Honors Chemistry Practice Final Exam

Multiple ChoiceIdentify the choice that best completes the statement or answers the question.

__D__ 1. Which of the following is not a physical change?a. grinding c. boilingb. cutting d. burning

__C__ 2. Which of the following is not a chemical change?a. rusting c. meltingb. igniting d. burning

__D__ 3. A chemical change occurs whena. dissolved minerals solidify to form a crystal.b. ethanol is purified through distillation.c. salt deposits form from evaporated seawater.d. a leaf changes color in the fall.

__D__ 4. A physical change occurs when aa. peach spoils.b. silver bowl tarnishes.c. bracelet turns your wrist green.d. glue gun melts a glue stick.

___A_ 5. Noble gases are in Group 18, and are best known because they area. unreactive. c. rare.b. excellent conductors. d. lanthanides.

___D_ 6. Nitrogen monoxide and oxygen, both colorless gases, form a red-brown gas when mixed. Nitrogen monoxide and oxygen are called thea. products. c. synthetics.b. equilibria. d. reactants.

__D__ 7. The liquid state of matter can be described asa. having definite shape and definite volume.b. having neither a definite shape nor a definite volume.c. having lost electrons owing to energy content.d. having a definite volume but not a definite shape.

__C__ 8. What happens to the energy in a substance when it changes state?a. It is destroyed.b. It is changed into matter.c. It changes form, but is neither destroyed nor increased.d. The energy remains unchanged.

__C__ 9. Which part of the illustration below shows the particles in a heterogeneous mixture?

a. a c. cb. b d. d

__C__ 10. A homogeneous mixture is also calleda. chemically bonded. c. a solution.b. a compound. d. a solute.

__D__ 11. The horizontal rows on the periodic table are calleda. actinides. c. elements.b. families. d. periods.

__A__ 12. A nonmetal is usuallya. brittle. c. a good conductor.b. malleable. d. used to make jewelry.

__B__ 13. The metric unit for length that is closest to the diameter of a pencil is thea. micrometer. c. centimeter.b. millimeter. d. decimeter.

__D__ 14. The symbols for units of length in order from largest to smallest area. m, cm, mm, km. c. km, mm, cm, m.b. mm, m, cm, km. d. km, m, cm, mm.

__C__ 15. Which of these metric units is used to measure mass?a. m c. gb. mm d. L

__B__ 16. The liter is defined asa. 1000 m3. c. 1000 g3.b. 1000 cm3. d. 1000 c3.

__D__ 17. The SI base unit for time is thea. day. c. minute.b. hour. d. second.

__D__ 18. Which pair of quantities determines the density of a material?a. mass and weight c. volume and concentrationb. volume and weight d. volume and mass

__C__ 19. When density is measured,a. a graduated cylinder is always used.b. the units are always kg/m3.c. the temperature should be specified.d. the material must be a pure substance.

_B___ 20. The density of aluminum is 2.70 g/cm3. What is the mass of a solid piece of aluminum with a volume of 1.50 cm3?a. 0.556 g c. 4.05 gb. 1.80 g d. 4.20 g

__D__ 21. A measurement that closely agrees with an accepted value is best described asa. precise. c. significant.b. reproducible. d. accurate.

__B__ 22. A numerical result is said to have good precision ifa. it agrees closely with an accepted value.b. repeated measurements agree closely.c. it has a small number of significant figures.d. it is a large whole number.

__D__ 23. If repeated measurements agree closely but differ widely from the accepted value, these measurements area. neither precise nor accurate.b. accurate, but not precise.c. both precise and accurate.d. precise, but not accurate.

__B__ 24. The number of significant figures in the measurement 0.000 305 kg isa. 2. c. 6.b. 3. d. 7.

__B__ 25. The number of significant figures in the measured value 0.032 0 g isa. 2. c. 4.b. 3. d. 5.

__A__ 26. Which of these measurements has only nonsignificant zeros?a. 0.0037 mL c. 400. mLb. 60.0 mL d. 506 mL

__D__ 27. Using a metric ruler with 1 mm divisions, the sides of a rectangular piece of plywood were measured as 3.54 cm and 4.85 cm, which corresponds to an area of 17.1690 cm2. Which of these shows the area expressed correctly?a. 17.1 cm2. c. 17.17 cm2.b. 17.169 cm2. d. 17.2 cm2.

