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1. CHEMISTRY TEST Note: For all questions involving solutions, assume that the solvent is water unless otherwise stated. Throughout the test the following symbols have…
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  • 1. CHEMISTRY TEST Note: For all questions involving solutions, assume that the solvent is water unless otherwise stated. Throughout the test the following symbols have the definitions specified unless otherwise noted. H M n P R s T V enthalpy molar number of moles pressure molar gas constant entropy temperature volume atm ob J KJ] L mL flrm mol V atmosphere(s) gram(s) joule(s) kilojoule(s) liter(s) milliliter(s) millimeter(s) mole(s) volt(s) Part A Directions: Each set of lettered choices below refers to the numbered statements or questions immediately fol- bwing it. Select the one lettered choice that best fits each statement or answers each question and then fiIl in the oorreslonding circle 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 elements for which the 3nound-state electron configurations are shown lelorv. (A) lsz }sr (B) lsz 2s2 (c) ls2 2s22p2 (D) rs2 2s22p5 (E) 1s2 2s22p6 The configuration of the element with the largest second ionization energy The configuration of the element whose atoms are most likely to form four covalent bonds The configuration of the element most likely to form diatomic molecules of the form X2 The configuration of the element that exists as single gaseous atoms at OoC and 1 atm Questions 5-7 refer to the following. (A) White precipitate (B) Blue precipitate (C) Orange precipitate (D) Gas bubbles (E) No change 5. Observed when concentrated hydrochloric acid is added to calcium carbonate Observed when sodium sulfate solution is added to barium chloride solution Observed when sodium chloride solution is added to potassium nitrate solution 6. 7. ,119-
  • 2. CHEMISTRY TEST-Co ntinued Questions 8-10 are based on the following heating curve for a pure substance. The substance begins as a solid and ends as a gas; each segment represents a different process. 8. Boiling 9. Melting 10. A gas is heated. () d l-r 0) O{ ,c) F Unauthorized copying or reuse of any part of this page is lllegal. Energy Added (kJ) -120-
  • 3. Questions (A) CHEMISTRY TEST: C ontinue d ll-14 refer to the following graphs. (B) (D) copying or reuse of part of this page is i!!egal. 1 1. Which graph could represent the pH of a 0.1 M solution of nitric acidverszs the volume of a 0.1 M solution of sodium hydroxide that is added to it? 12. Which graph could represent the concentration of one reactant versus time as a reaction approaches and reaches equilibrium? 13. Which graph could represent the pressure of a sample of an ideal gas versus its absolute temperature at constant volume? 14. Which graph could represent the product of pressure times volume, PV, for an ideal gas versus its pressure at constant temperature? -121-
  • 4. CHEMISTRY TEsT-Continued Questions 15-17 refer to the following types of substances. (A) Hydride (B) Halide (C) Hydroxide (D) Hydrate (E) Hydrocarbon 15. A crystalline substance in which water is one of the structural units 16. A compound that contains only a metal and hydrogen 17. An organic compound Questions 18-19 refer to the following substancm at room temperature. (A) CO2 (B) N2O (c) No2 (D) SiO2 (E) Cao 18. Is an ionic solid 19. Is a gas in which each molecule has an unpairal electron Unauthorized copying or reuse of any part of this page is illegal. Questions 20-22 (A) Oxidation (B) Decomposition (C) Precipitation (D) Acid-base (E) Reduction Which of the above best describes the reaction represented by each of the following equations? 20. CaCOr(s) + CaO(s) + COz(S) 21. Pb2+(ae) + 2 I-(aq) + Pblr(s) 22. Fez+(aq) -+ Fe3*1aq) + e- GO ON TO THE NEXT PAGE -122-
