ࡱ>  uwtz{?Wq] @bjbj:: ,X*\X*\7?@$P*T~4^0OOO5777777$[|O[0p***Nl:05*5**J Y\,q 0 [ $!0w $ " $q $q OvT*D]<OOO[[(OOO$OOOOOOOOO> : Chemistry 120: Final Exam Practice Question 1. How many significant figures are in the volume measurement 15.56 mL? 6 4 3 2 none of the above Question 2. Name the term for an extensively tested proposal of a scientific principle that states a measurable relationship under different experimental conditions? scientific law scientific method hypothesis scientific theory experiment Question 3. How many gallons are in 4.78 g of water (density = 1.00 g/mL)? 1.26 x 10-3 gallons 1.26 x 103 gallons 0.00126 4.78 x 103 gallons none of the above Question 4. In 1 cm there are _____ mm. 1000 100 10 11 none of the above Question 5. The density of olive oil is 0.918 g/mL, if 2.00 mL of oil are added to a hot pan, how many grams is that? 1.836 g 1.84 g 1.84 0.459 g 2.18 g Question 6. How many ft3 are in 255 mm3? 9.00 x 10-6 ft3 0.837 ft3 17.2 ft3 160,000 ft3 none of the above Question 7. What is 400.0 K in Fahrenheit? 126.9 F 752.0 F 353 F 260.3 F none of the above Question 8. Convert 0.0011540 to scientific notation. 1.154 x 103 11.540 x 10-4 1.1540 x 10-3 0.1154 x 10-4 none of the above Question 9. Complete the following calculation to the correct number of significant figures: 376.5 (23.555)(1.1) = 350.5895 351 376.5 352.9 350.6 Question 10. 55.7 is what percent of 95.7? 172% 95.5% 58.2% 85.2% none of the above Question 11. Record the measurement to the correct number of significant figures:  EMBED PBrush  Question 12. Which of the following is a chemical change? burning of coal oxidation of copper fading of carpet color all of the above none of the above Question 13. What is the temperature change in 224 g of water upon the absorption of 55 kJ of heat, the specific heat of water is 4.18 J/g C? 59 C 0.059 C 2.9 x 106 C 1.0 x 103 C none of the above Question 14. A cube has a volume of 1 L. What is the length of each side? 10 cm 1.0 m 0.5 m 100 m none of the above Question 15. ________ has oscillates around a fixed point, is spaced close together, and has a definite shape and volume. solid liquid gas plasma none of the above Question 16. Sublimation is the term for: solid becoming a liquid solid becoming a gas liquid becoming a gas gas becoming a solid gas becoming a liquid Question 17. Which of the following is not a compound? carbon monoxide water xylene iron none of the above Question 18. If 25.0 g of calcium carbonate decomposes to 14.0 g of calcium oxide, how many grams of carbon dioxide is produced? 11.0 g 39.0 g 37.3 g not enough information none of the above Question 19. What is the chemical symbol for the ferrous ion? F2- I2+ Fe2+ Fe3+ none of the above Question 20. How many protons, electron, and neutrons are in Cl-35? 17, 17, 20 17, 18, 18 17, 17, 17 17, 17, 18 none of the above Question 21. Who did not propose a model of the atom? John Dalton J. J. Thomson Ernest Rutherford Robert Boyle Niels Bohr Question 22. What is the atomic mass of 6Li, if the atomic mass of lithium is 6.941 amu, and 7Li is 92.58% abundant and weighs 7.015 amu? 6.015 amu 7.420 amu 0.074 amu not enough information none of the above Question 23. How many electrons is a group 2/IIA element likely to lose or gain? lose 2 electrons gain 2 electrons lose 3 electrons gain 1 electron lose 0 electrons Question 24. Molar mass of lead (IV) oxide = 223.2 g/mol 430.4 g/mol 239.2 g/mol 446.4 g/mol none of the above Question 25. How many sodium atoms are in 0.240 moles? 1.44 x 1020 atoms 3.99 x 10-25 atoms 2.51x 103 atoms 1.44 x 1023 atoms none of the above Question 26. Calculate the mass of oxygen in 4.42 x 1021 molecules. 0.118 g 0.235 g 8.80 x 1046 g 0.02295 g 0.459 g Question 27. Which of the following does not exist in nature as a diatomic element? nitrogen oxygen iridium chlorine none of the above Question 28. A hydrocarbon is composed of 85.57% carbon and 14.43% hydrogen and a molar mass of 28.06 g/mol. What is the molecular formula? CH2 CH3 C2H4 C2H2 none of the above Question 29. What is the percent rubidium in rubidium chloride? 