__B__ 28. When 64.4 is divided by 2.00, the correct number of significant figures in the result isa. 1. c. 4.b. 3. d. 6.

__C__ 29. When 5.7 m is divided by 2 s, the quotient is correctly reported asa. 2.8 m/s. c. 2.9 m/s.b. 2.85 m/s. d. 3 m/s.

__A__ 30. The product of 13 cm and 5.7 cm is correctly reported asa. 74 cm2. c. 74.1 cm2.b. 74.0 cm2. d. 75 cm2.

__C__ 31. The measurement 0.020 L is the same asa. 2.0 10–3 L. c. 2.0 10–2 L.b. 2.0 102 L. d. 2.0 10–1 L.

__D__ 32. If values for x and y vary as an inverse proportion,a. their quotient is a constant. c. their product is a constant.b. their graph is a parabola. d. their graph is a straight line.

C 33. The principles of atomic theory recognized today were conceived bya. Avogadro. c. Dalton.b. Bohr. d. Rutherford.

__D__ 34 Which concept in Dalton's atomic theory has been modified?a. All matter is composed of atoms.b. Atoms of different elements have different properties and masses.c. Atoms can combine in chemical reactions.d. Atoms cannot be divided.

__B__ 35. When an electrical current passed through a glass tube, it caused the surface of the tube directly across from the cathode to glow. Scientists concluded thata. a magnetic field was produced.b. the particles of the beam were negatively charged.c. there was gas in the tube.d. atoms were indivisible.

__B__ 36. In Rutherford's experiments, most of the particlesa. bounced back. c. were absorbed by the foil.b. passed through the foil. d. combined with the foil.

__A__ 37. Rutherford's experiments led him to conclude that atoms contain massive central regions that havea. a positive charge. c. no charge.b. a negative charge. d. both protons and electrons.

___B_ 38. A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)a. nuclide. c. electron.b. neutron. d. isotope.

__D__ 39. The nucleus of an atom has all of the following characteristics except that ita. is positively charged.b. is very dense.c. contains nearly all of the atom's mass.d. contains nearly all of the atom's volume.

__C__ 40. An atom is electrically neutral becausea. neutrons balance the protons and electrons.b. nuclear forces stabilize the charges.c. the numbers of protons and electrons are equal.d. the numbers of protons and neutrons are equal.

C 41. All isotopes of hydrogen containa. one neutron. c. one proton.b. two electrons. d. two nuclei.

__B__ 42. As the atomic number increases, the number of electrons in a neutral atoma. decreases. c. remains the same.b. increases. d. is undetermined.

___A_ 43. The average atomic mass of an element is the average of the atomic masses of itsa. naturally occurring isotopes. c. radioactive isotopes.b. two most abundant isotopes. d. artificial isotopes.

__C__ 44. An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number isa. 13. c. 27.b. 14. d. 40.

_B___ 45. Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, hasa. 6 neutrons. c. 10 neutrons.b. 8 neutrons. d. 14 neutrons.

__D__ 46. Neon-22 contains 12 neutrons. It also containsa. 12 protons. c. 22 electrons.b. 22 protons. d. 10 protons.

__B__ 47. The mass of 2.0 mol of oxygen atoms (atomic mass 16.00 amu) isa. 16 g. c. 48 g.b. 32 g. d. 64 g.

__B__ 48. A sample of tin (atomic mass 118.71 amu) contains 3.01 1023 atoms. The mass of the sample isa. 3.01 g. c. 72.6 g.b. 59.3 g. d. 11 g.

__A__ 49. The mass of 5.000 mol of cesium (atomic mass 132.9 amu) isa. 664.5 g. c. 6.022 1023 g.b. 132.9 g. d. 5.000 g.

__A__ 50. The periodic tablea. permits the properties of an element to be predicted before the element is discovered.b. will be completed with element 118.c. has been of little use to chemists since the early 1900s.d. was completed with the discovery of the noble gases.

___B_ 51. Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement bya. mass number. c. group number.b. atomic number. d. series number.

_D___ 52. Elements in a group or column in the periodic table can be expected to have similara. atomic masses. c. numbers of neutrons.b. atomic numbers. d. properties.