  • 5. CHEMISTRY TEST- C o ntinu e d Questions 23-25 refer to the following energy diagram. Principal Quantum Numbers 5 4 3 2 ( The diagram above is a plot of the energy levels for the electron of the hydrogen atom (roughly to scale) according to the Bohr theory. The vertical lines represent possible transitions (increases or decreases of energy) that can occur. 23. The transition from the ground state to the first excited state of hydrogen 24. Otthe transitions shown, the one that involves the LEAST energy 25. The transition that represents the ionization energy of hydrogen C) >, bo o r! -14.0 -123-
  • 6. CHEMISTRY TEST- C ontinu e d PLEASE GO TO THE SPECIAL SECTION AT THE LOWER LFFT-HAND CORNER OF THE PAGE OF THE ANSWER SHEET YOU ARE WORKING ON AND ANSWER QUESTIONS 101-115 ACCORDTNG TO THE FOLLOWTNG DTRECTIONS. Part B Directions: Each question below consists of two statements, I in the left-hand colunrn and II in the right-hand column. For each question, determine whether statement I is true or false and whether statement tr is true or false and fiIl in the corresponding T or F circles on your answer sheet. Fill in circle CE only if statement tr is a correct explanation of the true statement I. EXAMPLES: .I II EX 1. H2SO4 is a strong acid BECAUSE H2SO4 contains sulfur. EX 2. An atom of oxygen is BECAUSE an oxygen atom contains an equal electrically neutral number of protons and electrons. SAMPLE ANSWERS HXl I II CE* o@ a@ o@ a@ C oE){2 I 101. The volume of a gas at constant pressure increases with increasing temperature 102. A I M solution of sodium hydroxide has a high pH 103. H2S is a polar substance 104. In its ground state, a magnesium atom has more electrons in its outer shell than does a potassium atom 105. Liquid water in an open container evaporates 106. Metallic copper is an electrical conductor 107 . Acetic acid, HC2H3O 2, is a stronger acid than sulfuric acid II BECAUSE the average speed of gas molecules decreases with increasing temperature. BECAUSE solutions with a high H+ concentration have a high pH. BECAUSE HrS is a gas at room temperature. BECAUSE the total number of electrons in a magnesium ' atom is greater than the total number of electrons in a potassium atom. BECAUSE some molecules at the surface of liquid water in an open container have enough lcinetic energy to overcome intermolecular attractions. BECAUSE in metallic copper, the atoms of copper ilre coyalently bonded. BECAUSE acetic acid has more hydrogen atoms in its molecular structure than does sulfuric acid. Unauthorized copying or reuse of any part of this page is illegal. -124-
  • 7. CHEMISTRY TEST- C ontinued I 108. Under identical conditions, N2(g) is more chemically reactive than Oz@) 109. To prepare a 1 M solution of chloride ions from CaCl, (molar mass 110 g/mol), 110 g of CaCl2 should be dissolved in I L of solution 110. The first ionization energy of K is greater than that of Li 111. Catalysts increase the rates of chemical reactions BECAUSE the N2(g) molecule has a single bond and the Oz(S) molecule has a double bond. BECAUSE each mole of CaCl, dissolves to produce I mol of chloride ions. BECAUSE the Li atom has a smaller radius than the K atom. BECAUSE the activation energy of a reaction is lowered by a catalyst for the reaction. ll2. In the paper chromatography experiment represented above, component 1 moved up fastest 113. The boiling point of water, HzO, is much higher than that of methane, CH4, 115. Atzs"C,the average speed of Hr(g) molecules is less than the average speed of Oz(S) molecules Unauthorized copying or reuse of any part of this page is Solvent Front Component 3 Component 2 Component I Original Spot BECAUSE in the paper chromatography experiment represented above, component I moved a shorter distance up the paper than component 2 or 3 did. BECAUSE the molar mass of water is greater than that of methane. BECAUSE at25"C, the average kinetic energy of H2G) molecules is less than the average kinetic energy of Or(g) molecules. lF( e o a @ @ @ O 2C2H6@) + 7 O2G) -+ COr(g) + 6HrO(J) 114. For the reaction represented by the equation BECAUSE in the reaction represented above, there are above, the entropy increases as the products more moles of products than of reactants. form -125-
