Chemistry 105 Practice Test: Answer Key

Chem one hundred five Pract grouchTest 1Note There will not be this many questions on your running game, I just wanted to give you as much give as accomplishable. Also, n whiz of these exact questions will be on the test, just similar questions. Also, make authoritative you gutter do the homework, as I may raise some questions similar to the homework questions.1. Molecules can be described as a. a mix of deuce or more pure plazas. b. a florilegium of two or more elements that has a special(prenominal) symmetry betwixt components. c. two or more fragments chemic altogethery joined unneurotic. d. a inhomogeneous mixture e. a homogeneous mixture attend C2. Daltons Atomic Theory states . that only elements have some(prenominal) isotopes. b. that matter is constitute of small las erectg particles. c. that the properties of matter bumgeic subject 18 cond by the properties of pinchs. d. that energy is incomplete created nor destroyed during a chemic reaction. e. that an atom is predominantly empty space. dish B3. Which of the quest embodys a hypothesis? a. nuclear round 11 reacts with water supply to ca-ca atomic number 11 hydroxide and hydrogen hitman. b. Nitrogen gas is a fairly inert substance. c. Nickel has a capitaly sheen. d. When a substance combusts, it combines with air. e. When wood burns, heat is prone up off. resolution D4. Which is true of a Scientific Theory (circle all that apply) a. It is an interpretation for an comment b. It is a general explanation for the manifestation and doings of all nature c. It can be validated or invalidated by experiment and observation d. It describes why things happen come B, C, and D5. Mass (circle all that apply) a. Is dependent on location (gravity) b. Is the numerate of matter in a substance and remains the self alike(p)(prenominal) regardless of location c. can be measured by using a scale or balance d. is measured in ml respond B and C6. The states of matter be a. inviolable and gas b. Liquid and gas . Gas, solid, and fluidness d. Gas, air, and vapor manage C7. A liquid (circle all that apply) a. Has a definite the great unwashed b. Has particles that are less orderly and can move about freely c. Has particles that are tightly packed d. Has no definite rule book or shape e. solution A and B8. distinguish dry trash as a solid, liquid, or gas. a. solid b. liquid c. gas d. both solid and liquid say A9. When a gas is cooled (circle all that apply) a. Its counterspyecules have few energetic collisions b. The motion of the gas particles go down c. The motion of gas particles increase d. Nothing happens to the gas particles retort A and B10. Classify individually of the interest as a mixture or a pure substance a. Carbon dioxide _____________________ b. profligate ______________________ c. Helium (He) ______________________ d. Sugar water _______________________ serve up A-pure substance B-mixture C-pure substance D-mixture 11. Choose the pure substance from the reheel below. a. sea water b. sugar c. air d. lemonade e. milk assist B12. Choose the varied mixture from the list below. a. Gatorade b. centiliter gas c. black coffee d. chickenhearted noodle soup e. railway one C (graphite) service D13. Which of the pursual avouchments about crystalline and uncrystallized solids is true? a. A crystalline solid is imperturbable of atoms or seawallecules arranged with long-range repeating order. b. An exemplar of a crystalline solid is glass. c. An example of an amorphous solid is table salt (NaCl). d. An amorphous solid is composed of atoms or counterspyecules with a majority of its deal empty. e. either of the above statements are TRUE. serve well A14. A substance that cant be chemically upset(a) down into simpler substances is considered to be a. a homogeneous mixture. b. an element. c. a heterogeneous mixture. d. coalesce. e. an electron. resolving B15. Two or more substances in variable proport ions, where the composition is constant passim are considered a. a compound. b. an element. c. a heterogeneous mixture. d. a homogeneous mixture. e. a crystalline solid. set D16. Which of the spare-time activity are examples of physiologic interchange? a. sugar is dissolved in water. b. coffee is brewed. c. dry ice sublimes. d. ice (solid water) melts. e. All of these are examples of physical change. execute E17. Which of the future(a) are examples of a chemical change? a. coffee brewing b. water boiling c. nails rusting d. alt dissolves in water e. no(prenominal) of the above are chemical changes. dish up C18. Which of the followers represents a physical property? a. Sodium silver element is extremely reactive with chlorine gas. b. Mercury is a smooth liquid at fashion temperature. c. the tendency of aluminum to rust d. the flammability of justane go off e. the unreactive nature of argon gas practise B19. Define thermal energy. a. susceptibility associated with the temperature of an object. b. heartiness associated with the motion of an object. c. Energy associated with the force of an object. d. Energy associated with the gravity of an object. e.Energy associated with the position of an object. dissolving agent A20. Which of the succeeding(a) are examples of intensive properties? a. tightness b. volume c. plenitude d. no(prenominal) of the above are examples of intensive properties. e. All of the above are examples of intensive properties. retort A21. If the temperature is 178F, what is the temperature in degrees celsius? a. 352C b. 451C c. 67C d. 81. 1C e. 378C do D22. If the temperature is 25C, what is the temperature in F? a. 45F b. 298. 15F c. 77F d. -3. 89F serve well C23. If the temperature is 25C, what is the temperature in K? a. 45 K b. 298 K c. 77 K . -3. 89 K Answer B24. set the density of an object that has a kettle of fish of 149. 8 g and displaces 12 . 