__D__ 53. Identify the sublevels in a period that contains 32 elements.a. s, f c. s, p, db. s, p d. s, p, d, f

__C__ 54. How many elements are in a period in which only the s and p sublevels are filled?a. 2 c. 18b. 8 d. 32

__A__ 55. Elements in which the d-sublevel is being filled have the properties ofa. metals. c. metalloids.b. nonmetals. d. gases.

__A__ 56. Strontium's highest occupied energy level is 5s2. To what group does strontium belong?a. Group 2 c. Group 6b. Group 5 d. Group 8

__A__ 57. Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong?a. Group 2 c. Group 5b. Group 3 d. Group 12

__C__ 58. A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is calleda. electron affinity. c. electronegativity.b. electron configuration. d. ionization potential.

__C__ 59 A positive ion is known as a(n)a. ionic radius. c. cation.b. valence electron. d. anion

__A__ 60. Across a period in the periodic table, atomic radiia. gradually decrease.b. gradually decrease, then sharply increase.c. gradually increase.d. gradually increase, then sharply decrease.

_C___ 61. Valence electrons are those s and p electronsa. closest to the nucleus. c. in the highest energy level.b. in the lowest energy level. d. combined with protons.

_C___ 62. In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded bya. 2 electrons. c. 8 electrons.b. 4 electrons. d. 10 electrons.

__D__ 63. What is the correct Lewis structure for hydrogen chloride, HCl?

a. A c. Cb. B d. D

__D__ 64. The ions in most ionic compounds are organized into aa. molecule. c. polyatomic ion.b. Lewis structure. d. crystal.

__B__ 65. In metals, the valence electronsa. are attached to particular positive ions. c. are immobile.

b. are shared by all of the atoms. d. form covalent bonds.

__D__ 66. Malleability and ductility are characteristic of substances witha. covalent bonds. c. Lewis structures.b. ionic bonds. d. metallic bonds.

__A__ 67. According to VSEPR theory, the shape of an AB3 molecule isa. trigonal-planar. c. linear.b. tetrahedral. d. bent.

__B__ 68. A polar molecule containsa. ions.b. a region of positive charge and a region of negative charge.c. only London forces.d. no bonds.

__D__ 69. Iodine monochloride (ICl) has a higher boiling point than bromine (Br2) partly because iodine monochloride is a(n)a. nonpolar molecule. c. metal.b. polyatomic ion. d. polar molecule.

_A___ 70. A chemical formula for a molecular compound represents the composition ofa. a molecule. c. the ions that make up the compound.b. an atom. d. the crystal lattice.

_A___ 71. Name the compound Fe(NO3)2.a. iron(II) nitrate c. iron(III) nitrateb. iron(II) nitrite d. iron(III) nitride

__D__ 72. Name the compound Al2S3.a. aluminum sulfate c. aluminum(II) sulfateb. aluminum sulfur d. aluminum sulfide

__C__ 73. Name the compound CF4.a. calcium fluoride c. carbon tetrafluorideb. carbon fluoride d. monocalcium quadrafluoride

__D__ 74. Name the compound N2O3.a. dinitrogen oxide c. nitric oxideb. nitrogen trioxide d. dinitrogen trioxide

__D__ 75. What is the formula for diphosphorus pentoxide?a. P2PeO5 c. P2O4

b. PO5 d. P2O5

__D__ 76. The molar mass of an element is the mass of onea. atom of the element. c. gram of the element.b. crystal of the element. d. mole of the element.

__D__ 77. What is the formula mass of (NH4)2SO4?a. 114.09 amu c. 128.06 amub. 118.34 amu d. 132.16 amu

__D__ 78. The molar mass of CS2 is 76.15 g/mol. How many grams of CS2 are present in 10.00 mol?a. 0.13 g c. 10.00 gb. 7.614 g d. 761.5 g

_C___ 79. The molar mass of NH3 is 17.03 g/mol. How many moles of NH3 are present in 107.1 g?a. 0.1623 mol c. 6.289 molb. 3.614 mol d. 107.1 mol

