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C2A PT1 Multiple Choice Write you name and section number on both your test booklet and your Scantron Answer Sheet. Identify the choice that best completes the statement or answers the question and fill the space coresponding to your answer on your Scantron Answer Sheet. Be sure to erase mistakes completely. 1. Which of the following is not a step in the scientific method? a. Make an observation. b. Formulate a hypothesis. c. Perform an experiment. d. Change results to agree with your hypothesis. e. Develop a theory (or model). 2. Write 8,394 in standard scientific notation. a. 8394 b. 8.394 10–3 c. 839.4 101 d. 8.394 1000 e. 8.394 103 3. The number 0.002 expressed in exponential notation is a. 2 103 b. 2 104 c. 2 10–3 d. 2 10–4 e. none of these 4. 1.8 kilograms contain this many grams. a. b. c. d. e. 5. Convert: 6.0 mm = _____________ km. a. km b. c. d. e. km km km km 66. Using the rules of significant figures, calculate the following: 12.67 + 13.005 = a. b. c. d. e. 25.675 25 20 25.68 26 7. The number 3.00183 rounded to four significant figures is a. 3.002 b. 3.001 c. 3.000 d. 3.183 e. none of these 8. How many significant figures are in the number 1.20 103? a. 1 b. 2 c. 3 d. 4 e. 5 9. A student finds that the weight of an empty beaker is 14.049 g. She places a solid in the beaker to give a combined mass of 14.142 g. To how many significant figures is the mass of the solid known? a. 2 b. 3 c. 1 d. 5 e. 4 10. The result of the following calculation has how many significant figures? (0.4333 J/g °C) (33.12°C – 31.12°C)(412.1 g) a. 1 b. 2 c. 3 d. 4 e. 5 11. The product of 0.1400 6.02 1023 will have how many significant figures? a. 2 b. 3 c. 23 d. 1023 e. 7 12. How many significant figures are in the number 0.0040090? a. 8 b. 7 c. 6 d. 5 e. 4 17. Convert: –10.5°F = _______________ °C. a. –23.6°C b. 11.9°C c. –76.5°C d. 38.7°C e. 262.5°C 18. If 1.000 kg equals 2.205 lb, what is the mass in pounds of a human who weighs 51.35 kg? a. 113.2 lb b. 23.29 lb c. 93.2 lb d. 53.56 lb e. none of these 19. Find the volume of an object that has a density 13. Convert 316718.0 mm to kilometers. a. 3.167180 km b. 0.3167180 km c. 316.7180 km d. 3167.180 km e. km of 3.14 g/mL and a mass of 94.7 g. a. 30.2 mL b. mL c. 297 mL d. mL e. mL 14. Convert: 6.76 qt = ___________ mL. a. 7.17 mL b. mL 20. An experiment requires 74.2 mL of ethyl c. d. 6.38 mL e. mL mL 15. Convert: 2.80 in = _____________ mm. a. 71.1 mm b. 7.11 mm c. 1.102 mm d. 0.71 mm e. 711 mm alcohol. If the density of ethyl alcohol is 0.790 g/cm3, what is the mass of 74.2 mL of ethyl alcohol? a. 93.9 g b. 10.6 g c. 58.6 g d. g e. none of these 21.A graduated cylinder contains 20.0 mL of water. An 116.` Convert: 366.2 K = ________________ °C. a. 639.2°C b. 93.2°C c. 691.2°C d. 235.4°C e. 203.4°C irregularly shaped object is placed in the cylinder, and the water level rises to the 31.2-mL mark. If the object has a mass of 80.4 g, what is its density? a. 7.18 g/mL b. 0.139 g/mL c. 2.58 g/mL d. 4.02 g/mL e. none of these 22. Which of the following is a physical change? a. burning gasoline b. cooking an egg c. decomposing meat d. evaporating water e. rusting iron 28. The symbol for the element mercury is a. Hg b. Mg c. He d. Mn e. none of these 23. Which of the following is a chemical change? a. Water condenses on a mirror. b. A damp towel dries. c. Peanuts are crushed. d. A “tin” can rusts. e. At least two of the above (a-d) exhibit a 29. Si is the symbol for a. silver b. silicon c. selenium d. sodium e. sulfur chemical change. 24. Water is an example of a. a homogeneous mixture b. a heterogeneous mixture c. a compound d. an element 30. How many atoms of hydrogen are in five molecules of C5H6Cl? a. b. c. d. e. 30 5 x 1023 6 10 x 1023 6 x 1023 25. Which is an example of a homogeneous mixture? 31.The total number of atoms represented by the a. vodka formula Co3(PO4)2 is b. oily water a. 13 c. soil (dust) b. 11 d. sodium chloride c. 8 e. aluminum d. 17 26. Which of the following processes is a chemical e. 6 change? 