1 mL of water when placed in a graduated cylinder. a. 8. 08 g/mL b. 1. 38 g/mL c. 12 . 4 g/mL d. 18. 1 g/mL e. 11. 4 g/mL Answer C25. A student per airs an experiment to determine the density of a sugar solution. She obtains the spare-time activity solutions 4. 11 g/mL, 4. 81 g/mL, 4. 95 g/mL, 3. 75 g/mL. If the actual quantify for the density of the sugar solution is 4. 75 g/mL, which statement below best describes her results? a. Her results are precise, but not accurate. b. Her results are accurate, but not precise. . Her results are both precise and accurate d. Her results are uncomplete precise nor accurate. e. It isnt possible to determine with the in strainingation given. Answer D26. Read the water aim with the go down heel of portentous figures. a. 5 mL b. 5. 3 mL c. 5. 32 mL d. 5. 320 mL e. 5. 3 two hundred mL Answer B (Note cogitate, your last of import figure is the one that is uncertain. Because thither are only exclusively number marks, the most certain significant figure is the 5, consequently we estimate where the meniscu s of the liquid is between the 5 and the 6. This is why the better reading is 5. 3, where the 3 is uncertain.If there were marks between the whole numbers, the correct answer would have 3 significant figures, since you could more accurately determine the volume. )27. Read the length of the metal bar with the correct number of significant figures. a. 20 cm b. 15 cm c. 15. 0 cm d. 15. 00 cm e. 15. 000 cm Answer D28. How many significant figures are in 1009. 630 mL? a. 1009. 630 ml _____7______ b. 3. 408 x 104 m _____4_______ c. 0. 0005890 g ______4_______29. Complete the following calculations and cogitation your answer with the correct number of significant figures a. (249. 362 + 41)/63. 498 = ____4. 57________ b. 433. 621 + 0. 02 = ____433. 4_________ c. (965. 43 x 3. 911) + 9413. 4136 = ____1. 319 x 104 or 13190_____30. What wavelength of light would you newspaper publisher in units of nm, if the light had a wavelength of 7. 60 x 10-10 m? a. 7. 60 ? 10-3 nm b. 7. 60 ? 10-19 nm c. 1. 32 nm d. 0. 760 nm e. 760 nm Answer D31. How many cm3 are contained in 3. 77 ? 104 mm3? a. 3. 77 ? 104 cm3 b. 3. 77 ? 101 cm3 c. 3. 77 ? 10-10 cm3 d. 3. 77 ? 1020 cm3 e. 3. 77 ? 106 cm3 f. Answer B32. If a get on requires 25. 4 square yards of carpeting, what is the area of the down in units of ft2? (3 ft = 1 yd) a. 76. 2 ft2 b. 8. 47 ft2 c. 282 ft2 d. 229 ft2 e. 68. 6 ft2 Answer D33. Convert 15. km to miles. (use conversions in the back of your book. These will be given for the test a. 24. 1 miles b. 9. 32 miles c. 591 miles d. 33. 1 miles e. Answer B34. Gas is sold for $1. 399 per liter in Toronto, Canada. Your car needs 12. 00 gallons. How much will your mention card be charged in dollars? ( use conversions in the back of your book. These will be given for the test) a. $16. 79 b. $67. 15 c. $4. 44 d. $63. 54 Answer D35. Crude oil is an example of a. a compound. b. an element. c. a heterogeneous mixture. d. a homogeneous mixture. Answer C 36. NaCl is an example of a. a comp ound. b. an element. c. a heterogeneous mixture. . a homogeneous mixture. Answer A37. A piece of metal ore weighs 8. 25 g. When a student places it into a graduated cylinder containing water, the liquid level rises from 21. 25 mL to 26. 47 mL. What is the density of the ore? a. 0. 312 g/mL b. 0. 633 g/mL c. 1. 58 g/mL d. 3. 21 g/mL Answer C38. A mickle of mercury occupies 0. 950 L. What volume would an disturb atomic reactor of ethanol consume? The density of mercury is and the density of ethanol is 0. 789 g/mL. a. 0. 0553 L b. 0. 0613 L c. 16. 3 L d. 18. 1 L Answer C 39. finish out the following number to four significant figures and express the result in standard exponential notation 229. 13 a. 0. 2296 ? 103 b. 229. 6 c. 2. 296 ? 10-2 d. 2. 296 ? 102 e. 22. 96 ? 10-1 Answer D40. Round off 00907506 to four significant figures. a. 0091 b. 9076 c. 9100 d. 9. 075 ? 105 Answer D41. The diameter of an atom is approximately 1 ? 10-10 m. What is the diameter in millimeters? a. 1 ? 10 -16 mm b. 1 ? 10-13 mm c. 1 ? 10-7 mm d. 1 ? 10-4 mm Answer C42. How many liters of wine can be held in a wine place whose capacity is 26. 0 gal? 1 gal = 4 qt = 3. 7854 L. a. 1. 46 ? 10-4 b. 0. 146 c. 98. 4 d. 6. 87 ? 103 e. 6. 87 Answer C43. 128) How many liters of air are in a room that measures 10. 0 x 11. 0 ft and has an 8. 0 ft ceiling? 1 in. = 2. 54 cm (exactly) 1 L = 103 cm3. a. 2. 49 ? 104 b. 92. 8 c. 26. 8 d. 2. 68 ? 107 e. 8. 84 ? 105 Answer A44. 1) Which of the following is an example of the law of multiple proportions? a. A examine of chlorine is show to contain three times as much Cl-35 as Cl-37. b. Two different compounds organize from carbon and group O have the following jam ratios 1. 33 g O 1 g C and 2. 66 g O 1 g C. c. Two different samples of table salt are found to have the selfsame(p)(prenominal) ratio of sodium to chlorine. d. The nuclear good deal of bromine is found to be 79. 90 amu. e. Nitrogen dioxide always has a mass ratio of 2. 8 g O 1 g N. Answe r B45. Identify the element that has an atomic number of 40. a. neon b. atomic number 20 c. zirconium d. bromine Answer C46. The atomic mass for cadmium is a. 48 b. 112. 41 c. 40. 08 d. 20 Answer B47. The mass number is equal to a. the sum of the sum of the electrons and protons. b. the sum of the sum of the neutrons and electrons. c. the sum of the number of protons, neutrons, and electrons. d. the sum of the number of protons and neutrons. Answer D48. What element is delineate by the following reading? p+ = 11n = 12 e- = 11 a. sodium b. five c. magnesium d. titanium Answer A49. ) What does X represent in the following type? X a. silicon b. sulfur c. zinc d. ruthenium e. nickel Answer A50. 