__B__ 80. What is the mass of 0.240 mol glucose, C6H12O6?a. 24.0 g c. 180.16 gb. 43.2 g d. 750. g

__C__ 81. How many Cl– ions are present in 2.00 mol of KCl?a. 1.20 1024 c. 2.00b. 6.02 1024 d. 0.5

_B___ 82. How many OH– ions are present in 3.00 mol of Ca(OH)2?a. 3.00 c. 3.61 1024

b. 6.00 d. 2.06 1023

__A__ 83. How many molecules are there in 5.0 g of methyl alcohol, CH3OH?a. 9.4 1022 c. 3.6 1024

b. 3.0 1024 d. 3.8 1024

_B___ 84. What is the percentage composition of CF4?a. 20% C, 80% F c. 16.8% C, 83.2% Fb. 13.6% C, 86.4% F d. 81% C, 19% F

__C__ 85. The empirical formula for a compound shows the symbols of the elements with subscripts indicating thea. actual numbers of atoms in a molecule.b. number of moles of the compound in 100 g.c. smallest whole-number ratio of the atoms.d. atomic masses of each element.

__A__ 86. The empirical formula may not represent the actual composition of a unit of a(n)a. ionic compound. c. salt.b. molecular compound. d. crystal.

_B___ 87. What is the empirical formula for a compound that is 53.3% O and 46.7% Si?a. SiO c. Si2Ob. SiO2 d. Si2O3

__A__ 88. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?a. H2O c. HO2

b. H2O2 d. HO

__C__ 89. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?a. CHO c. C3H4O3

b. CH2O d. C2H4O2

___D_ 90. What is the small whole number that appears in front of a formula in a chemical equation?a. a subscript c. a ratiob. a superscript d. a coefficient

_C___ 91. In the chemical equation 2Mg(s) + O2(g) ? 2MgO(s),a. Mg represents the product magnesium. c. Mg represents the reagent magnesium.b. the reaction yields magnesium. d. O2 represents the product oxygen gas.

__C__ 92. A chemical formula written over the arrow in a chemical equation signifiesa. a by-product. c. a catalyst for the reaction.b. the formation of a gas. d. an impurity.

__D__ 93. Which equation is not balanced?a. 2H2 + O2 2H2Ob. 4H2 + 2O2 4H2Oc. H2 + H2 + O2 H2O + H2Od. 2H2 + O2 H2O

__D__ 94. In what kind of reaction do two or more substances combine to form a new compound?a. decomposition reaction c. double-displacement reactionb. ionic reaction d. synthesis reaction

__B__ 95. The equation AX A + X is the general equation for aa. synthesis reaction. c. combustion reaction.b. decomposition reaction. d. single-displacement reaction.

___A_ 96. In what kind of reaction does one element replace a similar element in a compound?a. displacement reaction c. decomposition reactionb. combustion d. ionic reaction

_A___ 97. In what kind of reaction does a single compound produce two or more simpler substances?a. decomposition reaction c. single-displacement reactionb. synthesis reaction d. ionic reaction

__C__ 98. In one type of synthesis reaction, an element combines with oxygen to yield a(n)a. acid. c. oxide.b. hydroxide. d. metal.

__A__ 99. The decomposition of a substance by an electric current is calleda. electrolysis. c. ionization.b. conduction. d. transformation.

__A__100. An active metal and a halogen react to form a(n)a. salt. c. acid.b. hydroxide. d. oxide.

__B__101. Many metal hydroxides decompose when heated to yield metal oxides anda. metal hydrides. c. carbon dioxide.b. water. d. an acid.

__C__102. In the equation 2Al(s) + 3Fe(NO3)2(aq) 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced bya. nitrate. c. aluminum.b. water. d. nitrogen.

__B__103. A precipitate may form in a double-displacement reaction whena. hydrogen gas reacts with a metal.b. positive ions combine with negative ions.c. water boils out of the solution.d. a gas escapes.

__D__104. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the solution isa. a halogen. c. not on the activity series.b. higher on the activity series. d. unreactive.

_A___105. Predict what happens when lead is added to nitric acid.a. No reaction occurs. c. Lead oxide forms.b. Oxygen is released. d. Hydrogen is released.

