Chemistry Reviewer 1. Uranium-235 and uranium-238 have the same number of which of the following? a. Protons and electrons b. neutrons c. protons d. electrons 2. What is the valence (oxidation state) of carbon in sodium carbonate (Na2CO3)? a. -4 b. 4 c. 2 d. -2 3. Water and SO3 combine to sulfuric acid (H2SO4) according to the following reaction. How many grams of water must be added to 100 g of 20% oleum (20% SO3 and 80% H2SO4by weight) to produce a 95% solution ( byweight) of sulfuric acid? a. 3.3 g b. 14 g c. 5.0 g d. 7.5 g 4. During a laboratory experiment at 1.0 atm and 25oC, a student observed that oxygen gas was produced by de-composition of 15 g of sodium chlorate. What was the volume of oxygen? a. 1.27 L b. 6.54 L c. 5.17 L d. 3.85 L 5. Which of the following does a catalyst change? a. the activation energy of a reaction b. the equilibrium constant of areaction c. the concentration of product at equilibrium d. the heat of reaction of a reaction 6. What is an isomer? a. a substance containing a hydroxyl ion b. a single atom c. different arrangement of the same atoms d. a basic building block for large chemical chains 7. The reaction shown occurs in a gaseous phase. Once equilibrium has been achieved in a particular reaction vessel, additional HI gas is injected directly into the reaction vessel. Compared to the initial conditions, which of the following statemnets is correct after the new equilibrium has been achieved? a. The amount of H2 will have decreased. b. The partial pressure of H2 will have decreased. c. The amount of I2 will have increased. d. The partila pressure of HI will have decreased. 8. Which of the following compounds would be ionic, considering the electronegativities of the elements? a. I2 b. NO c. CO d. KCI 9. An unknown gas with a temperature of 25oC and a pressure of 740 mm Hg is collected in a sampling bag. The volume and mass of the gas are 24.0 L and 34.9 g,
respectively. Which chemical formula could represent the gas? a. N2 b. H2S c. HCI d. Ar
b. There would be no change in the amount of ammonia (NH3) present. c. More ammonia (NH3) would be generated. d. The amount of ammonia (NH3) would double.
10. What is the percentage (by mass) of htdrogen in glucose (C6H12O6)? a. 0.067 b. 0.093 c. 0.17 d. 0.4
19. Which of the following statements concerning reversible reactions is false? a. Temperature affects the direction of the reaction. b. Concentration have no effect on the direction of the reaction c. Concentration remain constant once equilibrium is reached. d. Both reactants and products are always present.
11. 2.00 g of a substance dissolved in 250 g of water produces a boiling point elevation of 0.065oC. What is the molecular weight of the substance? a. 63 b. 92 c. 16 d. 8 12. A current of 0.075 A passes through a solution of silver nitrate for 10 munites. How much silver is deposited? a. 0.040g b. 0.035 g c. 0.030 g d. 0.050 g 13. How many grams of copper will be deposited at an electrode if a current of 1.5 A is supplied for 2 hours to a CuSO4? a. 7.1 g b. 3.6 g c. 48 g d. 2.4 g 14. What is the order of reaction with respect to reactant E and the overall order of the reaction described by the following rate law? a. second order with respect to E; second order overall b. first order with respect to E; second order overall c. second order with respect to E; fourth order overall d. first order with respect to E; fourth order overall 15. What is the term for a quantity of a susbstance to which a chemical formula can be assigned and whose mass is equal to its formula weight? a. a mole b. an equivalent c. a molecule d. a one-normal solution 16. The pH of a 0.001 M HCI solution is a. 5 b. 3 c. 7 d. 1 17. The half-life of radioactive carbon is approximately 5700 years. If a sample is found to have 7000 atoms after 6000 years, how many atoms were presents initially? a. 13800 atoms b. 14500 atoms c. 14300 atoms d. 14100 atoms 18. Given the following reversible chemical reaction, assume all reactants and products are ideal gases. a. The amount of ammonia (NH3) would halve.
