A_521912_2009-05-209

A_521912_2009-05-209 - Final_CHE1103 Student: 1. Select the...

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Unformatted text preview: Final_CHE1103 Student: 1. Select the answer that expresses the result ofthis calculation with the correct number of significant figures. 13.602 ><1.90 x305 _ 4.2341409? 13.3568 13.357 13.36 13.4 13 571.0093? 2. Which measurement is expressed to 4 significant figures? A. 0.00423 kg B. 24.049 cm 0. 1300 K D. 82,306 m E. 62.40 g 3- Bud N. Chemist must determine the density of a mineral sample. His four trials yield densities of 4.77 g/cm3, 4.67 9/ cm3, 4.69 g/cm3, and 4.81 g/cm3. Independent studies found the correct density to be 4.75 g/cm3. Which of the following statements represents the best analysis of the data? A. Bud's results have much greater accuracy than precision B. Bud's results have much greater precision than accuracy C. Bud's results have high accuracy and high precision D. Bud's results have low accuracy and low precision E. Bud's equipment is faulty 4. The appropriate number ofsignificant figures in the result of 15.234 x 15.208 is A. WUOW 001pr Page 1 5. A flask has a mass of 78.23 9 when empty and 593.63 g when filled with water. When the same flask is filled with concentrated sulfuric acid, H2804, its mass is 1026.57 9. What is the density of concentrated sulfuric acid? (Assume water has a density of 1.00 g/cm3 at the temperature of the measurement.) A. 1.992 g/cm3 3 1.840 g/cm3 0- 1.729 g/cm3 D. 1.598 g/cm3 E. o.543_g/cm3 6. Atoms X, Y, Z, and R have the following nuclear compositions: 410 410 412 15X HEY 185R Which two are isotopes? A.X&Y B. X&R C. Y&R D. Z&R E. X&Z 7. Which one of the following combinations of names and formulas of ions is incorrect? A- Ba2+ barium 13- 82' sulfate CN‘ cyanide CIO4' perchlorate HCO3‘ bicarbonate F100 8. Silver chloride is used in photographic emulsions. What is its formula? A. Angl3 B. Angl 0. AgC|3 D. AgCIz E. AgCl 9. Ammonium sulfate, (NH4)ZSO4, is a fertilizerwidely used as a source of nitrogen. Calculate its molecular mass. A. 63.07 amu B. 114.l0 amu C. 118.13 amu D. 128.11 amu E. 132.13 amu Page 2 10. Silicon, which makes up about 25% of Earth's crust by mass, is used widely in the modern electronics industry. It has three naturally occurring isotopes, 28Si, 29Si, and 30Si. Calculate the atomic mass of silicon. isotope isotopic Mass (amui Abundance % 253i 27.976927 92.23 295i 28.976495 4.67 305i 29.973770 3.10 A. 29.2252 amu B. 28.9757 amu C. 28.7260 amu D. 28.0855 amu E. 27.9801 amu 11. Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 9 C02 and 0.226 9 H20. What is its empirical formula? A. C2H3O4 C3H402 C4H302 CSH1204 CZHZO F1009? 12. In the combustion analysis of 0.1127 g of glucose (CeH1206), what mass, in grams, of 002 would be produced? A. 0.04519 B. 008259 0. 0.16529 D. 0.41329 E. 1.4669 13. Magnesium (used in the manufacture of light alloys) reacts with iron(lll) chloride to form magnesium chloride and iron. 3Mg(s) + 2FeC|3(s) —> 3MgCl2(s) + 2Fe(s) A mixture of 41.0 g of magnesium (W1 = 24.31 g/mol) and 175 g of iron(lll) chloride ( M = 162.2 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. A. Limiting reactant is Mg; 67 g of FeCl3 remain. Limiting reactant is Mg; 134 g of FeCI3 remain. Limiting reactant is Mg; 104 g of FeCl3 remain. Limiting reactant is FeClg; 2 g of Mg remain. Limiting reactant is FeCI3; 87 g of Mg remain. WUOW Page 3 14. What will be the final volume of a solution prepared by diluting 25 mL of 8.25 M sodium hydroxide to a concentration of 2.40 M? A. 330 mL B. 210 mL C. 86 mL D. 60 mL E. 7.3 mL 15. Calcium fluoride, CaFg, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass. A. 