Sample Test Questions Chemistry Washington Educator Skills Tests The Washington Professional
Transcription
Sample Test Questions Chemistry Washington Educator Skills Tests The Washington Professional
The Washington Professional Educator Standards Board Washington Educator Skills Tests Sample Test Questions Chemistry WA-SG-FLD023-02 Washington Educator Skills Tests—Endorsements (WEST–E) SAMPLE TEST QUESTIONS The sample test questions in this document are designed to give you an introduction to the nature of the questions included in the Washington Educator Skills Tests—Endorsements (WEST–E). They represent the various types of questions you may expect to see on an actual test in this test field; however, they are not designed to provide diagnostic information to help you identify specific areas of individual strength or weakness or to predict your performance on the test as a whole. Work through the sample questions carefully before referring to the answer key that follows. The answer key provides the correct response for each question and lists the objective within the test framework to which each question is linked. When you are finished with the sample questions, you may wish to review the test objectives and descriptive statements provided in the test framework for this test field. In addition to reading and answering the sample questions, you should also utilize the following preparation materials available on the WEST Web site: Read WEST–E Test-Taking Strategies to understand how test questions are designed to measure specific test objectives and to learn important test-taking strategies for the day of the test. Review the Test Summary and Framework for your test field to familiarize yourself with the structure and content of the test. This document contains general testing information as well as the percentage of the total test score derived from each content domain described in the test framework. Please note that a periodic table, a set of constants, and a set of formulas are provided for this test. Please refer to these materials as needed in responding to the sample test questions. These materials are located in the Reference Materials section at the end of this document. A scientific calculator may be used for this test as needed in responding to the sample test questions, and one will be provided at the test administration. Please refer to the current WEST registration information regarding the use of calculators at the test administration. Readers should be advised that this document, including many of the excerpts used herein, is protected by federal copyright law. Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 Pearson and its logo are trademarks in the U.S. and/or other countries of Pearson Education, Inc. or its affiliate(s). —1— SAMPLE TEST QUESTIONS Chemistry SAMPLE MULTIPLE-CHOICE QUESTIONS 1. A chemist has determined that an unknown sample has a high melting point, is ductile, and forms hydrogen gas and a salt when reacted with HCl acid. Based on these findings, the unknown sample is also likely to: A. 2. 3. Rutherford's gold foil experiment provided evidence that led to which of the following conclusions about atomic structure? A. Electrons exist only in certain discrete energy levels. B. Atoms contain small densely packed nuclei. C. The exact location of an electron at any given time cannot be determined. D. Atoms display the properties of both particles and waves. have a high electronegativity value. B. be brittle at room temperature. C. have a dull appearance. D. be a good conductor of electricity. In which of the following sets of elements are the elements arranged in order of increasing atomic radius? A. Po, Sb, Ge B. Li, Na, K C. Si, P, S D. Br, Cl, F Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —2— SAMPLE TEST QUESTIONS Chemistry 4. Use the reactions below to answer the question that follows. 235 92U 236 92U + 10n A A 141 56Ba 6. Use the diagram below to answer the question that follows. Phase Diagram for a Compound 236 92U 500 1 + 92 36K + 3 0n 400 5. A. the medical treatment of cancer B. the dating of archaeological artifacts C. the production of electricity D. the irradiation of food products Ethanol has a specific heat of 2.45 J/g•K and a density of 0.7893 g/cm3. How much heat is required to raise the temperature of 100.0 mL of ethanol from 5.0°C to 20.0°C? A. 2.90 kJ B. 3.68 kJ C. 55.7 kJ D. 70.6 kJ Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 300 Pressure (mm Hg) The reactions described in the equations above are used in which of the following applications? 