  • 8. CHEMISTRY TEST- C ontinue d 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 fiI1 in the corresponding circle on the answer sheet. 26. The oxidation number of S in SO3 is (A) +2 (B) +3 (C) +4 (D) +5 (E) +6 CrHs(s) + 5O2(g) + ZCOz@) + 4H2O(s) 27. How many moles of water would be produced if 1 1.0 g of propane (molar mass 44 g mol) were burned completely to carbon dioxide and water according to the equation represented above? (A) 1.0 mol (B) 2.0 mol (C) 3.0 mol (D) 4.0 mol (E) 5.0 mol Zn(s) + ZAg+(aq) + Znz+(aq) + 2Ag(s) 28. Which of the following is true of the reaction represented above? (A) Zn(s) is the oxidizing agent. (B) Ag*(aq) rs the oxidizingagent. (C) Zn(s) is reduced. (D) Ag*(aq) is oxidized. (E) A mole of electrons is transferred for each 0.5 mol of Ag(s) produced. . . . NH3(g) +. . . o2(s) -+. . . Nz(s) +. . . Hzo(s) 29. When the equation for the reaction represented above is balanced with all the coefficients reduced to the lowest whole-number terms, the coefficient for Or(g) is (A) 1 (B) 2 (c) 3 (D) 4 (E) 6 Unauthorized copying or reuse of any pert of this page is illegal. 30. When 0.0025 mol of HCI and 0.0035 mol of NaOH are added to water to make 1 L of solution, the pH of the resulting solution is approximately (A) 1 (B) 3 (c) 7 (D) 11 (E) t4 31. Which of the following molecules is polar? (A) Cl2 (B) C2H6 (c) NH3 (D) CO2 (E) CC14 32. An atom of which of the following elements has the greatest number of valence electrons? (A) Iodine (B) Arsenic (C) Barium (D) Oxygen (E) Carbon 33. Which of the following contains the greatest number of atoms? (A) 1.0 g of Fe (B) 1.0 g of U (C) 1.0 g of Li (D) 1.0 g of S (E) 1.0 g of C 34. What is the maximum mass of Al (molar mass 27 glmol) that can be obtained from 20.4 g of pure Al2O3 (molar mass 102 glmol) ? (A) 2.70 g (B) 5.40 g (C) 8.10 g (D) 10.8 g (E) 16.3 g -126-
  • 9. @ CHEMISTRY TEST- Continue d 35. Of the following solutions, which has the highest boiling point? (A) 0.1 M sucrose, CrrH zzOrt (B) 0.1 M acetic acid, HCzH3Oz (C) 0.1M NaCl (D) 0.1 M CaCt, (E) 0.1 M Alcl3 2 A(d + B(s) e C(s) + D(s) 36. Which of the following is likely to have the smallest effect on the equilibrium concentrations of reactants and products in the gas-phase reaction represented above? (A) Decreasing the temperature of the system by 25"C (B) Decreasing the volume of the system by half (C) Removing one of the products of the reaction from the system (D) Doubling the amount of one of the reactants in the system (E) Adding a small amount of a catalyst for the reaction to the system Unauthorized copying or reuse of any part of this page is lllegal. 37 . Ot the following, the conditions under which the molar volume of gaseous helium is greatest are (A) 237 K and I atm (B) 300 K and I atm (C) 400 K and I atm (D) 500 K and2 atm (E) 600 K and2 atm 38. How many grams of RbNO: (molar mass 147 glmol) are required to produce 0.500 L of a 0.200 M RbNO3 solution? (A) 73.5 g (B) 2e.6 g (C) 14.7 g (D) 2.e6 g (E) t.47 g 39. SiO2 has a high melting point because its solid state structure is (A) ionic (B) metallic (C) hydrogen bonded (D) nonpolar covalent molecular (E) covalent network . . . Pb(NO)2(s) + . . . PbO(s) + . . . NOr(s) + . . . Oz(s) 40. When the equation above is balanced and all coefficients are reduced to lowest whole-number terms, the coefficient for NO2(s) is (A) 2 (B) 4 (c) 6 (D) 8 (E) 10 -127-