0.7068% 70.68% 29.32% 99.99% none of the above Question 30. Which of the following is not evidence of a chemical reaction? permanent color change heat produced or absorbed formation of bubbles all of the above none of the above Question 31. Balance the following reaction: __C4H10 (l) + __O2 (g) ( __CO2 (g) + __H2O (l) 1, 1, 1, 1 1, 13, 4, 5 2, 13, 4, 5 2, 13, 2, 5 none of the above Question 32. Complete and balance the following molecular equation: chloric acid + sodium phosphate ( 3 NaClO3 (aq) + H3PO4 (aq) NaClO3 (aq) + H3PO4 (aq) HClO3 (aq) + Na3PO4 (aq) 3 NaH (aq) + (ClO3)3PO4 (aq) no reaction Question 33. What is the net ionic equation for: HClO4 (aq) + NaOH (aq) ( NaClO4 (aq) + H2O (l) H+(aq) + OH-(aq) ( H2O (l) ClO4-(aq) + Na+(aq) ( NaClO4 (aq) same as above all of the above none of the above Question 34. What are the products of the single replacement reaction: Sr (s) + Pb(NO3) (aq) ( no reaction SrNO3 (aq) + Pb (s) Sr(NO3)2 (aq) + Pb (s) SrPb (s) + NO3 (aq) none of the above Question 35. What evidence would be seen for the reaction of sulfuric acid and calcium solid? formation of a precipitate heat release permanent color change see bubbles no reaction Question 36. Name the term that in a redox reaction is the substance being reduced. oxidizing agent oxidation reducing agent reduction none of the above Question 37. What the oxidation number of the sulfur atom in the sulfate ion? 2 6 +2 +6 none of the above Question 38. How many moles of zinc oxide is produced if 4.44 moles of zinc react with excess oxygen? 2.22 mole 8.88 mole 4.44 mole 4 mole none of the above Question 39. If 25.0 g manganese(IV) oxide reacts with 15.0 g of aluminum, how much manganese metal is produced? MnO2 (l) + Al (l) ( Mn (l) + Al2O3 (s) 15.8 g 22.9 g 38.7 g 30.5 g none of the above Question 40. If 1.25 g of copper(II) nitrate reacts with excess sodium carbonate to produce 0.765 g of copper(II) carbonate, what is the percent yield? Cu(NO3)2 (aq) + Na2CO3 (aq) ( CuCO3 (s) + 2 NaNO3 (aq) 100% 40.3% 108% 93.0% none of the above Question 41. Which type of radiation has the shortest wavelength? x-rays visible light infrared light FM radiowaves eigenrays Question 42. What is the maximum number of electrons in the fourth energy level? 18 6 2 32 10 Question 43. Which subshell has the lowest energy? s p d f g Question 44. Which of the following species is isoelectronic with the argon? Ca+ K+ S- all of the above none of the above Question 45. What is the electron configuration for the mercury(II) ion? [Xe] 6s25d10 4f14 [Xe] 6s25d8 4f14 [Xe] 5d10 4f14 [Xe] 6s25d106p2 4f14 none of the above Question 46. What is the electron configuration for germanium? 1s22s22p63s23p64s23d104p2 1s22s22p63s23p63d104s24p2 1s22s22p63s23p64s24p2 1s22s22p63s23p64s23d104p6 none of the above Question 47. How many valence electrons does a potassium atom have? 19 18 10 6 1 Question 48. Which atom has the largest atomic size? S Sn Ba Kr He Question 49. Which atom has the least metallic character? Kr Ar Ni I Sc Question 50. What is the molecular geometry of carbon tetrafluoride? linear bent trigonal pyramidal tetrahedral none of the above Question 51. What is the electronic geometry of an atom that has 2 double bonds and 0 lone pairs? linear bent trignonal pyramidal tetrahedral none of the above Question 52. Which molecule has a polar covalent bond? NaBr Cl2 HF all of the above none of the above Question 53. Which of the following is true about hydrogen cyanide: linear molecule bent molecule 1 single and 1 double bond 1 single and 1 triple bond a & d Question 54. Which of the following is part of the kinetic molecular theory of gases? move like waves particles are not attracted have inelastic collisions packed closely together all of the above Question 55. How many torr are in 1.00 atm? 760 exactly 760. 1.00 14.7 none of the above Question 56. If a 375 L helium balloon is heated from 15 C to 30 C, what is the new volume, assume constant pressure? 395 L 1.05 x 103 L 750 L 188 L none of the above Question 57. A sample of iodine has a volume of 1.0 L at 0.998 atm and 295K, how grams is in the container? 5.22 g 10.5 g 8.88 g unknown none of the above Question 58. What the partial pressure of oxygen in a container with a total pressure of 755 torr that has 58.6% oxygen? 760 torr 755 torr 442 torr 313 torr none of the above Question 59. Which of the following is a crystalline solid? quartz butter rubber rocks all of the above Question 60. As the surface tension increases, the intermolecular forces ___________. remain the same decrease increase unknown none of the above Question 61. Which of the following has the highest intermolecular forces? argon methanol, CH3OH butane, CH3CH2CH2CH3 ammonia all of the above Question 62. Which compound would have the highest melting point? water sodium chloride propane, C3H8 sugar, C12H22O11 iron Question 63. Which of the following solvents would be immiscible in water. methanol, CH3OH glycerin, C3H5(OH)3 acetic acid, HC2H3O2 none of the above all of the above Question 64. What mass of glucose is needed to have a 55.0% glucose solution in 325.0 g water? 397 g 179 g 266 g 0.00376 g none of the above Question 65. What is the molarity of 2.34 g calcium nitrate in 25.00 mL water? 