Chemistry Exam Questions and Concepts, Exams of School management&administration

Download Chemistry Exam Questions and Concepts and more Exams School management&administration in PDF only on Docsity! C111_section2 Exam # Final.B Thursday, 12/18/03 Name ________________________________ Calculator #:____________________ 40 multiple choice questions, 5 points per correctly answered question, 200 points total. 1.) What pressure will be exerted by 1.3 moles of ideal gas in a 13 liter flask at 22°C ? (use ideal gas law and your knowledge about gas volume of 1 mol at standard conditions). a.) 5.5 atm b.) 2.4 atm c.) 0.41 atm d.) 0.18 atm e.) 1.00 atm 2.) Hydrogen bonding is a special case of a.) London dispersion forces b.) Ion-dipole attraction c.) Ionic bonding d.) Dipole-dipole attraction e.) None of the above 3.) which of the following compounds will have hydrogen bonds as one of its intermolecular forces? a.) H2S b.) SiH4 c.) HCl d.) NH3 e.) CH4 4.) What is the final concentration of a hydrochloric acid solution made by diluting 205 mL of a 1.778 M HCl to 800.0 mL? a.) 0.182 M b.) 0.456 M c.) 16.6 M d.) 1.78 M e.) 0.306 M 5.) What is the oxidation number of sulfur in SF7 ? a.) –2 b.) +2 c.) -6 d.) +6 e.) +7 6.) The following reaction occurs for the hypothetical element E: 2E (l) + O2 (g) ‡ 2EO (g) DH0= -333 kJ EO (g) + O2 (g)‡ EO3 (s) DH0= -196 kJ What is DH0 in kJ for the reaction 2E (l) + 3O2 (g) ‡ 2 EO3 (s)? a.) –529 b.) +526 c.) +725 d.) –725 e.) -137 7.) How many grams of carbon dioxide are produced when 5555 kJ of heat are generated by the combustion of methane (CH4)? CH4 (g) + 2 O2 (g) Æ 2 H2O (l) + CO2 (g) DH = -890 kJ a.) 7.05 g b) 400 g c.) 137 g d.) 100 g e.) 275 g 8.) How many mL of a 4.00 M H2SO4 solution are required to completely neutralize 144.0 mL of a 3.03 M KOH solution? a.) 54.5 ml b.) 218 ml c.) 87.3 ml d.) 109 mL e.) 380 ml 9.) In which of the following compounds has the oxidation number for phosphorus the value ‘–III’ (minus three) ? a. PH3 b. H3PO4 c. P2O5 d. NaH2PO3 e. PF3 10.) A particular nitrogen oxide contains 63.65% by mass nitrogen. What could be a molecular formula for this nitrogen oxide (contains only N and O)? a.) NO b.) N2O c.) NO2 d.) NO3 e.)N2O4 11.) 10 meter of water exert about the same pressure as 760 mm Hg. Estimate the pressure in torr that a diver experiences 30 m below the surface. (don’t forget the pressure of the atmosphere above the water – at sea level) a.) 3040 torr b.) 760 torr c.) 2290 torr d.) 4000 torr e.) 400 torr 12.) 