11) Determine the number of protons, neutrons and electrons in the following X a. p+ = 18n = 18e- = 22 b. p+ = 18n = 22e- = 18 c. p+ = 22n = 18e- = 18 d. p+ = 18n = 22e- = 40 e. p+ = 40 n = 22e- = 18 Answer B51. Identify a cation. a. An atom that has muddled an electron. b. An atom that h as gained an electron. c. An atom that has lost a proton. d. An atom that has gained a proton. Answer A52. What element is defined by the following in smorgasbordation? p+ = 17n = 20 e- = 17 a. calcium b. atomic number 37 c. hlorine d. neon e. type O Answer C53. What species is represented by the following information? p+ = 17 n = 18 e- = 18 a. Cl b. Cl- c. Ar d. Ar+ e. Kr f. Answer B54. Give the number of electrons for carbon-14, with a -2 charge . a. 7 b. 4 c. 6 d. 8 Answer D 55. prefigure the charge that an aluminum ion would have. a. 5- b. 1+ c. 1- d. 2+ e. 3+ Answer E56. Predict the charge that the ion formed from bromine would have. a. 1- b. 2+ c. 1+ d. 4+ e. 2- f. Answer A57. Which of the following elements is non a metal? a. Ba b. Mg c. Xe d. Pb e. Ga Answer C58. Which of the following elements is a magisterial gas? a. Ar b. Br c. N d. O e. K Answer A59. Which of the following elements is an alkali metal? a. Zn b. Xe c. F d. Li e. Ca Answer D60. Which of the following sta tements is FALSE? a. Anions are unremarkably larger than their corresponding atom. b. Metals tend to form cations c. Atoms are unremarkably larger than their corresponding cation. d. The halogens tend to form 1+ ions. e. Nonmetals tend to gain electrons. Answer D61. Which of the following does NOT describe a nonmetal? a. Tend to gain electrons b. Found in the upper pay off hand corner of the weekly table. c. deplorable manager of electricity d. Nonmetals are generally unreactive. e. Poor conductor of heat. Answer D62. Silver has an atomic mass of 107. 868 amu. The Ag-109 isotope (108. 905 amu) is 48. 16%. What is the amu of the other isotope? a. 106. 905 amu b. 106. 908 amu c. 106. 903 amu d. D) 106. 911 amu Answer A63. Which of the following contains the MOST atoms? You shouldnt need to do a calculation here. a. 10. 0 g Ne b. 10. 0 g He c. 10. 0 g Ar d. 10. 0 g Kr e. 10. 0 g Mg Answer B64. How many ash grey atoms are contained in 3. 75 seawalles of silver? a. 6. 23 ? 1024 s ilver atoms b. 2. 26 ? 1024 silver atoms c. 1. 61 ? 1023 silver atoms d. 2. 44 ? 1026 silver atoms e. 6. 50 ? 1025 silver atoms Answer B65. How many moles of potassium are contained in 449 g of potassium? a. 11. 5 moles b. 17. 6 moles c. 69. 2 moles d. 23. 9 moles e. 41. 5 moles Answer A66. What mass, in kg, does 5. 84 moles of titanium (Ti) have? a. 0. 352 kg b. 0. 122 kg c. 0. 820 kg d. 0. 280 kg e. 0. 632 kg Answer D67. How many moles of Cs are contained in 595 kg of Cs? a. 2. 23 ? 102 moles Cs b. 4. 48 ? 103 moles Cs c. 7. 91 ? 104 moles Cs d. 1. 26 ? 103 moles Cs e. 5. 39 ? 102 moles Cs Answer B68. How many smoothing urge on atoms are contained in 354 g of iron? a. 2. 62 ? 1025 Fe atoms b. 2. 13 ? 1026 Fe atoms c. 4. 69 ? 1024 Fe atoms d. 3. 82 ? 1024 Fe atoms . 9. 50 ? 1022 Fe atoms Answer D69. compute the mass, in kg, of 4. 87 x 1025 atoms of Zn. a. 5. 29 kg b. 1. 89 kg c. 8. 09 kg d. 1. 24 kg e. 1. 09 kg Answer A Match the following. A) Fe B) C C) Mg D) Si E) K 70. magnes ium 71. carbon 72. potassium 73. iron 74. silicon Answers70) C71) B72) E73) A74) D75. Give the differentiate of the element whose symbol is Na. Answer sodium76. An atom of 131Xe contains ________ electrons. a. 131 b. 185 c. 77 d. 123 e. 54 Answer E77. An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is ________. a. 17O2- b. 17O2+ c. 19F+ d. 19F- e. 17Ne2+ Answer A78. How many protons does the Br- ion possess? a. 34 b. 36 c. 6 d. 8 e. 35 Answer E79. Predict the charge of the most constant ion of potassium. a. 3+ b. 1- c. 2+ d. 2- e. 1+ Answer E80. What is the chemical symbol for mercury? a. Ag b. Au c. Hg d. Pb Answer C81. Which are isotopes? An atom that has an atomic number of 20 and a mass number of 42 is an isotope of an atom that has a. an atomic number of 21 and a mass number of 42. b. an atomic number of 20 and a mass number of 40. c. 22 neutrons and 20 protons. d. 22 protons and 20 neutrons. Answer B82. How many protons (p) and neutrons (n) are in an atom of Sr? a. 38 p, 52 n . 38 p, 90 n c. 52 p, 38 n d. 90 p, 38 n Answer A83. The mass number of an atom of 128Xe is ________. a. 54 b. 182 c. 74 d. 128 e. 120 Answer D84. What is the individuation of element Q if the ion Q2+ contains 10 electrons? a. C b. O c. Ne d. Mg Answer D85. In which of the following sets do all species have the same number of electrons? a. F-, Ne, Mg2+ b. Ge, Se2-, Br- c. K+, Rb+, Cs+ d. Br, Br-, Br+ Answer A86. Argon belongs to the ________ group of the periodic table. a. alkali metal b. alkaline earth metal c. halogen d. noble gas Answer D87. Which of the following elements has chemical properties similar to tellurium? . fluorine b. hydrogen c. atomic number 7 d. sulfur Answer D88. An bean bond is best described as a. the sharing of electrons. b. the broadcast of electrons from one atom to another. c. the attraction that holds the atoms together in a polyatomic ion. d. the attraction between 2 nonmetal atoms. e. the attraction between 2 metal atoms . Answer B89. What is the empirical manifestation for C4H10O2? a. C2H5O b. CHO c. C2H4O d. CHO2 e. Cwater system Answer A90. draw up a possible molecular enactment for C4H4O. a. C8H8O2 b. C12H12O2 c. C2H2O d. C8H8O Answer A91. Which of the following is an atomic element? a. Br b. H c. N d. O e. Mg Answer E92. Which of the following is a molecular element? a. Kr b. Ag c. S d. Mg e. Ti Answer C93. Which of the following is a molecular compound? a. CuCl2 b. KCl c. NaNO3 d. CH3Cl e. RbBr f. Answer D94. Which of the following is an ionic compound? a. SCl2 b. Mg3(PO4)2 c. Cl2O d. CH2O e. PF5 Answer B95. Write the traffic pattern for the compound formed between potassium and sulfur. a. KS b. KS2 c. K2S d. K2SO3 e. K3S2 Answer C96. Give the name for SnO. a. tin (I) oxide b. tin (II) oxide c. tin (III) oxide d. tin (IV) oxide Answer B97. Write the formula for strontium nitride. a. Sr3N2 b. Sr(NO3)2 c. SrN d. Sr2N3 e. Sr(NO2)2 Answer A98. Write the name for Sn(SO4)2. Remember that Sn form s several ions. a. tin (I) sulfite b. tin (IV) sulphate c. tin sulfide d. tin (II) sulfite e. tin (I) sulfate Answer B99. Determine the name for CoCl26H2O. Remember that Co forms several ions. a. cobalt chloride hydrate b. cobalt (I) chloride heptahydrate c. cobalt (II) chloride heptahydrate d. cobalt (II) chloride hexahydrate e. cobalt (I) chloride Answer D100. Write the formula for copper (II) sulfate pentahydrate. a. Cu2SO3H5 b. Cu2SH2O c. CuS5H2O d. (CuSO4)5 e. CuSO45H2O Answer E101. Determine the name for H2CO3. a. carbonous loony toons b. dihydrogen carbonate c. carbonic sharp . hydrocarbonic acid e. hydrocarbide acid Answer C102. Identify the formula for nitrous acid. a. HNO3 b. HNO2 c. HNO d. HNO4 Answer A103. Determine the name for P4O10. a. phosphorus (IV) oxide b. diphosphorus pentoxide c. phosphorus oxide d. phosphorus (II) oxide e. tetraphosphorus decoxide Answer E104. place the poor boy mass for Mg(ClO4)2. a. 223. 21 g/mol b. 123. 76 g/mol c. 119. 52 g/mol d. 24 7. 52 g/mol e. 75. 76 g/mol Answer A105. Calculate the molar mass of Al(C2H3O2)3. a. 86. 03 g/mol b. 204. 13 g/mol c. 56. 00 g/mol d. 258. 09 g/mol e. 139. 99 g/mol Answer B106. How many millimoles of Ca(NO3)2 contain 4. 8 ? 1022 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164. 10 g/mol. a. 12. 6 mmol Ca(NO3)2 b. 13. 0 mmol Ca(NO3)2 c. 20. 7 mmol Ca(NO3)2 d. 79. 4 mmol Ca(NO3)2 e. 57. 0 mmol Ca(NO3)2 Answer D107. How many C2H4 molecules are contained in 45. 8 mg of C2H4? The molar mass of C2H4 is 28. 05 g/mol. a. 9. 83 ? 1020 C2H4 molecules b. 7. 74 ? 1026 C2H4 molecules c. 2. 71 ? 1020 C2H4 molecules d. 3. 69 ? 1023 C2H4 molecules e. 4. 69 ? 1023 C2H4 molecules Answer A108. What is the mass of 9. 44 ? 1024 molecules of NO2? The molar mass of NO2 is 46. 01 g/mol. a. 205 g b. 294 g c. 721 g d. 341 g e. 685 g Answer C109. Calculate the mass percent composition of sulfur in Al2(SO4)3. a. 28. 12 % b. 9. 372 % c. 42. 73 % d. 21. 38 % e. 35. 97 % Answer A110. How many moles o f N2O3 contain 2. 55 ? 1024 oxygen atoms? (change the molecule) a. 1. 41 moles N2O3 b. 4. 23 moles N2O3 c. 12. 7 moles N2O3 d. 7. 87 moles N2O3 e. 2. 82 moles N2O3 Answer A111. How many moles of PCl3 contain 3. 68 ? 1025 chlorine atoms? a. 61. 1 moles PCl3 b. 20. 4 moles PCl3 c. 16. 4 moles PCl3 d. 54. 5 moles PCl3 e. 49. 1 moles PCl3 Answer B112. How many sodium ions are contained in 99. 6 mg of Na2SO3? The molar mass of Na2SO3 is 126. 05 g/mol. a. 1. 52 ? 1027 sodium ions . 4. 76 ? 1020 sodium ions c. 2. 10 ? 1021 sodium ions d. 1. 05 ? 1021 sodium ions e. 9. 52 ? 1020 sodium ions Answer E113. Determine the volume of hexane that contains 5. 33 ? 1022 molecules of hexane. The density of hexane is 0. 6548 g/mL and its molar mass is 86. 17 g/mol. a. 8. 59 mL b. 13. 5 mL c. 7. 40 mL d. 12. 4 mL e. 11. 6 mL Answer E114. Determine the molecular formula of a compound that has a molar mass of 92. 0 g/mol and an empirical formula of NO2. a. N2O3 b. N3O6 c. N2O4 d. NO2 e. N2O5 Answer C115. Determine the empirical formula for a compound that is 36. 86% N and 63. 14% O by mass. a. NO b. N2O c. NO2 d.N2O3 e. NO3 Answer D116. Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor. a. 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) b. C2H6(g) + 5 O(g) 2 CO(g) + 3 H2O(g) c. 2 C2H6(g) + 5 O2(g) 4 CO(g) + 6 H2O(g) d. C2H6(g) + 7 O(g) 2 CO2(g) + 3 H2O(g) e. 2 CH3(g) + 5 O(g) 2 CO(g) + 3 H2O(g) Answer C117. Which of the following is one possible form of pentane? a. CH3CH2CH2CH2CH3 b. CH3CH=CHCH2CH3 c. CH3CH2CH2CH2CH2CH3 d. CH3CH2CH2CH2CH2NH2 e. CH3CH2-O-CH2CH2CH3 Answer A118. List the elements in a hydrocarbon Answer hydrogen and carbon119. What type of bind is found in the compound OF2? a. covalent bonding b. hydrogen bonding c. ionic bonding d. metallic bonding Answer A120. In which set do all elements tend to form cations in binary ionic compounds? a. K, Ga, O b. Sr, Ni, Hg c. N, P, Bi d. O, Br, I Answe r B121. Rb2S is named a. rubidium disulfide. b. rubidium sulfide. c. rubidium(II) sulfide. d. rubidium sulfur. Answer B122. An aqueous solution of H2S is named a. hydrosulfuric acid. b. hydrosulfurous acid. c. sulfuric acid. d. sulfurous acid. Answer A123. What is the molar mass of nitrogen gas? a. 14. 0 g/mol b. 28. 0 g/mol c. 6. 02 ? 1023 g/mol d. 1. 20 ? 023 g/mol Answer B124. What mass of carbon dioxide, C O2, contains the same number of molecules as 3. 00 g of trichlorofluoromethane, CCl3F? a. 0. 106 g b. 0. 961 g c. 1. 04 g d. 9. 37 g e. Answer B125. Which of the following has the greatest mass? a. 3. 88 ? 1022 molecules of O2 b. 1. 00 g of O2 c. 0. 0312 mol of O2 d. All of the above have the same mass. Answer A126. A sample of pure calcium fluoride with a mass of 15. 0 g contains 7. 70 g of calcium. How much calcium is contained in 40. 0 g of calcium fluoride? a. 2. 27 g b. 7. 70 g c. 15. 0 g d. 20. 5 g Answer D127. What is the empirical formula of a compound that is 62. % C , 10. 4% H, and 27. 5% O by mass? a. C3HO b. C6HO3 c. C6H12O2 d. C5H10O2 e. C3H6O Answer E128. How many oxygen atoms are there in 7. 00 g of sodium dichromate, Na2Cr2O7? a. 0. 187 oxygen atoms b. 2. 30 ? 1021 oxygen atoms c. 1. 60 ? 1022 oxygen atoms d. 1. 13 ? 1023 oxygen atoms Answer D129. Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 0. 80 g of methane reacts with 3. 2 g of oxygen to produce 2. 2 g of carbon dioxide? a. 1. 8 g b. 2. 2 g c. 3. 7 g d. 4. 0 g Answer A130. Combustion analysis of 1. 200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2. 86 g of CO2 and 1. 