__C__106. Which of the following would be investigated in reaction stoichiometry?a. the masses of hydrogen and oxygen in waterb. the amount of energy released in chemical reactionsc. the mass of potassium required to produce a known mass of potassium chlorided. the types of bonds that break and form when acids react with metals

__B__107. The coefficients in a chemical equation represent thea. masses, in grams, of all reactants and products.b. relative numbers of moles of reactants and products.c. number of atoms in each compound in a reaction.d. number of valence electrons involved in the reaction.

_A___108. A balanced chemical equation allows one to determine thea. mole ratio of any two substances in the reaction.b. energy released in the reaction.c. electron configuration of all elements in the reaction.d. mechanism involved in the reaction.

_B___109. A chemical equation is balanced when thea. coefficients of the reactants equal the coefficients of the products.b. same number of each kind of atom appears in the reactants and in the products.c. products and reactants are the same chemicals.d. subscripts of the reactants equal the subscripts of the products.

_A___110. If one knows the mass and molar mass of reactant A and the molar mass of product D in a chemical reaction, one can determine the mass of product D produced by using thea. mole ratio of D to A from the chemical equation.b. group numbers of the elements of A and D in the periodic table.c. estimated bond energies involved in the reaction.d. electron configurations of the atoms in A and D.

__C__111. In the reaction represented by the equation N2 + 3H2 2NH3, what is the mole ratio of hydrogen to ammonia?a. 1:1 c. 3:2b. 2:1 d. 6:8

_C___112. For the reaction represented by the equation 2H2 + O2 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?a. 2.0 mol c. 12 molb. 6.0 mol d. 18 mol

__D__113. For the reaction represented by the equation 2H2 + O2 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?a. 2.00 g c. 54.0 gb. 6.00 g d. 108 g

__D__114. For the reaction represented by the equation SO3 + H2O H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid in an excess of water?a. 80.0 g c. 240. gb. 160. g d. 320. g

__C__115. For the reaction represented by the equation Cl2 + 2KBr 2KCl + Br2, how many grams of potassium chloride can be produced from 300. g each of chlorine and potassium bromide?a. 98.7 g c. 188 gb. 111 g d. 451 g

__C__116. To determine the limiting reactant in a chemical reaction, one must know thea. available amount of one of the reactants. c. available amount of each reactant.b. amount of product formed. d. speed of the reaction.

_A___117. After calculating the amount of reactant B required to completely react with A, then comparing that amount with the amount of B available, one can determine thea. limiting reactant. c. energy released in the reaction.b. rate of the reaction. d. pathway of the reaction.

__D__118. For the reaction represented by the equation SO3 + H2O H2SO4, calculate the percentage yield if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid.a. 82.7% c. 91.2%b. 88.3% d. 93.9%

_D___119. For the reaction represented by the equation Mg + 2HCl H2 + MgCl2, calculate the percentage yield of magnesium chloride if 100. g of magnesium react with excess hydrochloric acid to yield 330. g of magnesium chloride.a. 71.8% c. 81.6%b. 74.3% d. 84.2%

__D__120. The kinetic-molecular theory explains the behavior ofa. gases only. c. liquids and gases only.b. solids and liquids only. d. solids, liquids, and gases.

_A___121. A real gasa. does not obey all the assumptions of the kinetic-molecular theory.b. consists of particles that do not occupy space.c. cannot be condensed.d. cannot be produced in scientific laboratories.

_A___122. What determines the average kinetic energy of the molecules of any gas?a. temperature c. container volumeb. pressure d. molar mass

_B___ 123 Which is an example of gas diffusion?a. inflating a flat tireb. the odor of perfume spreading throughout a roomc. a cylinder of oxygen stored under high pressured. All of the above

__A__124. Forces holding particles together are strongest in aa. solid. c. gas.b. liquid. d. vapor.

_A___125. Compared with a crystalline solid, the particles in an amorphous solida. occur in a random pattern.b. occur in a definite, three-dimensional arrangement.c. consist of molecular sheets.d. have a more complex unit cell.

_D___126. Which of the following is an amorphous solid?a. ice c. graphiteb. diamond d. glass

__B__127. Which of the following is a crystalline solid?a. a plastic milk container c. a glass bottleb. a quartz rock d. a three-dimensional glass cube

__B__128. What is the total three-dimensional array of points that describes the arrangement of the particles of a crystal called?a. unit cell c. diffraction patternb. crystal lattice d. crystalline system

__D__129. If the rate of evaporation from the surface of a liquid exceeds the rate of condensation,a. the system is in equilibrium.b. the liquid is boiling.c. energy as heat is no longer available.d. the concentration of the vapor is increasing.