118.15 g/mol B. 99.15 g/mol C. 78.07 g/mol D. 59.08 g/mol E. 50.01 g/mol 16. Potassium chloride, KCI, sodium sulfate, N32804, glucose, C5H1205, carbon dioxide, CO; and ammonium phosphate, (NH4)3PO4, are soluble in water. Which one produces the largest number of dissolved particles per mole of dissolved solute? A. KCI B. N32801:, C. C6H1206 D. C02 E. (NH4)3PO4 17. Calculate the oxidation number ofthe chlorine in perchloric acid, HCIO4, a strong oxidizing agent. A. -1 B. C. +5 D. E. none of these is the correct oxidation number 18. Automobile batteries use 3.0 M H2804 as an electrolyte. How much 1.20 M NaOH will be needed to neutralize 225 mL of battery acid? HZSO4(aq) + 2NaOH(aq) —> 2H20(I) + Na2804(aq) A. 0.045 L B. 0.28 L C. 0.56 L D. 0.90 L E. 1.1 L Page 4 19. Select the classification forthe following reaction. H2(g) + C|2(g) —> 2HCllg) A. combination B. decomposition C. displacement D. acid-base E. none ofthese choices is correct 20. Balance the following redox equation using the smallest integers possible and select the correct coefficient for the chromate anion, CrO42'. CrO42'(aq) + CN'(aq) + H20(/) —> CNO'(aq) + Cr(OH)4‘(aq) + OH'(aq) mcom> macaw—x 21. Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its absolute temperature, other factors remaining constant? Volume (L) O Tern perature (K) A.a B.b C.c D.d E.e 22. A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP? A. 25.2 L 30.6 L 33.6 L 37.1 L 49.2 L “1.0.0.03 Page 5 23. A sample of ammonia gas at 655°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8°C and its pressure is 524 torr? A. 3.69 L B. 11.6 L C. 20.2 L D. 63.5 L E . not possible, since the volume would have to be negative 24. A gas mixture, with a total pressure of 300. torr, consists of equal masses of Ne (atomic weight 20.) and Ar (atomic weight 40.). What is the partial pressure of Ar, in torr? A. 75 torr B. 100. torr C. 150.torr D. 200. torr E. none of these choices is correct 25. Arrange the following gases in order of increasing rate of effusion. C2H5 Ar HCI PH3 A. Ar < HCI <PH3 < CzHe B. 02H5 < PH3 < HCI < Ar C. Ar < PH3 < C2H5 < HCI D. 02H6 < HCl < PH3 < Ar E. Ar <PH3 < HCI < C2H5 26. Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation. A.4Ixm39J B.4ixp3°J 0.32x1049J D.a2x1o%J E~bemeen10mand10wJ 27. According to the Rydberg equation, the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm) of A. 91.2 nm B-1JOX1OQnm C1on1fnm D.f1ox1d6nm E. none of these choices is correct Page 6 28, In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed? re .5 m; a. 3 l3 0 b. 3 1 ~1 c. 3 2 2 d, 3 2 ml '6. 3 3 2 m U 0 w > (DQOO'OJ 29- According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 x 103 m/s, the uncertainty in its position (in m) is at least A.i7xmfm B.eexm$m C. 17 m D. 66 m E. none of these choices is correct 30- A photon has an energy of 5.53 x 10'17 J. What is its frequency in 3‘1? A~366x1060s1 B.1.2oxlo”s4 0.3.59x10'95‘1 D 278x1oas4 E.8.35x101654 31. The effective nuclear charge for an atom is less than the actual nuclear charge due to A. shielding. B. penetration. paramagnetism. electron—pair repulsion. relativity. WUO Page 7 32. Which one of the following statements about atomic structure and quantum numbers is incorrect? A. In a given atom, the maximum number of electrons having principal quantum number n = 3, is 18. B. The number of orbitals in a given fsubshell is 7. C. For n = 4, the largest possible value of / is 3. D. For n = 4, the largest possible value of m/ is 2. E . The following set of quantum numbers for a single orbital is not allowed: n = 3, /= 1, m, = -2. 