134 g of H2O. What is the empirical formula of the compound? a. C2H5O b. C2H5O2 c. C2H10O3 d. C3H8O2 Answer D131. What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? _____ C2H6O (l) + _____ O2(g) _____ CO2(g) + _____ H2O(l) a. 9 b. 7 c. 5 d. 3 Answer D132. atomic number 20 phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered coefficients? a. 1 b. 2 c. 3 d. none of these Answer CChemistry 105 Practice Test Answer recognizeChem 105 PracticeTest 1Note There will not be this many questions on your test, I just wanted to give you as much practice as possible. Also, none of these exact questions will be on the test, just similar questions. Also, make sure you can do the homework, as I may have some questions similar to the homework questions.1. Molecules can be described as a. a mixture of two or more pure substances. b. a mixture of two or more elements that has a specific ratio between components. c. two or more atoms chemically joined together. d. a heterogeneous mixture e. a homogeneous mixture Answer C2. Daltons Atomic Theory states . that all elements have several isotopes. b. that matter is composed of small indestructible particles. c. that the properties of matter are determined by the properties of atoms. d. that energy is neither created nor destroyed during a chemical reaction. e. that an atom is predominantly empty space. Answer B3. Which of the following represents a hypothesis? a. Sodium reacts with water to form sodium hydroxide and hydrogen gas. b. Nitrogen gas is a fairly inert substance. c. Nickel has a silvery sheen. d. When a substance combusts, it combines with air. e. When wood burns, heat is given off. Answer D4. Which is true of a Scientific Theory (circle all that apply) a. It is an interpretation for an observation b. It is a general explanation for the manifestation and behavior of all nature c. It can be validated or invalidated by experiment and observation d. It describes why things happen Answer B, C, and D5. Mass (circle all that apply) a. Is dependent on location (gravity) b. Is the amount of matter in a substance and remains the same regardless of location c. can be measured by using a scale or balance d. is measured in ml Answer B and C6. The states of matter are a. Solid and gas b. Liquid and gas . Gas, solid, and liquid d. Gas, air, and vapor Answer C7. A liquid (circle all that apply) a. Has a definite volume b. Has particles that are less orderly and can move about freely c. Has particles that are tightly packed d. Has no definite volume or shape e. Answer A and B8. Identify dry ice as a solid, liquid, or gas. a. solid b. liquid c. gas d. both solid and liquid Answer A9. When a gas is cooled (circle all that apply) a. Its molecules have fewer energetic collisions b. The motion of the gas particles decrease c. The motion of gas particles increase d. Nothing happens to the gas particlesAnswer A and B10. Classify each of the following as a mixture or a pure substance a. Carbon dioxide _____________________ b. Blood ______________________ c. Helium (He) ______________________ d. Sugar water _______________________ Answer A-pure substan ce B-mixture C-pure substance D-mixture 11. Choose the pure substance from the list below. a. sea water b. sugar c. air d. lemonade e. milk Answer B12. Choose the heterogeneous mixture from the list below. a. Gatorade b. chlorine gas c. black coffee d. chicken noodle soup e. carbon (graphite) Answer D13. Which of the following statements about crystalline and amorphous solids is TRUE? a. A crystalline solid is composed of atoms or molecules arranged with long-range repeating order. b. An example of a crystalline solid is glass. c. An example of an amorphous solid is table salt (NaCl). d. An amorphous solid is composed of atoms or molecules with a majority of its volume empty. e. All of the above statements are TRUE. Answer A14. A substance that cant be chemically broken down into simpler substances is considered to be a. a homogeneous mixture. b. an element. c. a heterogeneous mixture. d. compound. e. an electron. Answer B15. Two or more substances in variable proportions, where the composition is constant throughout are considered a. a compound. b. an element. c. a heterogeneous mixture. d. a homogeneous mixture. e. a crystalline solid. Answer D16. Which of the following are examples of physical change? a. sugar is dissolved in water. b. coffee is brewed. c. dry ice sublimes. d. ice (solid water) melts. e. All of these are examples of physical change. Answer E17. Which of the following are examples of a chemical change? a. coffee brewing b. water boiling c. nails rusting d. alt dissolves in water e. None of the above are chemical changes. Answer C18. Which of the following represents a physical property? a. Sodium metal is extremely reactive with chlorine gas. b. Mercury is a silver liquid at room temperature. c. the tendency of aluminum to rust d. the flammability of butane fuel e. the unreactive nature of argon gas Answer B19. Define thermal energy. a. Energy associated with the temperature of an object. b. Energy associated with the motion of an object. c. Energy associated with the force of an object. d. Energy associated with the gravity of an object. e.Energy associated with the position of an object. Answer A20. Which of the following are examples of intensive properties? a. density b. volume c. mass d. None of the above are examples of intensive properties. e. All of the above are examples of intensive properties. Answer A21. If the temperature is 178F, what is the temperature in degrees celsius? a. 352C b. 451C c. 67C d. 81. 1C e. 378C Answer D22. If the temperature is 25C, what is the temperature in F? a. 45F b. 298. 15F c. 77F d. -3. 89F Answer C23. If the temperature is 25C, what is the temperature in K? a. 45 K b. 298 K c. 77 K . -3. 89 K Answer B24. Determine the density of an object that has a mass of 149. 8 g and displaces 12 . 1 mL of water when placed in a graduated cylinder. a. 8. 