__B__130. At its triple point, water cana. have only three pressure values.b. exist in equilibrium in three different phases.c. only be present as vapor.d. exist only as a solid.

_B___131. The equilibrium vapor pressure of water isa. constant at all temperatures.b. specific for any given temperature.c. unrelated to temperature.d. inversely proportional to the temperature.

__A__ 132 Whenever a liquid changes to a vapor, ita. absorbs energy from its surroundings. c. is boiling.b. is in equilibrium with its vapor. d. is condensing.

__A__133. During boiling, the temperature of a liquida. remains constant. c. decreases.b. increases. d. approaches water's boiling point.

_A___134. During the process of freezing, a liquida. loses kinetic energy. c. gains potential energy.b. loses potential energy. d. gains kinetic energy.

_D___135. The molar enthalpy of fusion for water is 6.008 kJ/mol. What quantity of energy is released when 253 g of liquid water freezes? (Molar mass of water is 18.02 g/mol.)a. 759 kJ c. 2.33 kJb. 0.429 kJ d. 84.4 kJ

__B__136. Why does a can collapse when a vacuum pump removes air from the can?a. The inside and outside forces balance out and crush the can.b. The unbalanced outside force from atmospheric pressure crushes the can.c. The atmosphere exerts pressure on the inside of the can and crushes it.d. The vacuum pump creates a force that crushes the can.

_C___137. To correct for the partial pressure of water vapor in a gas collection bottle, the vapor pressure of H2O at the collecting temperature is generallya. subtracted from the partial pressure of the collected gas.b. added to the pressure of the collected gas.c. subtracted from the atmospheric pressure.d. added to the atmospheric pressure.

_D___138. A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm Hg?a. 80.0 mL c. 600. mLb. 490. mL d. 640. mL

__C__139. If the temperature of a fixed quantity of gas decreases and the pressure remains unchanged,a. its volume increases. c. its volume decreases.b. its volume is unchanged. d. its density decreases.

__B__140. At 7.0C, the volume of a gas is 49 mL. At the same pressure, its volume is 74 mL at what temperature?a. 3.0C c. 120Cb. 423C d. 150C

__B__141. On a cold winter morning when the temperature is –13C, the air pressure in an automobile tire is 1.5 atm. If the volume does not change, what is the pressure after the tire has warmed to 15C?a. –1.5 atm c. 3.0 atmb. 1.7 atm d. 19.5 atm

_B___ 142 The pressure of a sample of gas at 10.0C increases from 700. mm Hg to 900. mm Hg. What is the new temperature?a. 0C c. 39.0Cb. 364C d. 90.9C

_C___143. The volume of a sample of oxygen is 300.0 mL when the pressure is 1.00 atm and the temperature is 27.0C. At what temperature is the volume 1.00 L and the pressure 0.500 atm?a. 22.0C c. 0.50 Kb. 45.0C d. 227C

__C__144. The volume of a gas collected when the temperature is 11.0C and the pressure is 710 mm Hg measures 14.8 mL. What is the calculated volume of the gas at 20.0C and 740 mm Hg?a. 7.8 mL c. 14.6 mLb. 13.7 mL d. 15 mL

__C__ 145. Volumes of gaseous reactants and products in a chemical reaction can be expressed as ratios of small whole numbersa. if all reactants and products are gases.b. if standard temperature and pressure are maintained.c. if constant temperature and pressure are maintained.d. if each mass equals 1 mol.

_B___146. If the pressure and temperature of a gas are held constant and some gas is added to the container or some is allowed to escape, a change is which of the following can be observed?a. kinetic energy c. rate of diffusionb. volume d. chemical properties

_A___147. Calculate the approximate volume of a 0.600 mol sample of gas at 15.0°C and a pressure of 1.10 atm.a. 12.9 L c. 24.6 Lb. 22.4 L d. 139 L

__C__148. How many times greater is the rate of effusion of molecular fluorine than that of molecular bromine at the same temperature and pressure?a. 2.051 c. 4.450b. 3.062 d. 7.280

__D__149. A sample of helium diffuses 4.57 times faster than an unknown gas diffuses. What is the molar mass of the unknown gas?a. 12 g/mol c. 38.8 g/molb. 18.2 g/mol d. 83.5 g/mol

_D___150. A sample of hydrogen gas diffuses 3.8 times faster than an unknown gas diffuses. What is the molar mass of the unknown gas?a. 4.0 g/mol c. 22 g/molb. 7.6 g/mol d. 29 g/mol

_C___151. Colloidsa. can be separated by filtering. c. scatter light.b. settle out when allowed to stand. d. contain particles larger than 1000 nm.