20. Which of the following reactions are not balanced? a. IV only b. I only c. II and III d. I and III 21. 2.00 g of a substance dissolved in 250 g of water produces a boiling point elevation of 0.065oC. What is the molecular weight of the substance? a. 92 b. 16 c. 8 d. 63 22. Oxygen reacts stoichimetrically with methane to form 14 g of carbon monoxide. How many moles of methane are consumed? a. 1 mol b. 0.5 mol c. 2 mol d. 1.5 mol 23. Which o fthe following chemical formulas is incorrect? a. Na2CO3 b. KOH c. Ca(OH)2 d. CaCI 24. What are the chemical formulas for the following compounds: aluminum nitrate, magnesium hydroxide, calcium oxide, and cupric carbonate? a. AINO3,Mg(OH),Ca2O3,CuCO3 b. AI(NO3)3,Mg(OH)2,CaO,CuCO3 c. AL2NO3,Mg(HO),CaO2,CuCO3 d. AINO3Mg(HO)2,CaO,Cu(CO3)2 25. Nitroglycerin is made by combining glycerol, nitric acid, and sulfuric acid. What are the minimum coefficients needed to balance the equation of this reactions? a. 4,2,1,1,3,1 b. 1,3,1,1,3,1 c. 1,3,3,1,3,2 d. 2,6,2,2,6,2
b. 320 kPa c. 240 kPa d. 160 kPa 28. A wastewater treatment plant uses chlorine gas as a reactant. A tank is filled with 800 m3 of 20oC water, and chlorine is added at a dosage of 125 g per cubic meter of water. (Assume all of the chlorine dissolves and none initially reacts chemically.) If the atmospheric pressure is 1.0 atm, what is the theoretical partial pressure of the chlorine gas at the tank surface immediately after the gas is added? a. 2.3 x 10-4 atm b. 0.11 atm c. 3.1 x 10-5 atm d. 0.039 atm 29. What family of compounds is produced from the reaction between an alcohol and a carboxylic acid? a. ether b. amine c. ester d. ketone 30. Which of the following statements pertaining to acids and bases is incorrect? a. Acids conduct electricity in aqueous solutions. b. Bases have a pH between 7 and 14. c. Bases have a sour taste. d. Acids turn blue litmus paper red. 31. As the pressure of a gas increases, the solubility of that gas in a liquid a. always increases. b. is not changed. c. always decreases. d. cannot be determined. 32. What is a distinguishing characteristic of the halogens? a. They are phosphorescent. b. Next to the noble gases, they are the most chemicallyinactive group. c. They readily accept an electron from another atom to form compounds. d. They have a high electrical conductivity. 33. Enthalpy of formation is most closely defined as the a. potential energy of a substance. b. energy absorbed during creation of 1 grammole of a compound from pure elements. c. energy absorbed or released during a chemical reaction. d. sum of the enthalpy of reactions. 34. Assuming all of the energy goes into the reaction, what electrical power is required to produce oxygen gas at a rate of 50 mg/s?
36. A transportation company specializes in the shipment of pressurized gaseous materials. An order is received for 100 L of a particular gas at STP (0oC and 1 atm). What minimum volume tank is necessary to transport the gas at 25oC and a maximum pressure of 8 atm? a. 14 L b. 12 L c. 16 L d. 10 L 37. In an experient, a compound was determined to contain 68.94% oxygen and 31.06% of an unknown element by weight. The molecular weight of this compound is 69.7 g/mol. What is this compound? a. SiO4 b. NO2 c. F2O2 d. B2O3 38. 6 g of a substance are dissolved in 1000 g of water. The solution freezes at -0.16oC. What is the molecular weight of the substance? a. 70 g/ mol b. 60 g/mol c. 75 g/mol d. 100 g/mol 39. A gaseous mixture consists of 2 kg of oxygen, 5 kg of nitrogen, and 3 kg of xenon. What is the mole fraction of the oxygen gas? a. 0.24 b. 0.17 c. 0.11 d. 0.13 40. The diameter of a spherical mothball is observed to halve in 200 days.approximately how long will it take for its remaining volume to become half of its volume at 200 days? a. 67 days b. 160 days c. 130 days d. 200 days 41. For a given isotope of an element, the atomic number plus the atomic weight is 148, and their difference is 58. how many protons does an atom of the isotope contain? a. 45 b. 90 c. 148 d. 58 42. 10 g of solid PCI5 is heated in a 0.5 m3 container to 150oC, producing gaseous PCI3 and CI2 gas according to the following decomposition reaction: The molecule weights of the compound are What is the increase in pressure in the container when 50% (By weight) of the PCI5 is decomposed? a. 0.250 kPa b. 18 kPa c. 0.120 kPa d. 0.350 kPa
26. Which of the following occurs when table salt (NaCI) is added to continuously heated boiling water? a. The water boils even more agitatedly. b. The temperature of the water decreases but boiling continues uninterrupted. c. The water continues to boil. d. The water momentarily stops boiling. 27. The final temperature of the hydrogen and chlorine described in Prob. 8 is 30oC. What is the final pressure in the reaction vessel? a. 80 kPa