08 g/mL b. 1. 38 g/mL c. 12 . 4 g/mL d. 18. 1 g/mL e. 11. 4 g/mL Answer C25. A student performs an experiment to determine the density of a sugar solution. She obtains the following results 4. 11 g/mL, 4. 81 g/mL, 4. 95 g/mL, 3. 75 g/mL. If the actual value for the density of the sugar solution is 4. 75 g/mL, which statement below best describes her results? a. Her results are precise, but not accurate. b. Her results are accurate, but not precise. . Her results are both precise and accurate d. Her results are neither precise nor accurate. e. It isnt possible to determine with the information given. Answer D26. Read the water level with the correct number of significant figures. a. 5 mL b. 5. 3 mL c. 5. 32 mL d. 5. 320 mL e. 5. 3200 mL Answer B (Note Remember, your last significant figure is the one that is uncertain. Because there are only whole number marks, the most certain significant figure is the 5, then we estimate where the meniscus of the liquid is between the 5 and the 6. This is why the correct reading is 5. 3, where the 3 is uncertain.If there were marks between the whole numbers, the correct answer would h ave 3 significant figures, since you could more accurately determine the volume. )27. Read the length of the metal bar with the correct number of significant figures. a. 20 cm b. 15 cm c. 15. 0 cm d. 15. 00 cm e. 15. 000 cm Answer D28. How many significant figures are in 1009. 630 mL? a. 1009. 630 ml _____7______ b. 3. 408 x 104 m _____4_______ c. 0. 0005890 g ______4_______29. Complete the following calculations and report your answer with the correct number of significant figures a. (249. 362 + 41)/63. 498 = ____4. 57________ b. 433. 621 + 0. 02 = ____433. 4_________ c. (965. 43 x 3. 911) + 9413. 4136 = ____1. 319 x 104 or 13190_____30. What wavelength of light would you report in units of nm, if the light had a wavelength of 7. 60 x 10-10 m? a. 7. 60 ? 10-3 nm b. 7. 60 ? 10-19 nm c. 1. 32 nm d. 0. 760 nm e. 760 nm Answer D31. How many cm3 are contained in 3. 77 ? 104 mm3? a. 3. 77 ? 104 cm3 b. 3. 77 ? 101 cm3 c. 3. 77 ? 10-10 cm3 d. 3. 77 ? 1020 cm3 e. 3. 77 ? 106 cm3 f. Answer B 32. If a room requires 25. 4 square yards of carpeting, what is the area of the floor in units of ft2? (3 ft = 1 yd) a. 76. 2 ft2 b. 8. 47 ft2 c. 282 ft2 d. 229 ft2 e. 68. 6 ft2 Answer D33. Convert 15. km to miles. (use conversions in the back of your book. These will be given for the test a. 24. 1 miles b. 9. 32 miles c. 591 miles d. 33. 1 miles e. Answer B34. Gas is sold for $1. 399 per liter in Toronto, Canada. Your car needs 12. 00 gallons. How much will your credit card be charged in dollars? ( use conversions in the back of your book. These will be given for the test) a. $16. 79 b. $67. 15 c. $4. 44 d. $63. 54 Answer D35. Crude oil is an example of a. a compound. b. an element. c. a heterogeneous mixture. d. a homogeneous mixture. Answer C 36. NaCl is an example of a. a compound. b. an element. c. a heterogeneous mixture. . a homogeneous mixture. Answer A37. A piece of metal ore weighs 8. 25 g. When a student places it into a graduated cylinder containing water, the liquid lev el rises from 21. 25 mL to 26. 47 mL. What is the density of the ore? a. 0. 312 g/mL b. 0. 633 g/mL c. 1. 58 g/mL d. 3. 21 g/mL Answer C38. A mass of mercury occupies 0. 950 L. What volume would an equal mass of ethanol occupy? The density of mercury is and the density of ethanol is 0. 789 g/mL. a. 0. 0553 L b. 0. 0613 L c. 16. 3 L d. 18. 1 L Answer C 39. Round the following number to four significant figures and express the result in standard exponential notation 229. 13 a. 0. 2296 ? 103 b. 229. 6 c. 2. 296 ? 10-2 d. 2. 296 ? 102 e. 22. 96 ? 10-1 Answer D40. Round off 00907506 to four significant figures. a. 0091 b. 9076 c. 9100 d. 9. 075 ? 105 Answer D41. The diameter of an atom is approximately 1 ? 10-10 m. What is the diameter in millimeters? a. 1 ? 10-16 mm b. 1 ? 10-13 mm c. 1 ? 10-7 mm d. 1 ? 10-4 mm Answer C42. How many liters of wine can be held in a wine barrel whose capacity is 26. 0 gal? 1 gal = 4 qt = 3. 7854 L. a. 1. 46 ? 10-4 b. 0. 146 c. 98. 4 d. 6. 87 ? 103 e. 6. 87 Answer C43. 128) How many liters of air are in a room that measures 10. 0 x 11. 0 ft and has an 8. 0 ft ceiling? 1 in. = 2. 54 cm (exactly) 1 L = 103 cm3. a. 2. 49 ? 104 b. 92. 8 c. 26. 8 d. 2. 68 ? 107 e. 8. 84 ? 105 Answer A44. 1) Which of the following is an example of the law of multiple proportions? a. A sample of chlorine is found to contain three times as much Cl-35 as Cl-37. b. Two different compounds formed from carbon and oxygen have the following mass ratios 1. 33 g O 1 g C and 2. 66 g O 1 g C. c. Two different samples of table salt are found to have the same ratio of sodium to chlorine. d. The atomic mass of bromine is found to be 79. 90 amu. e. Nitrogen dioxide always has a mass ratio of 2. 8 g O 1 g N. Answer B45. Identify the element that has an atomic number of 40. a. neon b. calcium c. zirconium d. bromine Answer C46. The atomic mass for cadmium is a. 48 b. 112. 41 c. 40. 08 d. 20 Answer B47. The mass number is equal to a. the sum of the sum of the electrons and pr otons. b. the sum of the sum of the neutrons and electrons. c. the sum of the number of protons, neutrons, and electrons. d. the sum of the number of protons and neutrons. Answer D48. What element is defined by the following information? p+ = 11n = 12 e- = 11 a. sodium b. vanadium c. magnesium d. titanium Answer A49. ) What does X represent in the following symbol? X a. silicon b. sulfur c. zinc d. ruthenium e. nickel Answer A50. 