32. Which atomic particle determines the chemical a. Dry ice sublimes when left on the demo behavior of an atom? table in lecture. a. proton b. The light on a candle burns until a bell jar is b. electron placed over it for a period of time. c. neutron c. When a few drops of red food coloring are d. nucleus added to a beaker of hot water, the water e. none of these immediately turns red. 33. An atom with 15 protons and 16 neutrons is an d. Liquid nitrogen dumped onto the floor atom of vaporizes at room temperature. a. P e. None of the above processes are chemical b. Ga changes. c. S 27. The symbol for the element iodine is d. Pd a. Io e. Rh b. In c. Id 34. A certain isotope X2+ contains 37 electrons and d. I 73 neutrons. What is the mass number for this e. Ie element? a. b. c. d. e. 112 110 108 39 35 35. How many neutrons are there in one atom of ? a. b. c. d. e. 22 24 46 68 none of these 36. Which of the following elements is an alkaline earth metal? a. b. c. d. e. Ra Au Gd Bi Cs 37. The correct name for LiCl is a. lithium monochloride b. lithium(I) chloride c. monolithium chloride d. lithium chloride e. monolithium monochloride 38. Which of the following formulas is incorrect? a. AlO3 b. KBr c. KNO3 d. Li2O e. CaSO4 39. A compound contains an unknown ion X and e. cyanous acid 41. The correct name for NiO is a. nickel(II) oxide b. nickel(I) oxide c. nickel oxide d. nickel monoxide e. nickel(I) monoxide 42. The name for the acid H2SO3 is a. sulfuric acid b. sulfurous acid c. hydrosulfuric acid d. hydrosulfurous acid e. sulfurite acid 43. The name for HClO3(aq) is a. chloric acid b. hydrogen chlorate c. perchloric acid d. hydrogen chlorate e. chlorous acid 44. The name for NaHCO3 is a. sodium hydrogen carbonate (sodium bicarbonate) b. sodium carbonate c. sodium(I) hydrogen carbonate d. sodium(I) bicarbonate e. none of these 45. The correct formula for iron(III) phosphide is a. Fe3P2 b. FeP c. Fe3P d. FeP3 e. Fe2P3 has the formula XCl2. Ion X contains 20 electrons. What is the identity of X? a. b. c. d. e. Ti2+ Sc+ Ca2+ Cr2+ Mn3+ 40. The correct name for an aqueous solution of HCN is a. b. c. d. hydrocyanic acid cyanic acid cyanate acid hydrocyanous acid 46. What is the formula for zinc(II) bromide? a. ZnBr b. Zn2Br c. ZBr d. Z2B e. ZnBr2 47. What is the correct formula for barium hydroxide? a. b. c. d. e. Ba2OH Ba(OH)2 BaOH Ba(OH)3 Ba(OH)4 48. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Na2S2O3 + I2 NaI + Na2S4O6 a. b. c. d. e. 1 2 3 4 6 49. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? P4O10 + H2O H3PO4 a. b. c. d. e. 10 6 4 2 1 50. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? NBr3 + NaOH N2 + NaBr + HOBr a. b. c. d. e. 1 2 3 4 5 51. When the equation Si(s) + HF(aq) SiF4(g) + H2(g) is balanced, what is the coefficient for HF? a. b. c. d. e. 0 1 2 3 4 a. evaporate b. are cations only c. form a second insoluble compound in the solution d. are left dissolved in the solution e. none of these 53. An aqueous solution of sodium sulfate is allowed to react with an aqueous solution of calcium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)?. a. b. c. d. e. 2Na+(aq) 2SO42-(aq) 3Ca2+(aq) NO3-(aq) K+(aq) 54. An aqueous solution of ammonium sulfide is allowed to react with an aqueous solution of barium chloride. What is the coefficient of the solid in the balanced equation (in standard form)? a. b. c. d. e. 1 2 3 4 5 55. The scientist who discovered the essential nature of acids through solution conductivity studies is a. b. c. d. e. Priestley Boyle Einstein Mendeleev Arrhenius 56. The reaction AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) is a(n) ______________ reaction. a. b. c. d. e. precipitation acid-base oxidation-reduction single-replacement none of these 57. A reaction that involves a transfer of electrons is called a(n) ______________ reaction. 52.When a precipitation reaction occurs, the ions that do not form the precipitate a. precipitation b. acid-base c. oxidation-reduction d. double-displacement e. none of these 58. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) a. oxidation-reduction b. synthesis c. decomposition d. combustion e. two of these Use the following choices to classify each reaction given below (more than one choice may apply). a. oxidation-reduction b. acid-base c. precipitation 59. ZnBr2(aq) + 2AgNO3(aq) Zn(NO3)2(aq) + 2AgBr(s) 60. KBr(aq) + AgNO3(aq) AgBr(s) + KNO3(aq) 61. HNO3(aq) + NaOH(aq) H2O(l) + NaNO3(aq) 62. 6Na(s) + N2(g) 2Na3N(s) 63. HC2H3O2(aq) + CsOH(aq) H2O(l) + CsC2H3O2(aq) Use the following choices to classify each reaction given below (more than one choice may apply). a. oxidation-reduction b. combustion c. synthesis d. decomposition 64. 2Cs(s) + F2(g) 2CsF(s) 65. S8(s) + 12O2(g) 8SO3(g) 76. 2GaN(s) 2Ga(s) + N2(g)