35. What is the oxidation number for chromium (Cr) in the compound BaCro? a. 2 b. 4 c. 1 d. 6
a. 9.2 kW b. 0.89 kW% c. 3.1 kW d. 1.5 kW
43. An alkyl radical is best defined as a. an electron that is shared in a covalent bond.
b. any functional group that substitutes for a hydrogen atom in an alkane. c. the remaining portion of an alkane after it loses a hydrogen atom. d. cancer-causing molecules found in foods 44. It is known that ozone (O3) will decompose into oxygen (O2) at a temperature of 100o. One mole of ozone is sealed in a container at STP (0oC and 1 atm). What will be pressure of the container once it is heated to 100oC? a. 37 kPa b. 1.4 kPa c. 2.1 kPa d. 210 kPa 45. How much water must be added to 100 mL of a 0.75 molar solution of KCI to make a 0.04 molar solution? a. 1.88 L b. 0.188 L c. 1.78 L d. 1.98 L 46. While moving from left to right across the second row of the periodic table (i.e., from Li to Ne), the atomic radii tend to a. first increase, then decrease. b. uniformly increase. c. remain the same. d. uniformly decrease. 47. A solution is adjusted from pH 8 to pH 9. The relative concentraation of the hydrogen [H+] ion has changed by a factor of what? a. 1100 b. 5 c. 110 d. 10 48. The solubility constant of stronyium sulfate, SrSO4, is 2.8 x 10-7. How many grams of SrSO4 must be dissolved in water to produce 1 L saturated solution? a. 0.1 g b. 2 g c. 0.00005 g d. 0.0005 g 49. Which of the following elements has the largest first ionazation energy? a. CI (chlorine) b. Ar (argon) c. H (hydrogen) d. Kr (krypton) 50. How many milliters of 1 M NaOH solution will 25 mL of 2 H2SO4neutralize? a. 50 mL b. 100 mL c. 75 mL d. 25 mL 51. What is the molarity of a solution obtained by dis-solving 25 g of NaCI in enough water to produce 4 L of solution? a. 6.25 b. 0.365 c. 0.428 d. 0.107 52. What is the half-life of a substance that decays to 25% of its original amount in six days? a. 3 days b. 0.08 days c. 8 days d. 12 days
53. Two moles of sodium react with 2 moles of water to produce which of the following? a. 1 mole of sodium hydroxide and 1 mole of hydrogen b. 2 moles of sodium hydroxide and 1 mole of hydrogen c. 1 mole of sodium hydroxide and 2 moles of hydrogen d. 2 moles of sodium hydroxide and 2 mole of hydrogen 54. When a deliquescent substance is exposed to air, it a. oxidizes. b. becomes moist c. crystallizes. d. loses water of hydration. 55. Which of the following elements does not exists as a diatomic molecule under normal (ambient) conditions? a. chlorine b. oxygen c. iodine d. sulfur 56. A given sample of radioactive material has 80% of the original substance remaining after 10 years. How much will remain after 90 additional years? a. 0.001 b. 0.017 c. 0.11 d. 0.13 57. The decay of U-238 to Pb-206 can be used to estimate the age of inorganic matter. The half-life of U-238 is 4.5 x 109 years. In a particular rock sample, the ratio of the numbers of Pb-206 to U-238 atoms is 0.66. Assume all of the Pb-206 present is due to the decay of U-238. What is the age of the rock? a. 3.3x 109 yr b. 1.4 x 109 yr c. 7.0 x 109 yr d. 9.3 x 109yr 58. How much energy is needed to convert ozone to oxygen? a. 43 kcal/mol b. 0 kcal/ mol c. 68 kcal/mol d. 140 kcal/mol 59. The group of metals that includes lithium, sodium,potassium, rubidium, and cesium forms a closely related family known as the a. rare earth group. b. halogens. c. alkali metals. d. alkaline earth metals. 60. Hydrogen and chlorine gas combine in a 35 m3 reaction vessel to produce hydrogen chloride. The masses of hydrogen and chlorine are 4.5 kg and 160 kg, respectively. How much hydrogen chloride gas is produced? a. 41 kg b. 21 kg c. 82 kg d. 160 kg 61. How many liters of 2M solution (i.e., a molarity of 2) can be produced from 184 g of enthyl alcohol (CH3CH2OH)? a. 1.5 L b. 5.0 L c. 2.0 L
d. 2.5 L 62. If the current, I, is 100 A, at what rate is oxygen produced?