200 100 50 40 30 20 10 0 –25 X 0 25 50 75 Temperature (°C) 100 Which of the following changes will lead to the sublimation of the sample at point X on the phase diagram above? A. increasing the pressure to 500 mm Hg B. decreasing the temperature to –5.0°C C. increasing the temperature to 100.0°C D. decreasing the pressure to 5 mm Hg —3— SAMPLE TEST QUESTIONS Chemistry 7. Use the information below to answer the question that follows. A 2CuO(s) + 2H2(g) 1 Cu(s) + 2 O2(g) 1 H2(g) + 2 O2(g) 2Cu(s) + 2H2O(B) A CuO(s) ΔH°f = –156.1 kJ/mol A H2O(B) ΔH°f = –285.8 kJ/mol Given the balanced equations and standard molar enthalpies of formation shown above, what will be the standard enthalpy ° ) for the reaction between change (ΔHrxn copper oxide and hydrogen? A. –259.4 kJ B. –441.9 kJ C. –883.8 kJ D. –1320 kJ Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —4— SAMPLE TEST QUESTIONS Chemistry 8. Use the table below to answer the question that follows. Molecule Molecular Geometry Molecular Polarity CH4 trigonal pyramidal polar CO2 linear nonpolar NH3 tetrahedral polar H2O bent nonpolar In the table above, which molecule is matched with its correct molecular geometry and molecular polarity? A. CH4 B. CO2 C. NH3 D. H2O Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —5— SAMPLE TEST QUESTIONS Chemistry 9. Use the table below to answer the question that follows. Line Chemical Formula IUPAC Name 1 Fe2O3 iron(II) trioxide 2 CH3CO2 methylcarbonate ion 3 CH3CH2CH3 propane 4 PCl5 phosphorus chloride – Which line in the table above correctly matches a chemical formula with its IUPAC name? A. Line 1 B. Line 2 C. Line 3 D. Line 4 Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —6— SAMPLE TEST QUESTIONS Chemistry 10. Use the equation below to answer the question that follows. Ca(OH)2(s) + H2SO4(aq) A CaSO4 • 2H2O(s) The equation above describes a process commonly used by coal-fueled power plants to remove sulfur oxides present in exhaust gases. This is an example of which of the following types of chemical reactions? A. combustion B. single replacement C. neutralization D. decomposition Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —7— SAMPLE TEST QUESTIONS Chemistry 11. Use the information below to answer the question that follows. Reaction of Nitrogen Dioxide and Carbon Monoxide overall reaction: NO2(g) + CO(g) A NO(g) + CO2(g) step 1 of reaction mechanism: NO2(g) + NO2(g) A NO3(g) + NO(g) At low temperatures, the reaction between nitrogen dioxide and carbon monoxide occurs in two steps. Given the information shown above, which of the following reactions is step 2 of the reaction mechanism? A. NO3(g) + NO(g) A N2O4(g) B. NO3(g) + CO(g) A NO2(g) + CO2(g) C. NO(g) + NO2(g) A 2NO(g) D. NO(g) + CO(g) A N(g) + CO2(g) Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —8— SAMPLE TEST QUESTIONS Chemistry 12. Use the reaction below to answer the question that follows. N2(g) + 3H2(g) f 2NH3(g) The Haber-Bosch process used in the commercial synthesis of ammonia from nitrogen and hydrogen is shown above. The process includes a condensation step in which the ammonia gas produced is condensed into a liquid. Which of the following best describes the role this condensation step plays in the process? A. Reducing the concentration of ammonia gas shifts the equilibrium to the right, driving the formation of more product. B. Removing ammonia gas from the system lowers the activation energy of the synthesis reaction. C. Condensing the ammonia gas into its liquid state removes contaminants that may have been introduced into the system. D. Converting ammonia gas to a liquid increases the equilibrium constant, leading to a greater yield of product. 13. Use the information below to answer the question that follows. 2Fe3+(aq) + 2I –(aq) A Standard Reduction Potentials (at 25°C) Half-reaction Fe3+(aq) + e– I2(s) + 2e– A A Fe2+(aq) 2 I–(aq) E°(V) 0.769 0.534 The net ionic equation for the reaction between iron(III) ions and iodide ions and the standard reduction potentials for the related half-reactions are shown above. Given the value for the Faraday constant of F = 9.648 × 104 J/mol•V, what will be the standard free-energy change (ΔG°) for this reaction at 25°C? A. –22.7 kJ B. –45.3 kJ C. –90.6 kJ D. Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 2Fe2+(aq) + I2(s) –251 kJ —9— SAMPLE TEST QUESTIONS Chemistry 14. Use the diagrams below to answer the question that follows. C Use the table below to answer the question that follows. H H NH2 15. COOH H NH2 C Ascorbic Acid (molar mass = 176.1 g/mol) COOH CH2 OH Percent by Mass of Component Elements Component Elements of Ascorbic Acid 54.5 oxygen 40.9 carbon 4.6 hydrogen The two amino acids shown above can be joined together using which of the following chemical reactions? A. esterification B. substitution C. combustion D. condensation Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 The table above gives the molar mass of ascorbic acid and the percent by mass of its component elements. Given this information, what is the molecular formula for ascorbic acid? A. C3H4O3 B. C6H6O6 C. C9H12O9 D. C6H8O6 —10— SAMPLE TEST QUESTIONS Chemistry 16. Use the reaction below to answer the question that follows. CO(g) + 2H2(g) A CH3OH(B) 534 g CO and 98.0 g H2 are combined to form methanol according to the reaction above. What mass of the excess reactant remains after all of the limiting reactant has been consumed? A. 21.2 g B. 59.7 g C. 98.2 g D. 338 g Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 17. Scuba divers that surface too quickly after spending time at depths greater than 15 m need to take precautions during their ascent to prevent the formation of nitrogen gas bubbles in the bloodstream. This problem experienced by divers is most similar to which of the following physical phenomena? A. The boiling point of water is increased by dissolving table salt in the water. B. The air molecules in a balloon expand the volume of the balloon as it rises into the atmosphere, where atmospheric pressure is lower. C. The adiabatic warming of an air mass occurs as the air is compressed. D. The dissolved carbon dioxide in soda comes out of solution when the pressure is decreased as the bottle is opened. —11— SAMPLE TEST QUESTIONS Chemistry 18. Use the chart below to answer the question that follows. Emissions Data for Four Experimental Fuel Additives additive 1 Emissions (as a percent of control) 100 90 additive 2 80 70 60 50 additive 3 40 30 additive 4 20 10 0 0 10 20 30 40 Speed (mph) 50 60 A research chemist has synthesized four fuel additives designed to reduce auto emissions. The experimental fuel additives were added to commercial gasoline and emissions data were collected for speeds ranging from 5 mph to 65 mph. The collected data were graphed in the above chart to show the effectiveness of each additive at different speeds. Which of the following conclusions is best supported by the results shown in the chart? A. Additive 1 demonstrates the greatest increase in fuel efficiency over the widest range of driving speeds. B. Additives 2 and 4 have the same effect on emissions if all driving speeds are considered. C. Additive 4 is most effective at reducing emissions at speeds greater than 50 mph. D. Additive 3 produces the greatest average reduction in emissions when all driving speeds are considered. Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —12— SAMPLE TEST QUESTIONS Chemistry 19. Read the newspaper article below; then answer the question that follows. New Energy Source Could End Country's Reliance on Fossil Fuels By providing abundant and clean energy, a newly discovered fusion process promises to dramatically reduce the country's reliance on fossil fuels. Researchers at a leading university announced that they have succeeded in producing abundant energy through a relatively inexpensive fusion process. With the world's reliance on fossil fuels implicated as a major cause of global warming, many people have proclaimed the discovery as one of the most important of our time. The researchers who worked on the project said that many existing power plants could be retrofitted with the new technology, reducing both the environmental and political problems associated with the country's dependence on fossil fuels. The newspaper article shown above describes the discovery of a new process for producing energy. In evaluating whether the researchers' claims about this fusion process are valid, which of the following questions is it most important to consider? A. Have the researchers released information on the source of funds used to develop the process? B. Will the process announced by the researchers provide affordable energy to the average consumer? C. Have the researchers' claims about the process been evaluated by scientists not connected to the project? D. Will the raw materials required to carry out the process be available to underdeveloped countries? Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —13— SAMPLE TEST QUESTIONS Chemistry 20. Use the diagram below to answer the question that follows. H2SO4 and water solution 6 V battery A scientist plans to set up and use the apparatus shown in the diagram above to decompose water by electrolysis. Which of the following aspects of setting up and using this apparatus represents the most serious safety hazard? A. the removal of insulation from the ends of the wires B. the addition of sulfuric acid to the water in the beaker C. the connection of the wires to the terminals of the 6 V battery D. the displacement of water within the inverted test tubes Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —14— SAMPLE TEST QUESTIONS Chemistry ANSWER KEY Question Number Correct Response Test Objective 1 D 0001 2 B 0002 3 B 0003 4 C 0004 5 A 0005 6 D 0006 7 A 0007 8 B 0008 9 C 0010 10 C 0011 11 B 0012 12 A 0013 13 B 0014 14 D 0016 15 D 0017 16 A 0018 17 D 0019 18 D 0020 19 C 0021 20 B 0022 Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —15— SAMPLE TEST QUESTIONS Chemistry REFERENCE MATERIALS Please use the reference materials on the following pages as needed in responding to the sample test questions. These materials will also appear in test booklets. Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —16— Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —17— 5 15 90 Th 232.0 89 Ac (227) Actinide Series 91 Pa 231.0 59 Pr 140.9 92 U 238.0 93 Np (237) 94 Pu (244) 95 Am (243) 111 96 Cm (247) 112 97 Bk (247) 113 98 Cf (251) 114 99 Es (252) 115 16 100 Fm (257) 116 84 Po (209) 17 101 Md (258) 117 85 At (210) 102 No (259) 118 86 Rn (222) 54 Xe 131.3 36 Kr 83.8 18 Ar 39.9 10 Ne 20.18 103 Lr (262) 71 Lu 175.0 53 I 126.9 35 Br 79.9 17 CI 35.5 9 F 19.00 VIIA 70 Yb 173.0 52 Te 127.6 34 Se 79.0 16 S 32.1 8 O 16.00 VIA 69 Tm 168.9 83 Bi 209.0 51 Sb 121.8 33 As 74.9 15 P 31.0 7 N 14.01 VA 68 Er 167.3 82 Pb 207.2 50 Sn 118.7 32 Ge 72.6 14 Si 28.1 67 Ho 164.9 81 TI 204.4 49 In 114.8 31 Ga 69.7 66 Dy 162.5 80 Hg 200.6 48 Cd 112.4 30 Zn 65.4 IIB 65 Tb 158.9 79 Au 197.0 47 Ag 107.9 29 Cu 63.5 IB 64 Gd 157.3 110 Ds (271) 78 Pt 195.1 46 Pd 106.4 28 Ni 58.7 63 Eu 152.0 109 Mt (268) 77 Ir 192.2 45 Rh 102.9 27 Co 58.9 VIIIB 62 Sm 150.4 108 Hs (277) 76 Os 190.2 44 Ru 101.1 26 Fe 55.8 61 Pm (145) 107 Bh (264) 75 Re 186.2 43 Tc (98.9) 25 Mn 54.9 VIIB 60 Nd 144.2 106 Sg (266) 74 W 183.9 42 Mo 95.9 24 Cr 52.0 VIB 13 AI 27.0 6 C 12.01 IVA Some of the elements 111 and above have been reported but not fully authenticated and named. 58 Ce 140.1 105 Db (262) 57 La 138.9 104 Rf (261) 73 Ta 180.9 41 Nb 92.9 23 V 50.9 Lanthanide Series 89–103 72 Hf 178.5 40 Zr 91.2 22 Ti 47.9 VB 88 Ra (226) 57–71 39 Y 88.9 21 Sc 45.0 IVB IIIB 87 Fr (223) 12 56 Ba 137.3 11 55 Cs 132.9 10 38 Sr 87.6 9 37 Rb 85.5 8 20 Ca 40.1 7 19 K 39.1 4 12 Mg 24.3 11 Na 23.0 3 4 Be 9.01 3 Li 6.94 5 B 10.81 IIIA IIA 6 14 2 He 4.00 13 2 VIIIA IA 1 H 1.01 18 1 PERIODIC TABLE OF THE ELEMENTS CONSTANTS Description Value Avogadro's number 6.02 × 1023/mol Molar gas volume at STP 22.4 L Ideal gas constant (R) 0.0821 L•atm/mol•K = 8.31 J/mol•K Molal freezing point depression constant for water (Kf) 1.86°C/m Molal boiling point elevation constant for water (Kb) 0.52°C/m Heat of fusion of water (ΔHfus) 334 J/g = 80 cal/g Heat of vaporization of water (ΔHvap) 2260 J/g = 540 cal/g Specific heat (s) of liquid water 4.18 J/g•°C = 1.0 cal/g•°C Specific heat (s) of water vapor 2.09 J/g•°C = 0.50 cal/g•°C Specific heat (s) of solid water 2.11 J/g•°C = 0.50 cal/g•°C Standard atmospheric pressure (STP) 101.325 kPa = 760 mm Hg Planck's constant (h) 6.63 × 10– 34 J•s Speed of light in a vacuum (c) 3.00 × 108 m/s Dissociation constant of water (Kw) 1.0 × 10– 14 at 25°C FORMULAS Description Formula Ideal gas law PV = nRT Gibbs free energy equation ΔG = ΔH – TΔS Free energy of a redox reaction ΔG° = –nFE° Root-mean-square speed urms = Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 3RT M —18— FORMULAS (continued) Description Formula Photon energy E = hν Speed of light c = λν Amount of heat (q) q = msΔT Boyle's and Charles' laws combined P1V1 P2V2 T1 = T2 Graham's law of diffusion r1 r2 = M2 M1 NOTES FOR CHEMISTRY TEST Not all constants and formulas necessary are listed, nor are all constants and formulas listed used on this test. While attention has been paid to significant figures, no answer should be considered incorrect solely because of the number of significant figures. Copyright © 2009 Pearson Education, Inc. or its affiliate(s). All rights reserved. Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004 —19—
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