  • 10. 41. Which of the following solutions has the lowest [H*] ? (A) 0.t0 M HNO2 (B) 0.r0 M HNO3 (c) 0.r0 M H2so4 (D) 0.ro M HCt (E) 0.10 M HBr 42. At 4"C, a 10. mL container filled with water has a mass of 35.6 g. The same container filled with methanol has a mass of 33.5 g. What is the approximate density of methanol? (The density of water at 4"C is 1.00 glmL.) (A) 0.79 slntL (B) 1.0 g/ml. (C) t.3 gmL (D) 2.1 glml, (E) 3.3 glmt- 43. Compounds that have the empirical formula CH include which of the following? I. HrC:::= CH, tr. HC=CH H .C / M. HC CH tilHC CH ./ fi (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III Unauthorized copying or reuse of any part of this page is illegal. CHEMISTRY TEST-Co ntinae d 44. The Fe3* ion contains how many electrons? (A) 23 (B) 26 (c) 2e (D) 31 (E) s3 45. The formula for the chloride of radium is (A) RaCl (B) RaCl2 (C) RaCl, (D) RqCl (E) RarCl, 46. Asample of H2(g) is stored in a 0.500 L vessel at 90.0 torr and 300. K. The gas is transferred to a 1.50 L vessel at constant temperature. Which of the following statements about the gas is correctl (A) The number of moles of H2(S) increases. (B) The number of moles of Hr(g) decreases. -(C) The pressure of the H2(S) increases to 270. tol:.. (D) The pressure of the Hz(S) decreases to 30.0 torr. (E) The pressure of the H2(g) remains unchanged. 47 . How many moles of O2G) are formed when a 6.0 mol sample of KCIOr(s) decomposes completely to produce C,2(6) and KCI(s) ? (A) 1.5 mol (B) 3.0 mol (C) 6.0 mol (D) 9.0 mol (E) 12 mol -128-
  • 11. CHEMISTRY TEST_ Continued c (graphite) + oz(s) + CozG) a,H = _3g4kt C (diamond) + Oz(S) -; COr(s) Ut = _396 kJ 48' on the basis of the information above, what is the change in enthalpy, LH, for the following reaction? C (graphite) + C (diamond) (A) -790 kJ (B) 4kJ (c) -2kI (D) +2kJ (E) +790 kr ''' Zn(s) + . . . NaoH(aq) + . . . HzC,(r) -) . . . NarZn(O H)o@Q +. . . Hzk) -'' X5?.1l:;ffi'Hdi;":Jt balanced and all coefficients are reduced to rowest whole-number terms, the (A) I (B) 2 (c) 3 (D) + (E) s -129-
  • 12. CHEMISTRY TEST- Continued 50. Which of the following best describes the type of bonding between iodine atoms in a molecule of Ir? (A) Ionic bonding (B) Metallic bonding (C) Hydrogen bonding (D) Covalent bonding (E) Dispersion (London) force interactions 51. When NarSOo dissolves in water, which of the following species is present in the greatest concentration in the solution? (A) Na+(aq) (ts) NarSO+(aq) (C) SOo2-(aq) (D) S2-(aq) (E) oz-(oq) 52. Which of the following statements is true of a solution of 0.10 M HCI(aq) ? (A) The pH is 1. (B) The concentration of Cl-(aq) is greater than the concentration of H+(aq). (C) The concentration of Cl-(aq) is equal to the concentration of OH-(aq). (D) The concentration of H*(aq) is equal to the concentration of OH-(aq). (E) The indicator phenolphthalein turns pink when added to the acid solution. 53. The half-life for the radioactive decay of ,32p" is 25,000 years. If 100. g of '32p" are presenr initially, how many grams of '32p" will remain after 50,000 years? (A) 100. e (B) 50.0 g (C) 25.0 g (D) 12.5 g (E) 0.000 g Unauthorized copying or reuse of any part of this page is illegal. 54. Which of the formulas above represent isomr. one another? (A) None (B) I and II only (C) I and III only (D) II and III only (E) I, II, and III 55. Which of the following is always characterisu_ an oxidizing agent? (A) It contains oxygen. (B) It is soluble in water. (C) It contains a transition element. (D) It can be reduced. (E) It forms an ionic lattice. 56. Which of the following statements about a lic*u that evaporates readily at room temperature ii correct? (A) It has strong intermolecular forces. (B) It has a high vapor pressure. (C) It is considered to be nonvolatile. (D) It would make its container feel warm rt, -Jr touch. (E) It should be stored in an open container. ' ,/cl C:C H/ "' I I Cl ,/C:CH' m "' /cC:C H/ , II GO ON TO THE NEXT PAGE -130-