11) Determine the number of protons, neutrons and electrons in the following X a. p+ = 18n = 18e- = 22 b. p+ = 18n = 22e- = 18 c. p+ = 22n = 18e- = 18 d. p+ = 18n = 22e- = 40 e. p+ = 40 n = 22e- = 18 Answer B51. Identify a cation. a. An atom that has lost an electron. b. An atom that has gained an electron. c. An atom that has lost a proton. d. An atom that has gained a proton. Answer A52. What element is defined by the following information? p+ = 17n = 20 e- = 17 a. calcium b. rubidium c. hlorine d. neon e. oxygen Answer C53. What species is represented by the following information? p+ = 17 n = 18 e- = 18 a. Cl b. Cl- c. Ar d. Ar+ e. Kr f. Answer B54. Give the number of electrons for carbon-14, with a -2 charge . a. 7 b. 4 c. 6 d. 8 Answer D 55. Predict the charge that an aluminum ion would have. a. 5- b. 1+ c. 1- d. 2+ e. 3+ Answer E56. Predict the charge that the ion formed from bromine would have. a. 1- b. 2+ c. 1+ d. 4+ e. 2- f. Answer A57. Which of the following elements is NOT a metal? a. Ba b. Mg c. Xe d. Pb e. Ga Answer C58. Which of the following elements is a noble gas? a. Ar b. Br c. N d. O e. K Answer A59. Which of the following elements is an alkali metal? a. Zn b. Xe c. F d. Li e. Ca Answer D60. Which of the following statements is FALSE? a. Anions are usually larger than their corresponding atom. b. Metals tend to form cations c. Atoms are usually larger than their corresponding cation. d. The halogens tend to form 1+ ions. e. Nonmetals tend to gain electrons. Answer D61. Which of the following does NOT describe a nonm etal? a. Tend to gain electrons b. Found in the upper right hand corner of the periodic table. c. Poor conductor of electricity d. Nonmetals are generally unreactive. e. Poor conductor of heat. Answer D62. Silver has an atomic mass of 107. 868 amu. The Ag-109 isotope (108. 905 amu) is 48. 16%. What is the amu of the other isotope? a. 106. 905 amu b. 106. 908 amu c. 106. 903 amu d. D) 106. 911 amu Answer A63. Which of the following contains the MOST atoms? You shouldnt need to do a calculation here. a. 10. 0 g Ne b. 10. 0 g He c. 10. 0 g Ar d. 10. 0 g Kr e. 10. 0 g Mg Answer B64. How many silver atoms are contained in 3. 75 moles of silver? a. 6. 23 ? 1024 silver atoms b. 2. 26 ? 1024 silver atoms c. 1. 61 ? 1023 silver atoms d. 2. 44 ? 1026 silver atoms e. 6. 50 ? 1025 silver atoms Answer B65. How many moles of potassium are contained in 449 g of potassium? a. 11. 5 moles b. 17. 6 moles c. 69. 2 moles d. 23. 9 moles e. 41. 5 moles Answer A66. What mass, in kg, does 5. 84 moles of ti tanium (Ti) have? a. 0. 352 kg b. 0. 122 kg c. 0. 820 kg d. 0. 280 kg e. 0. 632 kg Answer D67. How many moles of Cs are contained in 595 kg of Cs? a. 2. 23 ? 102 moles Cs b. 4. 48 ? 103 moles Cs c. 7. 91 ? 104 moles Cs d. 1. 26 ? 103 moles Cs e. 5. 39 ? 102 moles Cs Answer B68. How many iron atoms are contained in 354 g of iron? a. 2. 62 ? 1025 Fe atoms b. 2. 13 ? 1026 Fe atoms c. 4. 69 ? 1024 Fe atoms d. 3. 82 ? 1024 Fe atoms . 9. 50 ? 1022 Fe atoms Answer D69. Calculate the mass, in kg, of 4. 87 x 1025 atoms of Zn. a. 5. 29 kg b. 1. 89 kg c. 8. 09 kg d. 1. 24 kg e. 1. 09 kg Answer A Match the following. A) Fe B) C C) Mg D) Si E) K 70. magnesium 71. carbon 72. potassium 73. iron 74. silicon Answers70) C71) B72) E73) A74) D75. Give the name of the element whose symbol is Na. Answer sodium76. An atom of 131Xe contains ________ electrons. a. 131 b. 185 c. 77 d. 123 e. 54 Answer E77. An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is ________. a. 17O2- b. 17O 2+ c. 19F+ d. 19F- e. 17Ne2+ Answer A78. How many protons does the Br- ion possess? a. 34 b. 36 c. 6 d. 8 e. 35 Answer E79. Predict the charge of the most stable ion of potassium. a. 3+ b. 1- c. 2+ d. 2- e. 1+ Answer E80. What is the chemical symbol for mercury? a. Ag b. Au c. Hg d. Pb Answer C81. Which are isotopes? An atom that has an atomic number of 20 and a mass number of 42 is an isotope of an atom that has a. an atomic number of 21 and a mass number of 42. b. an atomic number of 20 and a mass number of 40. c. 22 neutrons and 20 protons. d. 22 protons and 20 neutrons. Answer B82. How many protons (p) and neutrons (n) are in an atom of Sr? a. 38 p, 52 n . 38 p, 90 n c. 52 p, 38 n d. 90 p, 38 n Answer A83. The mass number of an atom of 128Xe is ________. a. 54 b. 182 c. 74 d. 128 e. 120 Answer D84. What is the identity of element Q if the ion Q2+ contains 10 electrons? a. C b. O c. Ne d. Mg Answer D85. In which of the following sets do all species have the same number of electro ns? a. F-, Ne, Mg2+ b. Ge, Se2-, Br- c. K+, Rb+, Cs+ d. Br, Br-, Br+ Answer A86. Argon belongs to the ________ group of the periodic table. a. alkali metal b. alkaline earth metal c. halogen d. noble gas Answer D87. Which of the following elements has chemical properties similar to tellurium? . fluorine b. hydrogen c. nitrogen d. sulfur Answer D88. An ionic bond is best described as a. the sharing of electrons. b. the transfer of electrons from one atom to another. c. the attraction that holds the atoms together in a polyatomic ion. d. the attraction between 2 nonmetal atoms. e. the attraction between 2 metal atoms. Answer B89. What is the empirical formula for C4H10O2? a. C2H5O b. CHO c. C2H4O d. CHO2 e. CH2O Answer A90. Write a possible molecular formula for C4H4O. a. C8H8O2 b. C12H12O2 c. C2H2O d. C8H8O Answer A91. Which of the following is an atomic element? a. Br b. H c. N d. O e. Mg Answer E92. Which of the following is a molecular element? a. Kr b. Ag c. S d. Mg e. Ti Answer C93. Which of the following is a molecular compound? a. CuCl2 b. KCl c. NaNO3 d. CH3Cl e. RbBr f. Answer D94. Which of the following is an ionic compound? a. SCl2 b. Mg3(PO4)2 c. Cl2O d. CH2O e. PF5 Answer B95. Write the formula for the compound formed between potassium and sulfur. a. KS b. KS2 c. K2S d. K2SO3 e. K3S2 Answer C96. Give the name for SnO. a. tin (I) oxide b. tin (II) oxide c. tin (III) oxide d. tin (IV) oxide Answer B97. Write the formula for strontium nitride. a. Sr3N2 b. Sr(NO3)2 c. SrN d. Sr2N3 e. Sr(NO2)2 Answer A98. Write the name for Sn(SO4)2. Remember that Sn forms several