a. 18.7 mg/s b. 8.29 mg/s c. 16.7 mg/s d. 9.34 mg/s 63. What mass of lead nitrate, Pb(NO3)2, must be dis-solved in 1 L of water to produce a solution that contains 20 mg of lead ions? Assume 100% ionazation. a. 43 mg b. 52 mg c. 32 mg d. 26 mg 64. A compound in gas form Has a mass of 0.377 g and occupies 191.6 mL at standard conditions (0oC and 760 mm Hg). What is the formula of the compound? a. C3H8 b. CH4 c. C5H12 d. C2H6 65. A gas mixture of N2(g) and CO2(g) contained in a volume of 10.0 L has a total pressure of 0.750 atm at a temperature of 273K. The mixture is known to contain 3.00 g N2(g). What is the partial pressure of CO2(g) in the mixture? a. 0.120 atm b. 0.630 atm c. 0.510 atm d. 0.240 atm 66. Rank the following gas according to increasing effusion rates relative to O2 (reference). a. F2< CO24 b. F<2< CH<4< CO<2 c. CH42
d. Lower the temperature and add more water 69. What is the mass of 0.01 gram-moles of Na2SO4? a. 1.42 g b. 1.19 g c. 0.71 g d. 2.38 g 70. An ideal gas occupies a volume of 4L and has a pressure of 283.71kPa (1atm=101.325kPa). Under 22.50C, what most likely is the identity of the gas if 0.01293 Kg of gas is used. a. O2 b. Cl2 c. F2 d. N2 71. The reaction shown proceeds in a gaseous state. At equilibrium, the concentration of the components X,Y, and Z are measured to be 5.73 x 10-2 mol/L, 2.67 x 10-2 mol/L and 4.59 x 10-2 mol/L, respectively. What is the equilibrium constant for this reaction? a. 9.8 x 10-4mol/L b. 1.7 x 10-2mol/L c. 3.7 x 10-1 mol/L d. 2.1 x 10-2mol/L 72. If 1.5 L of an ideal gas at 250C is heated, the new volume increases 2.5 times the original volume. The pressure and amount of substance are held constant. What is the new temperature of gas in 0F a. 882 0F b. 8800F c. 820 0F d. 8280F 73. "::Add_Chem_013::Following are three states for fluorine:1s22s12p6 1s22s22p5 1s22s22p42d1 They are, respectively: _____" a. ground, excited, impossible b. ground, impossible, excited c. excited, impossible, ground d. excited, ground, impossible 74. At what temperature in 0C will O2 has under a pressure of 2.4 atm? (ρ of O2= 1.43 g/L) a. 645.7510C b. 3810C c. 315.570C d. 318.160C 75. Macro Vee collected hydrogen gas using water displacement method. He measured the temperature of water using a thermometer and found out that it is 230C with the correponding pressure of 21.1 mmHg. Calculate the pressure of hydrogen gas under standard atmospheric pressure. a. 95.81 KPa b. 98.51 Kpa c. 98.15 Kpa d. 95.18 Kpa 76. A sample of an unknown compound is found to be 49.3% carbons, 9.6% hydrogen, 19.2% nitrogen, and 21.9% oxygen by weight. What is its molecular formula? a. C3H7NO b. C3H7NO c. C4H<><> d. C4H4NO 77. Balance the following reaction. a. HBrO3 + 5HBr 3H2O + 3bR2
b. 3HBrO3 + HBr 2H2O + 2Br2 c. 2HBrO3 + 4HBr 3H2O + 3Br2 d. HBrO3 + 4HBr 3H2O + Br2 78. Which of the following is the correct electron configuration of Pb? a. [Xe]6s24f146s2 b. [Xe]6s25d104f146p2 c. [Xe]6s25d104f145d106p2 d. [Xe]5d104f146p2 79. The mole (mol) is the amount of a substance that contains as many elementary entities as there are atoms in exactly a. 12.00 grams of C. b. average atomic mass of isotopes of C. c. 12.01 grams/mol of C. d. 12.00 grams of 12C. 80. At STP the volume of 1.5 mole N2as compared to 1.0 mole O2 is a. higher to about three fourths b. the same, 22.4L c. different by about 11.2 L