  • 13. CHBMISTRY TEsT-Continued Hz(s)+Brr(g) e 2HBr(s) 57. Which of the following is an appropriate expression for the equilibrium constant of the reaction represented above? (A) K,=ffi lH,llBrz l (B) Kr=ffi IHBr](C) Kr=ffi IHBr]2(D) K,= 6ffiryi (E) K. = tHP'l'= _/ ^^c Etl2[gr]2 58. Atoms with high first ionization energies always have (A) relatively tightly bound outermost electrons (B) multiple oxidation states (C) low electronegativities (D) large atomic radii (E) distinctly metallic properties 59. Substances that can act both as an acid and as a base in aqueous solution include which of the following? I. Cl_ II. HSO4- III. CO32- (A) I only (B) II only (C) m only (D) I and II only (E) II and III only Unauthorized copying or reuse of any part of this page is illegal. ...CzHsOH(/) + ...O2@) +...COr(s) + ...HzO(s) 60. When the combustion reaction represented by the equation above is balanced using the lowest whole-number coefficients, what is the coefficient of Or(g) ? (A) 2 (B) 3 (c) 4 (D) s (E) 6 -131-
  • 14. 61. When 28 g of Fe reacts as completely as possible with 8.0 g of S to form FeS, which of the following is true? (A) Approximately 4.0 g of S remains unreacted. (B) Approximately 14 g of Fe remains unreacted. (C) Approximately equal masses of Fe and S react. (D) Approximately Z7 g of FeS is produced. (E) Approximately 36 g of FeS is produced. 62. A 9.0 g sample of liquid water has which of the following? I. 1.0 mol of hydrogen atoms II. 8.5 g. of oxygen III. A volume of 11 .2L at standard temperature and pressure (A) I only (B) II only (C) m only (D) I and II only (E) I, II, and III 63. How much energy is required to heat 100. g of HrO from 20.0"C to 40.0"C ? (The specific heat of HrO(/) is 4.18 J/(g.'C).) (A) e3.6I (B) 482 J (c) 2,000 J (D) 4,180 J (E) 8,360 J 64.If a student were to accurately analyze a mixture of solid NaCl and solid NaOH by titration of the hydroxide ion with a standardized solution of HCl, which of the following would be LEAST useful? (A) Bunsen burner (B) Analytical balance (C) Buret (D) Erlenmeyer flask (E) Indicator Unauthorized copying or reuse of any part of this page is illegal. CHEMISTRY TEST- Continued lt (d + Clr(s) + 2 HCI(s) LH = -185 kJ 65. According to the equation for the reaction represented above, what is A^FI for the production of 0.100 mol of HCI(g) ? (A) -37.0 kJ (B) -18.s kJ (c) -e.zs kJ (D) +9.25 kJ (E) +18.5 kJ 2SOz(s) + Oz(s) e 2SOr(s) + heat 66. For the system represented above, which of the following actions will shift the position of equilibrium to the left? (A) Increasing the pressure (B) Increasing the temperature (C) Putting the mixture in a smaller container (D) Adding some Oz(S) (E) Removing some SO3(S) 67. When Na(s) reacts with excess H2O(l), product*. of the reaction include which of the following? I. Na+(a4) II. OH-(aq) III. Hr(g) (A) I only (B) III only (C) I and II only (D) I and III only (E) I, II, and III 68. When the following air pollutants are presenr in small amounts, which is LEAST hazardous to humans? (A) Ammonia, NH: (B) Carbon dioxide, CO, (C) Sulfur dioxide, SOz (D) Nitrogen dioxide, NO, (E) Hydrogen sulfide, HrS GO ON TO THE NEXT PAGE -132-
  • 15. CHEMISTRY TEST- C ontinued 69. A compound containing only carbon and hydrogen is found to have a molar mass of 100 g/mol and to consist of 16 percent hydrogen by mass. The number of carbon atoms in one molecule of the compound is (A) I (B) 3 (c) 4 (D) 6 (E) 7 70. A 21 g sample of NaF(s) (molar mass 42 glmol) is dissolved in enough water to yield 2.0 L of solution. What is the molar concentration of Na+(aq) ? (A) 0.010 M (B) 0.0s0 M (c) O.Lo M (D) 0.2s M (E) 0.s0 M STOP IF YOU FINISH BEFORE TIME IS CALLED, YOU MAY CHECK YOUR WORK ON THIS TEST ONLY. DO NOT TURN TO ANY OTHER TEST IN THIS BOOK. Unauthorized copying or reuse of any part of this page is illegal. -133-
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