ions. a. tin (I) sulfite b. tin (IV) sulfate c. tin sulfide d. tin (II) sulfite e. tin (I) sulfate Answer B99. Determine the name for CoCl26H2O. Remember that Co forms several ions. a. cobalt chloride hydrate b. cobalt (I) chloride heptahydrate c. cobalt (II) chloride heptahydrate d. cobalt (II) chloride hexahydrate e. cobalt (I) chloride Answer D100. Write the formula for copper (II) sulfate pentahydrate. a. Cu2SO3H5 b. Cu2SH2O c. CuS5H2O d. (CuSO4)5 e. CuSO45H2O Answer E101. Determine the name for H2CO3. a. carbonous acid b. dihydrogen carbonate c. carbonic acid . hydrocarbonic acid e. hydrocarbide acid Answer C102. Identify the formula for nitric acid. a. HNO3 b. HNO2 c. HNO d. HNO4 Answer A103. Determine the name for P4O10. a. phosphorus (IV) oxide b. diphosphorus pentoxide c. phosphorus oxide d. phosphorus (II) oxide e. tetraphosphorus decoxide Answer E104. Calculate the molar mass for Mg(ClO4)2. a. 223. 21 g/mol b. 123. 76 g/mol c. 119. 52 g/mol d. 247. 52 g/mol e. 75. 76 g/mol Answer A105. Calculate the molar mass of Al(C2H3O2)3. a. 86. 03 g/mol b. 204. 13 g/mol c. 56. 00 g/mol d. 258. 09 g/mol e. 139. 99 g/mol Answer B106. How many millimoles of Ca(NO3)2 contain 4. 8 ? 1022 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164. 10 g/mol. a. 12. 6 mmol Ca(NO3)2 b. 13. 0 mmol Ca(NO3)2 c. 20. 7 mmol Ca(NO3)2 d. 79. 4 mmol Ca(NO3)2 e. 57. 0 mmol Ca(NO3)2 Answe r D107. How many C2H4 molecules are contained in 45. 8 mg of C2H4? The molar mass of C2H4 is 28. 05 g/mol. a. 9. 83 ? 1020 C2H4 molecules b. 7. 74 ? 1026 C2H4 molecules c. 2. 71 ? 1020 C2H4 molecules d. 3. 69 ? 1023 C2H4 molecules e. 4. 69 ? 1023 C2H4 molecules Answer A108. What is the mass of 9. 44 ? 1024 molecules of NO2? The molar mass of NO2 is 46. 01 g/mol. a. 205 g b. 294 g c. 721 g d. 341 g e. 685 g Answer C109. Calculate the mass percent composition of sulfur in Al2(SO4)3. a. 28. 12 % b. 9. 372 % c. 42. 73 % d. 21. 38 % e. 35. 97 % Answer A110. How many moles of N2O3 contain 2. 55 ? 1024 oxygen atoms? (change the molecule) a. 1. 41 moles N2O3 b. 4. 23 moles N2O3 c. 12. 7 moles N2O3 d. 7. 87 moles N2O3 e. 2. 82 moles N2O3 Answer A111. How many moles of PCl3 contain 3. 68 ? 1025 chlorine atoms? a. 61. 1 moles PCl3 b. 20. 4 moles PCl3 c. 16. 4 moles PCl3 d. 54. 5 moles PCl3 e. 49. 1 moles PCl3 Answer B112. How many sodium ions are contained in 99. 6 mg of Na2SO3? The molar mass of Na2SO3 is 126. 05 g/mol. a. 1. 52 ? 1027 sodium ions . 4. 76 ? 1020 sodium ions c. 2. 10 ? 1021 sodium ions d. 1. 05 ? 1021 sodium ions e. 9. 52 ? 1020 sodium ions Answer E113. Determine the volume of hexane that contains 5. 33 ? 1022 molecules of hexane. The density of hexane is 0. 6548 g/mL and its molar mass is 86. 17 g/mol. a. 8. 59 mL b. 13. 5 mL c. 7. 40 mL d. 12. 4 mL e. 11. 6 mL Answer E114. Determine the molecular formula of a compound that has a molar mass of 92. 0 g/mol and an empirical formula of NO2. a. N2O3 b. N3O6 c. N2O4 d. NO2 e. N2O5 Answer C115. Determine the empirical formula for a compound that is 36. 86% N and 63. 14% O by mass. a. NO b. N2O c. NO2 d.N2O3 e. NO3 Answer D116. Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor. a. 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) b. C2H6(g) + 5 O(g) 2 CO(g) + 3 H2O(g) c. 2 C2H6(g) + 5 O2(g) 4 CO(g) + 6 H2O(g) d. C2H6(g) + 7 O(g) 2 CO2(g) + 3 H2O(g) e. 2 CH3(g) + 5 O(g) 2 CO(g) + 3 H2O(g) Answer C117. Which of the following is one possible form of pentane? a. CH3CH2CH2CH2CH3 b. CH3CH=CHCH2CH3 c. CH3CH2CH2CH2CH2CH3 d. CH3CH2CH2CH2CH2NH2 e. CH3CH2-O-CH2CH2CH3 Answer A118. List the elements in a hydrocarbon Answer hydrogen and carbon119. What type of bonding is found in the compound OF2? a. covalent bonding b. hydrogen bonding c. ionic bonding d. metallic bonding Answer A120. In which set do all elements tend to form cations in binary ionic compounds? a. K, Ga, O b. Sr, Ni, Hg c. N, P, Bi d. O, Br, I Answer B121. Rb2S is named a. rubidium disulfide. b. rubidium sulfide. c. rubidium(II) sulfide. d. rubidium sulfur. Answer B122. An aqueous solution of H2S is named a. hydrosulfuric acid. b. hydrosulfurous acid. c. sulfuric acid. d. sulfurous acid. Answer A123. What is the molar mass of nitrogen gas? a. 14. 0 g/mol b. 28. 0 g/mol c. 6. 02 ? 1023 g/mol d. 1. 20 ? 023 g/mol Answer B124. What mass of carbon dioxide, C O2, con tains the same number of molecules as 3. 00 g of trichlorofluoromethane, CCl3F? a. 0. 106 g b. 0. 961 g c. 1. 04 g d. 9. 37 g e. Answer B125. Which of the following has the greatest mass? a. 3. 88 ? 1022 molecules of O2 b. 1. 00 g of O2 c. 0. 0312 mol of O2 d. All of the above have the same mass. Answer A126. A sample of pure calcium fluoride with a mass of 15. 0 g contains 7. 70 g of calcium. How much calcium is contained in 40. 0 g of calcium fluoride? a. 2. 27 g b. 7. 70 g c. 15. 0 g d. 20. 5 g Answer D127. What is the empirical formula of a compound that is 62. % C, 10. 4% H, and 27. 5% O by mass? a. C3HO b. C6HO3 c. C6H12O2 d. C5H10O2 e. C3H6O Answer E128. How many oxygen atoms are there in 7. 00 g of sodium dichromate, Na2Cr2O7? a. 0. 187 oxygen atoms b. 2. 30 ? 1021 oxygen atoms c. 1. 60 ? 1022 oxygen atoms d. 1. 13 ? 1023 oxygen atoms Answer D129. Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 0. 80 g of methane reacts with 3. 2 g of oxygen to produce 2. 2 g of carbon dioxide? a. 1. 8 g b. 2. 2 g c. 3. 7 g d. 4. 0 g Answer A130. Combustion analysis of 1. 200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2. 86 g of CO2 and 1. 134 g of H2O. What is the empirical formula of the compound? a. C2H5O b. C2H5O2 c. C2H10O3 d. C3H8O2 Answer D131. What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? _____ C2H6O (l) + _____ O2(g) _____ CO2(g) + _____ H2O(l) a. 9 b. 7 c. 5 d. 3 Answer D132. Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered coefficients? a. 1 b. 2 c. 3 d. none of these Answer C