d. differ by a factor of 1.25 81. "::Add_Chem_008:: How many grams of glucose, C6H12O6, are necessary to prepare 656 mL of a solution with a concentration that is 0.550 molar? _____" a. 0.00200 g b. 151 g c. 64.9 g d. 214 g 82. n the following reaction, which elements are the reducing and exidizing agents? a. Mg is the reducing agents; O2 is the oxidizing agent. b. MgO is the reducing agent; Mg is the oxidizing agent. c. Mg is the reducing agent;MgO is the oxidizing agent. d. O2 is the reducing agent; Mg is the oxidizing agent. 83. By decreasing the pressure of an ideal gas at constant temperature and amount of substance 1/3 times the original pressure, the volume of gas will a. expands two thirds the original b. increases three times the original c. multiply by a factor of 1/3 d. decreases three times the original 84. What is the gravimetric (i.e.m.,mass) percentage of oxygen in K2CrO4? a. 0.33 b. 0.66 c. 0.57 d. 0.42 85. There are 500 g of zinc sulfide (ZnS) in a load of zinc ore. The ZnS is roasted in excess air to form zinc oxide (ZnO) and sulfer dioxide (S)2). How many grams of zinc can be subsequently recovered if 5% of the zinc is lost in the roasting process? a. 340 g b. 380 g c. 320 g d. 400 g 86. What is the enthalpy of reaction at 25oC for the combustion of ethane ( C2H6)? a. -680 kcal/mol (exothermic) b. -340 kcal/mol ( exothermic) c. 130 kcal/mol (endothermic) d. 340 kcal/mol (endothermic)
87. A silver wire has a diameter of 0.500 mm.What length of this wire contains exactly 1.00 mol of silver? [Given: density of Ag = 10.5 g/cm3 a. 51.3 mm. b. 52.3 mm. c. 50.3 mm. d. 53.3 mm. 88. Which principal energy level has exactly four subshells? a. 4 b. 3 c. 1 d. 2 89. Which sample demonstrate particles arranged in regular geometric pattern? a. CO2(g) b. CO2(aq) c. CO2(l) d. CO2(s)
96. Which of the following isotopes has the greatest number of neutrons? a. 40AR b. 35Cl c. 31P d. 41Ca 97. When 38.0 mL of 0.1250 M H2SO4 is added to 100. mL of a solution of Pbl2, a precipitateof PbSO4 is then filtered from the solution,dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471 g, what was the concentration of iodide ions in the original solution? a. 3.10 x 10-3 M b. 3.11 x 10-3 M c. 3.12 x 10-2 M d. 3.11 x 10-2 M
90. An atom has eight electrons in a 3d subshell. How many orbitals in this subshell have an unpaired electron? a. 2. b. 1. c. 4. d. 3.
98. There are 500 g of zinc sulfide (ZnS) in a load of zinc ore. The ZnS is roasted in excess air to form zinc oxide (ZnO) and sulfer dioxide (S)2). How many grams of zinc can be subsequently recovered if 5% of the zinc is lost in the roasting process? a. 380 g b. 320 g c. 400 g d. 340 g
91. Which atom is not paired with its correct ion and ionic charge. a. Rb / Rb1b. F / F1c. Li / Li1+ d. Mg / Mg2-
99. Which substance can be decomoposed chemically? a. Hydrogen b. Iron c. Ammonia d. Neon
92. The Hall process for the production of the aluminun involves the reaction of the aluminum oxide with elemental carbon to give aluminum metal and carbon momoxide. If the yield of this reaction is 82% and aluminum ore is 71% by mass aluminum oxide,what mass of aluminum ore must be mined in order to produce 1.0 x 103 kg(1 metric ton) of aluminum metal by the Hall process? a. 3.3 x 103 kg b. 3.4 x 103 kg c. 3.1 x 103 kg d. 3.2 x 103 kg
