Name: __________________________ Date: _____________ 1. Ni(CO)4 can be prepared by reacting nickle (Ni) with gasous carbon monoxide (CO). If you have CO in a 1.50 L flask at a pressure of 418 mmHg at 25 oC along with excess Ni powder, what is the theoretical yield of Ni(CO)4? A) B) C) D) E) 1.44 g 5.75 g 2.88 g 1.31 g 3.83 g 2. If you place gasous unknown compound containing 25.53 % S in a 89.0 mL flask at 45 oC, and the total mass of the comound is 0.0955 g and the pressure is 83.8 mmHg. What is the molecular formula SxFy? A) B) C) D) E) S2F10 SF5 S3F15 S2F2 S2F5 3. In an experiment, it is determined that 0.66 moles of CF4 effuse through a porous barrier over a 4.8 minute period. How long will it take for 0.66 moles of CH4 to effuse through the same barrier? A) B) C) D) E) 2.0 min 0.66 min 0.33 min 1.5 min 1.2 min 4. Absolute zero is the point at which A) B) C) D) E) a straight-line graph of V versus T (K) intersects the origin. a straight-line graph of V versus 1/P at constant T intersects the origin. gaseous helium liquefies. a straight-line graph of 1/V versus P at constant T intersects the origin. a straight-line graph of V versus T (°C) intersects the origin. Page 1 5. The pressure of 5.4 L of nitrogen gas in a flexible container is decreased to one-half its original pressure, and its absolute temperature is increased to double the original temperature. The volume is now A) B) C) D) E) 22 L 2.7 L 5.4 L 11 L 1.4 L 6. Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65 oC, and contains 0.482 g of hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask? A) B) C) D) E) 0.557 atm 0.043 atm 1.11 atm 33.5 atm 67.0 atm 7. You add 0.255 g of a molecular compound to 11.2 g of benzene. The boiling point of the benzene rises from 80.10 oC to 80.26 oC. What is the molar mass of the compound? Kb = 2.53 oC/m A) B) C) D) E) 360. g/mol 63.0 g/mol 111 g/mol 700. g/mol 130. g/mol 8. Concentrated aqueous ammonia (NH3) has a molarity of 14.8 mol/L and a density of 0.90 g/cm3. What is the molality of the solution? A) B) C) D) E) 23 m 6.5 m 13 m 15 m 19 m Page 2 9. A solution is made by adding 50.0 mL of ethanol (C2H5OH, d = 0.789 g/mL) to 50.0 mL of water (d = 0.998 g/mL). What is the total vapor pressure over the solution at 20.0 o C? Given: Vapour pressure for the pure ethanol is 43.6 mmHg and water is 17.5 mmHg at 20.0 oC. A) B) C) D) E) 23.7 mmHg 35.6 mmHg 27.7 mmHg 38.5 mmHg 19.3 mmHg 10. The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7×10– 4 mol/L. What is the value of the Henry's Law constant in mol L–1 atm–1? A) B) C) D) E) 6.8 × 10–4 1.5 × 103 3.2 × 10–4 9.0 × 10–7 4.7 × 10–4 11. From the following list of aqueous solutions and water, select the one with the highest boiling point. A) B) C) D) E) 0.75 m CuCl2 0.75 m NaCl 1.0 m KNO3 2.0 m C12H22O11 (sucrose) pure water 12. A 0.100 m MgSO4 solution has a freezing point of –0.23°C. What is the van't Hoff factor for this solution? Kf = 1.86°C/m A) B) C) D) E) 1.2 1.5 2.0 1.8 1.4 Page 3 13. You are given a small bar of metal M. The density of the metal is 10.5 g/cm3. The edge of the face-centered cubic unit is 4.09 x 10-8 cm. Identify the M. A) B) C) D) E) Ag Au Co Pt Cu 14. The distance between layers in a MX crystal is 182 pm. X rays are diffrated from these layers at an angle of 22.20°. Assuming that n =1, calculate the wavelength of the X rays in nanometers. A) B) C) D) E) 0.138 nm 138 nm 14.2 nm 142 nm 0.142 nm 15. In hydrogen iodide, __________________ are the most important intermolecular forces. A) B) C) D) E) dipole–dipole forces covalent bonds polar covalent bonds hydrogen bonding London dispersion forces 16. The energy needed to increase the surface area of a liquid is A) B) C) D) E) surface tension. viscosity. capillary action. cohesion. specific elasticity. Page 4 17. How much energy (heat) is required to convert 52.0 g of ice at –10.0°C to steam at 100°C? specific heat of ice: 2.09 J/g·°C Hfus = 6.02 kJ/mol specific heat of water: 4.18 J/g·°C Hvap = 40.7 kJ/mol specific heat of steam: 1.84 J/g·°C A) B) C) D) E) 157.6 kJ 2570 kJ 1086 kJ 2296 kJ 40.20 kJ 18. Krypton has a higher melting point than argon because of its A) B) C) D) E) stronger dispersion forces. permanent dipole moment. greater ionization energy. ionic bonds. ion-dipole interactions among Krypton atoms. 