_D___152. The solubility of a substance at a given temperature is generally expressed asa. amount of solute.b. amount of solvent.c. amount of solute per amount of solvent.d. amount of water per 100 g of solute.

_A___153. In a solution, the slightly charged part of a water moleculea. attracts the ions in ionic compounds.b. forms ionic bonds with ions in ionic compounds.c. attracts nonpolar molecules.d. forms ionic bonds with other water molecules.

_A___154. Which of the following is soluble in water?a. potassium nitrate c. benzeneb. silver d. carbon tetrachloride

__D__155. Two immiscible substancesa. exist together in one phase.b. will not separate on standing.c. dissolve freely in one another in any proportion.d. will not form a solution.

_C___156. During the dissolving process, which particles interact?a. solute only c. solute and solventb. solvent only d. None of the above

__D__157. Pressure has the greatest effect on the solubility ofa. solids in liquids. c. gases in gases.b. liquids in liquids. d. gases in liquids.

__B__158. Which of the following expresses concentration?a. molality c. moles of solute per liter of solutionb. molarity d. All of the above

__C__159. What is the molality of a solution that contains 31.0 g HCl in 5.00 kg water? (molar mass of HCl = 36.46 g/mol)a. 0.062 m c. 0.170 mb. 0.425 m d. 15.5 m

Use the table below to answer the following questions.

General Solubility Guidelines1. Most sodium, potassium, and ammonium compounds are soluble in water.2. Most nitrates, acetates, and chlorates are soluble.3. Most chlorides are soluble, except those of silver, mercury(I), and lead. Lead(II) chloride is soluble

in hot water.4. Most sulfates are soluble, except those of barium, strontium, and lead.5. Most carbonates, phosphates, and silicates are insoluble, except those of sodium, potassium, and

ammonium.6. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and

ammonium.

__D__160. Which of the following pairs of solutions produces a precipitate when combined?a. KOH and NH4Cl c. Na2SO4 and KClb. Fe(NO)3 and KCl d. NH4Cl and AgNO3

__D__161. Which of the following is a weak electrolyte?a. hydrogen chloride c. sodium chlorideb. sugar d. acetic acid

__C__162. A 15 M acetic acid solution isa. concentrated and a strong electrolyte. c. concentrated and a weak electrolyte.b. dilute and a strong electrolyte. d. dilute and a weak electrolyte.

__A__163. Why is freezing-point depression a colligative property?a. It is inversely proportional to the molal concentration of a solution.b. It is directly proportional to the molal concentration of a solution.c. It does not depend on a molal freezing-point constant for each solvent.d. It depends on the properties of an electrolyte in a solvent.

__A__164. Which acid is found in vinegar?a. acetic acid c. phosphoric acidb. nitric acid d. hydrochloric acid

__A__165. The traditional definition of acids is based on the observations ofa. Brønsted and Lowry. c. Arrhenius.b. Lewis. d. Mendeleev.

__D__166. Which of the following did Arrhenius theorize?a. An acid increases the concentration of OH– ions in solution.b. A base increases the concentration of H+ ions in solution.c. Acids and bases contain nonpolar molecules.d. Because acids and bases carry electric current, they must produce ions in solution.

__C__167. An electron-pair acceptor is a(n)a. Brønsted-Lowry base. c. Lewis base.b. Lewis acid. d. Arrhenius acid.

_B___168. In the reaction represented by the equation , a conjugate acid-base pair is a. F– and H2O. c. H3O+ and HF.b. HF and F–. d. HF and H2O.

_A___169. In the equation , H2O is a weak base and H3O+ is a a. strong acid. c. weak acid.b. strong base. d. weak base.