100. How many liters of oxygen gas at 153oC and 0.820 atm can be produce by the decomposition of 22.4 g of solid KCIO3? (The other decomposition product is solid potassium chloride.) a. 9.7 L b. 11.7 L c. 12.7 L d. 10.7 L
93. Which of the following is not a conclusion Rutherford made from his experiment with alpha particles being shot at a thin sheet of gold foil? a. An atom is mainly empty space b. An atom has a negatively charged nucleus. c. An atom has a very small, compact nucleus d. An atom's mass is concentrated in the nucleus. 94. A liquid will boil when a. its vapor pressure is equal to the melting point b. its vapor pressure is equal to the surrounding pressure c. it is heated to a temperature that is below the boiling point. d. a salt has been added to the liquid 95. Which units could be usued to express the account absorved or released during chemical reaction? a. Torr and mmHg b. Gram and liter c. Calorie and joule d. Degree and gram
101. Which two elements will display the most similar chemical properties? a. Litium and potassium b. Aluminum and calcium c. Chlorine and sulfur d. Nickel and phosphorus 102. Assuming the ground state, all of the elements located in the group 12 of the periodic table will have the same number of a. electrons b. occupied principal energy levels c. nuclear particles d. valence electrons 103. The modern periodic table is arranged based upon atomic a. isotopes b. density c. number d. radius 104. The gas present in electric bulbs is argon. If a samle of this gas is at a pressure of 101.325 kPa, when the volume is 0.1L and the temperature is 32oC,what must its temperature [in oC] be if its volumes becomes 200mL and its pressure 96 kPa? a. 305 b. 105 c. 205 d. 405
105. Which electron configuration demonstrates an atom in the excited state? a. 1s22s23s1 b. 1s22s1 c. 1s22s22p4 d. 1s22s2 106. A 350. mL samle of 0.276 M HNO3 is partially neutralized by 125mL of 0.0120 M Ca(OH)2. Find the concentration of nitric acid in the resulting solution. a. 0.197 M b. 0.187 M c. 0.157 M d. 0.167 M 107. Identify the oxidizing agent in the chemical reaction 2MnO4? + 5H2SO3 ? 2Mn2+ +5SO42? + 3H2O. a. MnO4 ? 108. The elements that display the greatest non-metallic character are located toward which corner of the periodic table? a. Lower right b. Upper right c. Dead center d. Upper left 109. What mass of KCIO3 must be decomposed to produce 126 L of oxygen gas at 133oC and 0.880 atm? (The other reaction product is solid KCI.) a. 282 g b. 272 g c. 252 g d. 262 g 110. The mineral manganosite is a cmpound of manganese-55 and oxgen-16. If 77%o f the mass manganosite is due to manganese,what is the empirical formula of manganosite? a. MnO2 b. Mn3O4 c. MnO d. MnO3 111. A method of removing CO2 from a spacecraft is to allow the CO2 to react with sodium hydroxide. (The products of the reaction are sodium carbonate and water.) What volume of carbon dioxide at 25oC and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts? a. 309 L b. 308 L c. 311 L d. 310 L 112. Which gas under a high temperature and a low pressure behaves most like an ideal gas? a. Ne b. O2 c. He d. NH3 113. The radius of the Earth is approximately 6370 km. If one could dig down straight towards the center of the Earth, one would find that the innermost 3480 km (the core) has an average of density of about 11 g/cm3. Above that are the mantle and crust.