19. The cost of the gold is $ 1350 per 31.103 g. It has been estimated that 8 x 104 tons of gold (Au) have been extracted. What is the total worth of this quantity? (1 ton = 2000 lb; 1 lb = 16 oz; 1 oz = 28.35 g) A) B) C) D) E) $ 3 x 1012 $ 1 x 1011 $ 9 x 1013 $ 7 x 1013 $ 8 x 1011 20. Convert 244.2°F into degrees Celsius. A) B) C) D) E) 117.9°C 382.0°C 167.7°C 153.4°C 103.7°C Page 5 21. What is the correct formula for aluminium hydrogen phosphate? A) B) C) D) E) Al2(HPO4)3 Al(HPO4)3 Al3(HPO4)2 Al(H2PO4)3 Al(HPO3)3 22. The correct name of the compound HBrO2 is A) B) C) D) E) bromous acid hypobromous acid hydrogen bromite bromic acid hydrogen bromine dioxide 23. A sample of xenon fluoride compound contains molecules of the type XeFn, where n is some whole number. Given that 9.03 x 1020 molecules of XeFn, weigh 0.368 g, determine the value for n in the formula. A) B) C) D) E) 6 5 4 3 2 24. The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. What number of H atoms are present in a 2.00 g of styrene? A) B) C) D) E) 9.25 x 1022 1.16 x 1022 6.13 x 1022 5.78 x 1021 1.85 x 1021 Page 6 25. Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Don't forget to count coefficients of one. The sum of the total coefficients is __ SF4 + __ H2O A) B) C) D) E) __ H2SO3 + __ HF 9 11 13 7 6 26. What volume of 0.0350 M barium hydroxide is required to completely neutralize 26.00 mL of 0.0600 M phosphoric acid? A) B) C) D) E) 66.9 mL 15.0 mL 29.7 mL 53.5 mL 43.3 mL 27. Which choice gives the correct oxidation numbers for all three elements in Rb2SO3 in the order that the elements are shown in the formula? A) +1, +4, 2 B) 2, +6, 2 C) 1, +4, 3 D) +2, +4, 2 E) +1, +6, 6 28. Use the following data to calculate the standard enthalpy of formation of hexane, C6H14(l): 2C6H14(l) + 19O2(g) → 12CO2(g) + 14 H2O(l) ΔH° = -8326 kJ Given ΔH° kJ/mol: CO2(g) = -393.5; H2O(l) = -285.8 A) B) C) D) E) -199 kJ/mol -398 kJ/mol 398 kJ/mol -355 kJ/mol 199 kJ/mol Page 7 29. A baloon is being inflated to its full extent by heating the air inside it. In the final stages of the process, the volume of the ballon changes from 4.00 x 106 L to 4.50 x 106 L by the addition of 1.3 x 108 J of energy as heat. Assuming that the balloon expands against a constant pressure of 1 atm, calculate ΔU for the process. [ 1L·atm = 101.3 J] A) B) C) D) E) 8 x 107 J 5 x 105 J 2 x 108 J 1 x 108 J 3 x 106 J 30. Which of the following statements is/are correct? i. The importance of the equation E = mc2 is that energy has mass. ii. Electromagnetic radiation can be thought of as a stream of particles called photons. iii. Electromagnetic radiation exhibits wave properties. iv. Energy can only occur in discrete units called quanta. A) B) C) D) E) All of them i, ii and iv only i, iii and iv only i, ii and iii only ii, iii and iv only 31. What is the frequency of electromagnetic radiation with wavelength 532 nm? A) B) C) D) E) 5.64 × 1014 s–1 4.18 × 1018 s–1 6.48 × 1012 s–1 3.75 × 1015 s–1 6.23 × 1014 s–1 32. The complete electron configuration of tin (Sn) is A) B) C) D) E) 1s22s22p63s23p64s23d104p65s24d105p2 1s22s22p63s23p64s24p65s24d105d105p2 1s22s22p63s23p64s23d104d104p2 1s22s22p63s23p64s23d104p65s24d105d105p2 1s22s22p63s23p64s23d104p65s25d105p2 Page 8 33. Which of the following processes represents the ionization energy of bromine? A) B) C) D) E) Br(g) Br2(g) Br(s) Br(l) Br(s) Br+(g) + e– Br2+(g) + e– Br+(s) + e– Br+(g) + e– Br+(g) + e– 34. Which of the following groups contains no ionic compound(s)? A) B) C) D) E) CH2O, CO2, NH3 HCN, NO2, Ca(NO3)2 PCl5, LiBr, Zn(OH)2 NaCl, CCl4, SF4 NaH, CaBr2, NaNH2 35. Which one of the following statements is not correct for the SF4 molecule? A) B) C) D) E) The molecule has sp3 hybridization. It has a see-saw structure. It has a total 13 lone pairs. The molecule contains a net dipole moment The S-F bonds are polar 36. What are the approximate O S O bond angles in SO32–? A) B) C) D) E) 109.5 90 and 180 180 120 90 Page 9 37. Which of the following species will have expanded octet? (Note: The first atom is the central atom) i. TeBr4 ii. ICl2 iii. XeF4 A) B) C) D) E) All of them i and ii only i and iii only ii and iii only none of them 2 38. For which of the following molecules and or ions does the central atom have sp hybridization? (The central atom is underlined in each formula below; for I3 one of the I is in centre) A) B) C) D) E) NOBr SO42– SBr2 I3CO2 39. Which of the following statements are correct for the molecular orbital theory? i. Hund's rule is obeyed. ii. electrons are assigned to orbitals of successively higher energy. iii. a bonding molecular orbital is lower in energy than its parent atomic orbitals. iv combination of two atomic orbitals creates one molecular orbital. A) B) C) D) E) i, ii and iii only i, ii and iv only i and iv only ii, iii and iv only all of them 40. Consider the molecules B2, C2, N2 and F2. Which two molecules have the same bond order? A) B) C) D) E) B2 and F2 C2 and N2 N2 and F2 C2 and F2 B2 and C2 Page 10 Answer Key 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A A Page 11