_C___170. An amphoteric species is one that reacts as a(n)a. acid only. c. acid or base.b. base only. d. None of the above

__B__171. What is the product of H3O+ ion and OH– ion concentrations in water?a. 10–28 c. 10–7

b. 10–14 d. 55.4

_C___172. Which expression represents the concentration of H3O+ ions in solution?a. 10–14 – [OH–] c. 10–14 [OH–]b. 10–14 [OH–] d. [OH–] 10–14

__B__173. The pH of an acidic solution isa. less than 0. c. greater than 7.b. less than 7. d. greater than 14.

__D__ 174 How would you classify KOH in the equation below?

a. a weak acid c. a weak baseb. a strong acid d. a strong base

__D__175. What is the hydronium ion concentration of a solution whose pH is 4.12?a. 4.4 10–8 M c. 6.4 10–5 Mb. 5.1 10–6 M d. 7.6 10–5 M

_C___176. What is the hydronium ion concentration of a solution whose pH is 7.30?a. 1.4 10–11 M c. 5.0 10–8 Mb. 3.8 10–8 M d. 7.1 10–6 M

__A__177. Which indicator is used to study neutralizations of strong acids with strong bases?a. phenolphthalein c. bromthymol blueb. methyl orange d. None of the above

__D__178. What process measures the amount of a solution of known concentration required to react with a measured amount of a solution of unknown concentration?a. autoprotolysis c. neutralizationb. hydrolysis d. titration

__C__179. In an acid-base titration, equivalent quantities of hydronium ions and hydroxide ions are presenta. at the beginning point. c. at the end point.b. at the midpoint. d. throughout the titration.

__A__180. A standard solution always containsa. a known concentration of solute. c. a base.b. an acid. d. a primary standard.

_C___181. Balance the following equation: ____ + a. c.

b. d.

__A__182. Beta particles area. electrons. c. electromagnetic waves.b. helium nuclei. d. neutrons.

__B__183. Which is not a parent nuclide?a. uranium-238 c. uranium-235b. lead-206 d. thorium-232

__C__184. Artificial radioactive nuclides area. found naturally in space. c. not found naturally on Earth.b. found naturally on Earth. d. nonexistent.

__C__185. Which of the following has the greatest penetrating ability?a. alpha particles c. gamma raysb. beta particles d. All have the same penetrating ability.

__D__186. Which of the following does not detect radiation?a. film badges c. scintillation countersb. Geiger-Müller counters d. radioactive tracers

__B__187. Which of the following instruments detect radiation by counting electric pulses carried by gas atoms ionized by radiation?a. film badges c. scintillation countersb. Geiger-Müller counters d. radioactive tracers

__D__188. How do radioactive nuclides affect photographic film wrapped in lightproof paper?a. They have no effect on the film. c. They melt the film.b. They disintegrate the film. d. They expose the film.

__D__189. Radioactive tracers are used toa. measure the energy of nuclear reactions.b. calculate the half-life of a nuclide.c. estimate the age of a material.d. follow the movement of substances in a system.

__D__190. Which of the following is a fusion reaction?a. uranium-235 absorbing a neutron and splitting into xenon-140, strontium-94, and two neutronsb. hydrochloric acid combining with sodium hydroxide to form NaCl and waterc. carbon-14 decaying into nitrogen-14 and a beta particled. curium-246 combining with carbon-12 to form nobelium-254 and four neutrons

__B__191. What is the function of shielding in a nuclear reactor?a. to cool the reactor c. to absorb free neutronsb. to contain radiation d. to slow neutrons

__C__192. Carbon atoms readily join with atoms ofa. metals. c. both other elements and carbon.b. carbon only. d. nonmetals.

_D___193. What do all organic compounds contain?a. hydrogen c. oxygenb. water d. carbon

__C__194. The diversity of organic compounds is so great because carbona. has many allotropes. c. compounds have many isomers.b. has many isotopes. d. compounds are very reactive.

__A__195. The carbon-hydrogen bonds of alkanes area. polar. c. double bonds.b. nonpolar. d. ionic bonds.

__A__196. Hydrocarbons in which carbon atoms form only single bonds and are arranged in a ring are calleda. cycloalkanes. c. alkenes.b. alkynes. d. aromatic hydrocarbons.