If the average density of the Earth is 5.5 g/cm3, what is the average density of the Earth's mantle and crust?(Recall that the volume of a sphere is given V=(4/3)?r3.) a. 4.3 g/cm3 b. 4.4 g/cm3 c. 4.5 g/cm3 d. 3.4 g/cm3 114. Which setence below is incorrect? a. Salads are heterogeneous mixtures. b. Sand and water make heterogeneous mixture. c. Pure iron is a heterogeneous mixture. d. Milk is a homogeneous mixture. 115. An object will float at the surface of a liquid if the mass of the object is less than the mass of the lliquid that it displaces. A spherical vessel (diameter = 5.00 cm) when empty has a mass of 12.00 g. What is the greatest volume of water that can be placed in the vessel and still have the vessel float at the surface of benzene? (Given: density of water = 1.00 g/cm3; density of benzene = 0.879 g/cm3) a. 25.5 L b. 45.5 L c. 55.5 L d. 35.5 L 116. Which gas is expected to have the highest rate of effusion? a. He b. O2 c. H2O d. F2 117. The mineral hausmannite is a compound of manganese-55 and oxygen-16. If 72% of the mass of hausmannite is due to manganese, what is the empirical formula of hausmannite? a. MnO2 b. Mn3O4 c. MnO3 d. MnO 118. A book is lifted off of the floor and placed on a table that is one meter above the floor. The book has a. gained potential energy b. gained kinetic energy c. gained sound energy d. lost chemical energy 119. Which phase change is described correctly? a. Gas to solid is called sublimation. b. Liquid to solid is called freezing c. Solid to liquid is called vaporization d. Solid to gas is called deposition 120. Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCI solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. a. 1.09 L b. 1.11 L c. 1.10 L d. 1.12 L
121. When octane (C8H18) is burned in a particular internal combustion engine, the yield of the products (carbon dioxide and water) is 93%. What mass of carbon dioxide will be produced in this engine when 15.0 g of octane is burned with 15.0 g of oxygen gas? a. 13 g b. 11 g c. 10 g d. 12 g 122. When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1oC and 0.85 atm that can be formed when 275 mL of 0.725 M HCI solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. a. 2.6 L b. 2.9 L c. 2.7 L d. 2.8 L 123. Which sample represent a homogeneous misture? a. CH3OH(g) b. CH3OH(aq) c. CH3OH(s) d. CH3OH(l) 124. In period 3 of the periodic table the atom with the largest atomic radius is located in group a.1 b. 3 c. 17 d. 18 125. A 250. mL sample of 0.0328 M HCI is partially neutralized by the addition of 100. mL of 0.0245 M NaOH.Find the concentration of hydrochloric acid in the resulting soution. a. 0.0173 M b. 0.0164 M c. 0.0174 M d. 0.0163 M 126. What is the mass of an object that has a density of 13 g/mL and a volume of 10 mL? a. 1.3 g/L b. 1.3 g/mL c. 130 g/mL d. 0.77 g/mL 127. In the chemical reaction 5S + 6KNO3 + 2CaCO3 ? 3K2SO4 + 2CaSO4 + CO2 + 3N2, the oxdizing agent is a. KNO3 128. An atom in the ground state has seven valence electrons. Which electron configuration could represent the valence electron configuration of this atom in the ground state? a. 3s63p1 b. 3s23p1 c. 3s13p6 d. 3s23p5 129. Which of the following bonds would you expect to be the most polar? a. N-P b. N-Bi
c. N-Sb d. N-As 130. At which temperature does a water sample have the highest average kinetic energy? a. 100 degrees Celcius b. 0 degrees Celcius c. 0 K d. 100 K 131. Americans combined drive about 4.0x109 miles per day and their vehicles get an average of 20 miles per gallon of fuel used.For each 1kg of gasoline that is burned,about 3.0 kg of carbon dioxed are produced. How many kilograms of CO2 are emitted into the atmosphere each day by cars in the U.S.? One gallon of gas weighs about 3.5 kg. a. 2.1x109 kg b. 3.1x109 kg c. 4.1x109 kg d. 1.1x109 kg 132. The Hall process for the production of the aluminun involves the reaction of the aluminum oxide with elemental carbon to give aluminum metal and carbon momoxide. If the yield of this reaction is 75%, what mass of aluminum metal can be produced from the reaction of 1.65 x 106 of aluminum oxide with 1.50 x 106 g of carbon? a. 6.3 x 105 g b. 6.6 x 105 g c. 6.5 x 105 g d. 6.4 x 105 g 133. It has been determined that 1.0 L of solution contain 52.7 g H2SO4, 240.8 g KMnO4, 11.3 g K2SO4, and 5.5 g Mn2O7. The reaction equation is The molecular weights of the compounds are What is the equilibrium constant for the reaction? a. 1.3 x 10-3 b. 6.9 x 10-3 c. 5.2 x 10-3 d. 2.6 x 10-3 134. When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1oC and 0.85 atm that can be formed when 275 mL of 0.725 M HCI solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. a. 2.9 L b. 2.8 L c. 2.6 L d. 2.7 L 135. A 2.50-L flask contains a mixture of methane (CH4) and propane (C3H8) at a pressure of 1.45 atm and 20oC.When this gas mixture is then burned in excess oxygen, 8.60g of carbon dioxide is formed.