0.0936 M 0.570 M 0.917 M 9.17 x 10-4M none of the above Question 66. What is the term for an ionic compound that contains a metal or polyatomic cation and a nonmetal or polyatomic anion? salt hydrate anhydrous salt water of hydration none of the above Question 67. A solution is a __________ mixture. heterogeneous homogeneous insoluble saturated none of the above Question 68. What is the term for the component present in the greatest amount in a solution? aqueous solution solvent solute all of the above none of the above Question 69. ____________: when one substance does not dissolve in another. miscible immiscible dilute concentrated none of the above Question 70. What is the mass of sulfuric acid, H2SO4, in 25.0 mL of 12.0 M sulfuric acid? 2.94 x 104 g 29.4 g 47.1 g 4.71 x 104 g none of the above Question 71. If 25.0 mL of 0.150 M aluminum bromide reacts with 15.0 mL of 0.200 M silver nitrate, what mass of silver bromide is produced? _AlBr3 (aq) +_AgNO3 (aq) ( _AgBr (s) + _Al(NO3)3 (aq) 2.11 x 104 g 2.11 g 5.63 x 104 g 0.563 g none of the above Question 72. What is the molarity of aluminum ions in the above question before the reaction has taken place? 0.150 M Al3+ 0.350 M Al3+ 0.107 M Al3+ 0.557 M Al3+ none of the above Question 73. How many moles of ethylene glycol is needed to prepare a 250.0 g of a 0.4500 m solution? 0.1125 moles 1.800 moles 112.5 moles 1.125 x 105 moles none of the above Question 74. Calculate the boiling point of a 0.4500 m solution of ethylene glycol. 100.0000 C 0.2345 C 99.7656 C 100.2345 C none of the above Question 75. What is the term for a substance that accepts protons? Arrhenius acid Arrhenius base Brnstead-Lowry acid Brmstead-Lowry base conjugate acid Question 76. Which of the following is amphoteric? water bicarbonate ion hydrogen sulfate ion all of the above none of the above Question 77. Which of the following reactions will produce water? electrolysis combustion heating a hydrate neutralization all of the above Question 78. A solution is considered basic if [H3O+] _____________ [OH-]. less than greater than equal to 7 none of the above Question 79. What is the pH of a 5.40 x 10-2 M barium hydroxide solution? 1.267 12.732 0.967 13.033 none of the above Question 80. What is the formula a compound of tin(IV) and nitride ions? SnN Sn4N3 Sn12N12 N4Sn3 Sn3N4 Question 81. What is the name for Ag2CO3? silver(I) monocarbonate silver bicarbonate silver carbonate disilver monocarbonate silver(I) carbonate Question 82. What is the name for SO3? sulfur trioxide monosulfur trioxide sulfur oxide disulfur trioxide sulfur(II) oxide Question 83. What is the formula for iron(III) phosphate? Fe2PO4 FePO3 FePO4 Fe3(PO4)3 none of the above Question 84. What is the name for PbSO3? lead sulfate lead(II) sulfate plumbous sulfite lead(IV) sulfite plumbous sulfide Question 85. What is the formula for nickel(II) chloride tetrahydrate? NiClH2O NiCl2 4 H2O NiCl2 5 H2O NiCl2 none of the above Question 86. What is the name for H2C2O4 (aq)? oxalic acid dihydrogen dicarbon tetraoxide oxalous acid hydrogen oxalate hydrogen oxalic acid Question 87. Which of the following is a chemical indicator? litmus paper phenolphthalein congo red all of the above none of the above Question 88. What is the term for reading the meniscus of a liquid above or below eye level? meniscus error student error systematic error parallax error error Question 89. Which of the following is true about a graph? must have a title takes up most of the page axis have labels and units all of the above none of the above Question 90. The y-axis can also be referred to as: abscissa independent variable ordinate Cartesian axis all of the above Question 91. Strong acids, strong bases, and soluble salts are _____ _________. strong electrolytes weak electrolytes non-electrolytes medium electrolytes un-electrolytes Question 92. How will the concentration of the standardized sodium hydroxide solution be affected if deionized water is added to the Erlenmeyer flask? too high too low no change unknown none of the above Question 93. Name the piece of equipment: crucible crucible tongs ring stand clay triangle Question 94. Name the piece of equipment:  crucible crucible tongs deflagrating spoon clay triangle Question 95. Name the piece of equipment a) beaker b) Erlenmeyer flask c) evaporating dish d) crucible Question 96. Name the piece of equipment:  EMBED PBrush  Question 97. Name the piece of equipment:  EMBED PBrush  Question 98. Name the piece of equipment:  Question 99. Name the piece of equipment:  EMBED PBrush  Question 100. 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