5.0 moles of a gas at 1.0 atm is expanded at constant temperature from 10 L to 15 L. What is the final pressure of the ideal gas (use ideal gas law and your knowledge about gas volume of 1 mol at standard conditions). a.) 1.5 atm b.) 7.5 atm c.) 0.67 atm d.) 3.3 atm e.) 1.0 atm 13.) What is the volume that 12.28 g of H2 take at 400 K and 2.00 atm? a.) 275 L b.) 138 L c.) 22.4 L d.) 50 L e.) 100 L 14.) Which of the following is a legal set of quantum numbers (n,l,ml,mz) for an electron: a. (1,1,0,-1/2) b. (6,1,-1,-1/2) c. (3, 2,3,+1/2) d. (5,3,-4,-1/2) e. (6, -2, 1, 1/2) 15.) The energy of a photon of light is ________ proportional to its frequency and ________ proportional to its wavelength. a.) directly, directly b.) inversely, inversely c.) inversely, directly d.) directly, inversely e.) none of the above 35.) what sketch represents an orbital that cannot have a principle quantum number of 2 a.) # 1 b.) only #2 & #3 c.) #1, #2, & #3 d.) #4. and #5. e.) they all can have n = 2 #1 #2 #3 #4 #5 36.) Which one of the following molecules is planar? a.) CBr4 b.) PH3 c.) ICl3 d.) XeF4 e.) SF4 37.) Which one of the following has a seesaw molecular structure? a.) CBr4 b.) XeF2 c.) SF4 d.) KrF4 e.) ClF3 38.) Which of the following molecules has a permanent dipole moment (i.e is polar)? a.) XeF2 b.) SF2 c.) CS2 d.) SF6 e.) BH3 39.) The respective hybridizations of BrF3 and ClF5 are a.) sp3 and sp3d b.) sp3d and sp3d2 c.) sp3d and sp3 d.) sp3d2 and sp3d e.) sp3d2 and sp3d2 40.) In which of the following compounds is the oxidation number of the bromine = +1 ? a.) HBrO b.) NaBrO2 c.) KBr d.) Al(BrO3)3 e.) CaBr2 1A 8A 1 H 1.008 2A 3A 4A 5A 6A 7A 2 He 4.003 3 Li 6.941 4 Be 9.012 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00 10 Ne 20.18 11 Na 22.99 12 Mg 24.31 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B 13 Al 26.98 14 Si 28.09 15 P 30.97 16 S 32.07 17 Cl 35.45 18 Ar 39.95 19 K 39.10 20 Ca 40.08 21 Sc 44.96 22 Ti 47.88 23 V 50.94 24 Cr 52.00 25 Mn 54.94 26 Fe 55.85 27 Co 58.93 28 Ni 58.69 29 Cu 63.55 30 Zn 65.39 31 Ga 69.72 32 Ge 72.61 33 As 74.92 34 Se 78.96 35 Br 79.90 36 Kr 83.80 37 Rb 85.47 38 Sr 87.62 39 Y 88.91 40 Zr 91.22 41 Nb 92.91 42 Mo 95.94 43 Tc (98) 44 Ru 101.1 45 Rh 102.9 46 Pd 106.4 47 Ag 107.9 48 Cd 112.4 49 In 114.8 50 Sn 118.7 51 Sb 121.8 52 Te 127.6 53 I 126.9 54 Xe 131.3 55 Cs 132.9 56 Ba 137.3 57 La 138.9 72 Hf 178.5 73 Ta 181.0 74 W 183.8 75 Re 186.2 76 Os 190.2 77 Ir 192.2 78 Pt 195.1 79 Au 197.0 80 Hg 200.6 81 Tl 204.4 82 Pb 207.2 83 Bi 209.0 84 Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra 226.0 89 Ac 227.0 104 Rf 261.1 105 Ha 262.1 106 Sg 263.1 107 Bh 262.1 108 Hs (265) 109 Mt (266) 58 Ce 140.1 59 Pr 140.9 60 Nd 144.2 61 Pm (145) 62 Sm 150.4 63 Eu 152.0 64 Gd 157.3 65 Tb 158.9 66 Dy 162.5 67 Ho 164.9 68 Er 167.3 69 Tm 168.9 70 Yb 173.0 71 Lu 175.0 90 Th 232.0 91 Pa 231.0 92 U 238.0 93 Np 237.0 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260) Useful info: DH = H(products) – H(reactants) q = Ctot DT q = m s DT q = n Cmolar DT DT = Tfinal - Tinitial qrxn = - qcalorimeter or qrxn = - qsolution DHorxn = S n DHof(products) - S m DHof(reactants) DH = qP † l = c n c = 3.00 x 108 m/s h = 6.63 x 10-34 J s NA= 6.022 x 1023 † DE = hn = hc l = -2.18 ¥10-18 J( ) 1n f2 - 1 ni 2 Ê Ë Á Á ˆ ¯ ˜ ˜