(The other product is water.)What is the mole fraction of methane in the original gas mixture? a. 0.75 b. 0.85 c. 0.93 d. 0.73
136. Iron has a density of 7.78 g/cm3. What mass of iron would be required to cover a football playing surface of 120 yds x 60 yds to a depth of 1.0 mm?(1 inch = 2.54 cm) a. 57 Mg b. 47 Mg c. 27 Mg d. 37 Mg 137. The time required for a given volume of N2 to diffuse through an orifice is 35 sec. Calculate the molecular weight of a gas which requires 50 sec to diffuse through the same orifice under identical conditions. a. 51.75 g/mole b. 15.57 g/mole c. 57.15 g/mole d. 71.55 g/mole 138. Air contains 78% N2, 21% O2, and 1% Ar, by voolume. What is the density of air 1,000. torr and?10oC? a. 0.8 g/L b. 1.8 g/L c. 3.8 g/L d. 2.8 g/L 139. How many cubic centimeters of ore containing 0.22% by mass gold must be processed to obtain $100 worth of gold? The density of the ore is 8.0 g/cm3 and the price of gold is $418 pre troy ounce. (14.6 troy oz = 1.0 ordinary pound,called an avoirdupois pound; 1lb = 454g) a. 3.2 x 102 cm3 b. 4.2 x 102 cm3 c. 5.2 x 102 cm3 d. 3.3 x 102 cm3 140. A wastewater treatment plant uses chlorine gas as a reactant. A tank is filled with 800 m3 of 20oC water, and chlorine is added at a dosage of 125 g per cubic meter of water. (Assume all of the chlorine dissolves and none initially reacts chemically.)If the atmospheric pressure is 1.0 atm, what is the theoretical partial pressure of the chlorine gas at the tank surface immediately after the gas is added? a. 3.1x10-5 atm b. 3.2x10-5 atm c. 3.3x10-5 atm d. 3.0x10-5 atm 141. Dimenthly hydrazine (CH3)2NNH2 has been used as a fuel in space, with nitrogen tetraoxide (N2O4) as the oxidizer. The products of the reaction between these two in an engine are H2O, CO2, and N2. What is the mass of nitrogen tetraoxide required to burn 50 kg of dimenthly hydrazine? a. 153 kg b. 128 kg c. 100 kg d. 50 kg 142. An unknown quantity of hydrogen gas has a volume of 2.5 L at STP (0o and 1 atm). What is the mass of hydrogen? Select one: a. 0.19 g b. 0.51 g c. 0.073 g d. 0.22 g
143. How many valence electrons are in a atom with the configuration 1s22s22p63s23p2 Select one: a. 5 b. 2 c. 6 d. 4 144. The mole fraction of oxygen molecules in dry air is 0.2029.What volume of dry air at 1.00 atm and 25oC is required for burning 1.00 L of hexane (C6H14, density = 0.660 g/mL) completely, yeilding carbon dioxide and water? Select one: a. 8490 L b. 8495 L c. 8409 L d. 8499 L 145. The first step in the Otswald process for producing nitric acid is 4NH3(g) + 5O2(G) ? 4NO(g) + 6H2O(g). If the reaction of 150 g of ammonia with 150 g of oxygen gas yeilds 87 g of nitric oxide (NO), what is the percent yeild of this reaction? Select one: a. 0.44 b. 0.11 c. 0.22 d. 0.33 146. A 0.850-mole sample of nitrous oxide, a gas used as anasthetic by dentists, has a volume of 20.46 L at 123oC and 1.35 atm. What would be its volume [in L] at 468oC and 1.35 atm? Select one: a. 36.3 b. 37.3 c. 38.3 d. 39.3 147. A method of producing pure copper metal involves the reaction of copper(I) sulfide with oxygen gas to give copper metal and sulfur dioxide. Suppose the yield of this reaction is 87%. What mass of a copper ore consisting of 46% copper(I) sulfide must be mined in order to produce 1.0x103 kg (1.0 metric ton) of copper metal? Select one: a. 2.2x103 kg b. 5.2x103 kg c. 4.2x103 kg d. 3.2x103 kg 148. When 20.0 mL of a 0.250 M (NH4)2S solution is added to 150.0 mL of a solution of Cu(NO3)2, CuS precipitate forms. The precipitate is then filtered from the solution,dried, and weighed. If the recovered CuS found to have a mass of 0.3491 g, what was the concentration of copper ions in the originalCu(NO3)2 solution? Select one: a. 2.24 x 10-2 M b. 2.43 x 10-2 M c. 2.34 x 10-2 M d. 2.42 x 10-2 M