? (D) I and III only (A) 2 grams of hydrogen gas and 28 grams of nitro- (E) I. Which pair below represents isomers of the same com. (A) +450 kJ (B) −1.5 (E) 11 50. II. 74 grams of calcium hydroxide dissolved to (A) CH3CH2CH2OH and HOCH2CH2CH3 make 1 liter of solution (B) CH3CH2CH3 and CH3CH2CH2CH3 II. (D) The Ksp value will change. (B) The concentration of calcium ions will increase. (A) 0. (B) 0.334 J (E) Sugar water—filter paper 61. to it. hydrogen in excess.50 M (D) Increase the pressure. a gas without having a liquid phase. Naphthalene (C) Ca2+ + CO32− III. (C) 768 grams of HI can be made with 38 grams of (E) The equilibrium will shift to consume the iodine in excess. II. (D) 2286 grams of HI can be made with no excess reactants.258 J (C) Sand and water—separatory funnel (D) 350 J (D) Sand and sugar—tweezers (E) 5. what could be done to the reaction to shift the reactants.368 J (B) Salt water—distillation (C) 18.40 M it becomes a completely solid ice cube at 273 K.28 M (E) Remove B from the reaction. Sublimation is the process by which a solid becomes 57. 500 mL of a 0.70 M (D) 0. Which mixture is correctly paired with a method for this ice cube? separation of the mixture? (A) 16 J (A) Oil and water—filter paper (B) 4. (B) 768 grams of HI can be made with 6 grams of (C) The reaction will shift to the right. How many grams of HI can be made from 6 grams 58. How much heat was released by the sample of water to form 56. Iodine (B) Pb2+ + 2I1− II. equilibrium so that more D is made? (A) Increase the concentration of D. Which reaction between ions does not form a precipi. 55. Which will happen when sodium sulfate is added to a of H2 and 800 grams of I2 when hydrogen gas and saturated solution of CaSO4 that is at equilibrium? diatomic iodine react according to the equation: [CaSO4(s) ←→ Ca2+(aq) + SO42−(aq)] H2 + I2 → 2HI? (A) The solubility of the calcium sulfate will (A) 800 grams of HI can be made with 38 grams of decrease.14 M 60. decrease in sulfate ions. Which of these tate? can sublime? (A) Ag1+ + Cl1− I. Given the reaction 2A(g) + B(g) + Heat ←→ 3C(g) + (E) 806 grams of HI can be made with no excess D(g). A 16-gram sample of water at 273 K is cooled so that (E) 0. What is the new molarity of this solution? (C) Increase the temperature. (C) 0. 59.PRACTICE TEST 4 271 PRACTICE TEST—Continued 54. and III GO ON TO THE NEXT PAGE Page 134 of 136 . iodine in excess.2 M solution has 200 mL of water added (B) Increase the concentration of C. Carbon dioxide (D) Hg2+ + 2Br1− (A) I only (E) Na1+ + OH1− (B) II only (C) III only (D) I and III only (E) I. Which statement is true about the setup above? (A) The electrode potential for this cell is 1. 63. and (C) Electrons will be carried by the salt bridge. What is true about the partial pressures of the (E) The reaction is nonspontaneous. (C) Ni → Ni2+ + 2e– solved in water (D) 2Al3+ + 6e– → 2Al (C) Decreasing the temperature (E) Al3+ + 3e– → Al (D) Increasing the pressure (E) Adding a catalyst 65. (C) The partial pressure of gas C is 220 torr.54 V.272 PART IV / FOUR FULL-LENGTH PRACTICE TESTS PRACTICE TEST—Continued 62. Which of the following will decrease the rate of a reac. The con.3 moles of gas A. What is the half reaction that occurs at the cathode? tion? (A) Al →Al3+ + 3e– (A) Using powdered solids instead of whole pieces (B) Ni2+ + 2e– → Ni (B) Selecting ionic reactants that have been dis. (E) The partial pressure of gas B is 660 torr. The total pressure of the gases is (D) Ions will be carried through the wire.40 V. (B) The partial pressure of gas B is 396 torr.3 moles of gas C. Questions 64 and 65 refer to the voltaic cell below in Figure 2: Wire Salt Bridge Ni Electrode Al Electrode Ni2+(aq) Al3+(aq) Figure 2 GO ON TO THE NEXT PAGE Page 135 of 136 . gases? (A) The partial pressure of gas A is 264 torr. 64. 0. tainer has 0. (B) The electrode potential for this cell is 2. (D) The partial pressures of gases A and C are each 198 torr. 0.4 moles of gas B. 660 torr. Three gases are mixed in a sealed container. GO BACK AND CHECK YOUR WORK. (A) The pH of the stream now is one time more (A) −118 kJ acidic than it was years ago. (C) can be shifted by adding a catalyst gen. Equilibrium ago. appendix. (B) +118 kJ (B) The stream now has 10 times more hydroxide (C) −91 kJ ions than it did years ago. Which functional group below does not contain a car- bonyl group? (A) Aldehydes (B) Ketones (C) Esters (D) Ethers (E) Carboxylic acids S T O P IF YOU FINISH BEFORE TIME IS CALLED. (B) is defined as equal rates for forward and reverse reactions 67. reacts with oxy. What is going to be the general formula for the (D) can exist for chemical changes but not physical compound formed? changes (A) M2O (E) must always favor the formation of products (B) MO (C) MO2 (D) M2O3 (E) M3O2 68. (D) −1.9 to a pH of 5. An alkaline earth metal. (D) The stream is more basic now than it was years 70.042 kJ (C) The pH of the stream is now 10 times more (E) −833 kJ acidic than it was years ago.PRACTICE TEST 4 273 PRACTICE TEST—Continued 66. Over a number of years the average pH of a stream 69. element M.9 due to acid rain. calculate the change in the heat of reaction Which statement is true about the pH of the stream? for 2H2 + O2 → 2H2O. Using the bond dissociation energies found in the changes from a pH of 6. Page 136 of 136 . (A) is defined as equal concentrations of reactants (E) The concentration of hydronium ion in the and products stream has decreased over the years.