33. In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number / = ‘l? (The n, m, and mS quantum numbers may have any appropriate values.) A. 9 B. 12 C. 18 D. 24 E. 36 34. Which of the following electron configurations represents the ground state for an element? A. [Ne]3s13p1 B. [He12s12p3 C. [Ne]3s23p23d1 D. [Ne13s23p33d1 E. [Ne13s23p3 35. Which of the following elements has the largest first ionization energy? A. Na B. Cl C. Ca D. Te E. Br 36. In which of these substances are the atoms held together by polar covalent bonding? A. SrCl2 B. CsCl CIF . Tin SB lTlUO Page 8 37. Select the element whose Lewis symbol is correct. a. b. c. d, e. Fr - Ra - ~Pb~ ‘Te ' He v A. a B. b C. c D. d E. e 38. Which one of the following properties is least characteristic of typical ionic compounds? A. high melting point B. high boiling point C. brittleness D. poor electrical conductor when solid E. poor electrical conductor when molten 39. Arrange the following bonds in order of increasing bond strength. A. C—I < C-Br < C-Cl < C-F B. C-F < C-Cl < C-Br < C-I C. C-Br < C-l < C-Cl < C-F D. C—l < C-Br < C-F< C—CI E. none of these orders is correct 40. Select the most polar bond amongst the following. A. 0-0 B. Si-F C. Cl-F D. C—F E. C-I 41. In which one ofthe following species is the central atom (the first atom in the formula) an exception to the octet rule? A. NH3 NH4+ l2 3H4— SFe moow Page 9 42. According to VSEPR theory, a molecule with the general formula AX2 will have a _ molecular shape. 43. 44. 45. 46. A. linear B. bent C. trigonal planar D. tetrahedral E. triangular According to VSEPR theory, a molecule with the general formula AX2E2 will have a A. linear B. bent C. trigonal planar D. tetrahedral E. see-saw What is the molecular shape of BCl3 as predicted by the VSEPR theory? A. linear B. trigonal planar C. bent D. tetrahedral E. trigonal pyramidal What is the molecular shape of SiFsz' as predicted by the VSEPR theory? trigonal bipyramidal hexagonal tetrahedral see-saw octahedral WUOW?’ Valence bond theory predicts that xenon will use hybrid orbitals in XeOF4. A. sp B. 5p2 sp3 spad sps’d2 WOO Page 10 molecular shape. 47~ According to molecular orbital theory, what is the bond order in the 02+ ion? A. 5.5 B. 5 C. 4 D. 2.5 E. 1.5 48- According to valence bond theory, which of the following molecules involves sp2 hybridization of orbitals on the central atom? (central atom is bold) A. C2H2 B. C2H4 c. C2H5 D. co2 E. H20 49. A molecule with the formula AX4E2 uses to form its bonds. A. sp hybrid orbitals sp2 hybrid orbitals sp3 hybrid orbitals sp3d hybrid orbitals spad2 hybrid orbitals WUOFD 50. A molecule with the formula AX3 uses to form its bonds. A. sp hybrid orbitals 3 sp2 hybrid orbitals 0- sp3 hybrid orbitals 0- sp3d hybrid orbitals E- spsd2 hybrid orbitals Page 11 1. (p.27) E 2. (p. 27) E 3. (p. 29) A 4. (p. 27) D 5. (p. 22) B 6. (p. 51) E 7. (p.66) B 8. (p. 64) E 9. (p. 72) E 10. (p. 53) D 11. (p.98)C 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. (p. (p. (p- (p. (p- (p. (P. (p. (p. (p. (p- (P- (p. 95) C 110) D 118) C 89) C 137) E 152) D 147) E 158) A 154) B 184) C 188) D 188) B 196) B Final_CHE1103 Key Page 1 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. (p. 205) A (p. 253) E (p. 255) A (p. 279) E (p. 274) A (p. 263) E (p. 294) A (p. Sec. 8.3) D (p. Sec. 8.3) C (p. Sec. 8.3) E (p. 309) B (p. 353) C (p. 331) B (p. 337) E (p. 341) A (p. 355) B (p. 373) E (p. Sec. 10.2) A (p. Sec. 10.2) B (p. Sec. 10.2) B (p. Sec. 10. 2) E (p. Sec. 11.1) E (p. 415) D (p. Sec. 11.1. 11.2) B Page 2 49. (p. Sec. 11.1) E 50. (p. Sec. 11.1) B Pages ...
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A_521912_2009-05-209 - Final_CHE1103 Student: 1. Select the...

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