Practice Final Exam PDF

Practice Test- Final Exam 1. What is the formula of barium phosphate? A. BaPO3 B. BaPO4 C. Ba2(PO4)3 D. Ba3(PO4)2 2. What is the name of the compound Co(ClO2)3 ? A. cobalt (II) chlorate B. cobalt (II) chlorite...

Practice Test- Final Exam 1. What is the formula of barium phosphate? A. BaPO3 B. BaPO4 C. Ba2(PO4)3 D. Ba3(PO4)2 2. What is the name of the compound Co(ClO2)3 ? A. cobalt (II) chlorate B. cobalt (II) chlorite C. Cobaltous hypochlorite D. cobalt (II) trichlorite E. cobalt (III) chlorite 3. The empirical formula of an organic compound extracted from a medicinal plant is CH 2OS. Its molar mass is 186.0 g mol-1. What is its molecular formula? A. CH2OS B. C2H4O2S2 C. C3H4O3S3 D. C3H6O3S3 4. Which one of the sets below represents the correct values for the coefficients w, x, y and z in the following equation? w Fe(NO3)3 x Fe2O3 + y NO2 + z O2 w x y z A. 2 1 6 3 B. 2 2 6 3 C. 4 2 3 3 D. 4 2 12 3 5. During a laboratory session, in separate experiments, solutions of each of the following were mixed to determine whether a precipitate was formed. v. sodium chloride and potassium nitrate vi. potassium chloride and silver nitrate vii. sodium chloride and lead nitrate viii. barium chloride and sodium sulfate Use the solubility rules to decide which one of the following is true. A. A precipitate is formed in all experiments (i) to (iv) B. A precipitate is formed in experiments (i) and (ii) only. C. A precipitate is formed in experiments (ii), (iii) and (iv) only. D. A precipitate is formed in experiments (ii) and (iv) only. 6. What is the wavelength of electromagnetic radiation which has a frequency of 5.732 x 10 14 s-1? a. 1.718 x 1023 m b. 1.912 x 106 m c. 5.230 x 10-7 m d. 523.0 m e. 5.819 x 10-15 nm 7. The number of very fine beads of gold of equal size in a container is 1.5 x 10 7. What is the number of moles of gold beads in the container? A. 2.5 x 10-17 mol B. 2.5 x 10-16 mol C. 4 x 1015 mol D. 4 x 1016 mol 8. What is the mass (in g) of one molecule of oxygen gas (O2)? A. B. 16.0 16.0 C 2 x 16.0 x 6.02x1023 23 23 2 x 6.02x10 6.02x10 D 2 x 16.0 6.02x1023 9. Which of the following quantities of nitrogen gas (N2) contains the largest number of nitrogen molecules (molar mass N2 = 28.0 g mol-1)? a. 14 g b. 22.4 L at STP c. 1.4 mol d. 28.0 molecules 10. Which of the following nitrogeneous fertilizers contains the greatest number of moles of nitrogen in a mole of fertilizer? a. urea CON2H4 b. ammonium sulfate (NH4)2SO4 c. sodium nitrate NH4NO3 d. ammonium phosphate (NH4)3PO4 11. In the thermite process for welding of steel, the following reaction occurs 8 Al(s) + 3 Fe3O4(s) 4Al2O3(s) + 9 Fe(l) If the reaction is 85% complete, how many moles of iron are produced when 2.0 moles of aluminium reacts with an excess of Fe3O4. [Molar mass (g mol-1): Al = 27.0, Fe = 56.0] A. 9 85 x 2.0 x mol 8 100 B. 8 85 x 2.0 x mol 9 100 C. 9 100 x 2.0 x mol 8 85 D. 9 1 85 x x mol 8 2.0 100 12. A neutral atom of an element has the following electron configuration 1s22s22p63s23p64s2 In which group and period of the periodic table is this element located? a. Group III, Period 4 b. Group II, Period 4 c. Group IV, Period 2 d. Group II, Period 6 13. The ionic compounds of an element X contain X3+ ions. Which one of the following would be the electron configuration of a neutral atom of element X? a. 1s2 2s2 2p1 b. 1s2 2s2 2p6 3s1 c. 1s2 2s2 2p5 d. 1s2 2s2 2p3 14. The value of ΔE for a system that performs 13 kJ of work on its surroundings and loses 9 kJ of heat is __________ kJ. A) 22 B) -22 C) -4 D) 4 E) -13 15. The Lewis structure of PF3 is Which of the following best describes its electron-pair geometry? a. tetrahedral b. trigonal planar c. pyramidal d. linear 16. Which of the following molecules whose molecular geometry is given below is expected to have a dipole moment? A. B. C. D. tetrahedral trigonal planar trigonal planar linear 17. Which of the following best describes the formation of an ionic compound between atoms of two elements? a. sharing pairs of electrons between the atoms b. sharing of valence crystals to the entire crystal lattice. c. transfer of electrons between atoms d. formation of hydrogen bonds between atoms. 18. N2O4(g) decomposes according to the equation N2O4(g) 2 NO2(g) A sealed container contains 0.5 mol of N 2O4 gas at 100°C and 2.0 atmospheres pressure. What would be the pressure in the container if the N2O4 gas is decomposed completely to NO2 and the temperature were maintained at 100°C? a. 0.5 atm b. 1.0 atm c. 2.0 atm d. 4.0 atm 19. Flask X is filled with 20.0 g of O2 gas at 100 °C and another identical flask Y with 20.0 g N2 gas at the same temperature. Which one of the following statements is correct? [ Molar masses (g mol-1) O2 = 32.0; N2 = 28.0] a. The pressures of the gases in the two flasks are identical. b. The pressure of O2 in flask X is higher than that of N2 in flask Y. c. The pressure of O2 in flask X is lower than that of N2 in flask Y. d. The pressure of O2 in flask X is twenty times that of N2 in flask Y. 20. A gas in a container of fixed volume is heated from 100°C to 400°C. Which of the following is the best estimate of what will happen to the pressure of the gas? a. remain unaltered b. increase by a factor of 4 c. decrease by a factor of 4 d. increase by a factor of 1.8 21. The hydrides of the fifth group elements nitrogen (NH 3) and phosphorus (PH3) have the same molecular geometry (trigonal pyramidal.) However, the boiling temperature of NH 3 is considerably higher than that of PH3. Which of the following best explains the difference in their boiling temperature? a. The dispersion forces between NH3 molecules are stronger than those between PH3 molecules. b. the hydrogen bonding intermolecular forces between NH3 molecules are stronger than those between PH3 molecules. c. The N-H bond in NH3 is stronger than the P-H bond in PH3. d. The N-H bond in NH3 is weaker than the P-H bond in PH3. 22. Some of the properties of the pure substances W, X, Y and Z are given below Sub-stance Hardness Melting Electrical conductivity of solid temperature (°C) of solid of solution W soft -114 negligible negligible X soft 18 negligible negligible Y hard 810 negligible high Z hard 2700 negligible insoluble Which substance is most likely to be an ionic crystal? a. W c. Y b. X d. Z 23. Both the melting point and boiling point of nitrogen gas (O 2) are very low. However it is very difficult to dissociate O2 molecules into atomic oxygen (O). Which of the following best explains these properties of oxygen? a. The intramolecular bonding of oxygen molecules is stronger than the intermolecular bonding. b.The intramolecular bonding of oxygen molecules is weaker than the intermolecular bonding. c. The intramolecular bonding of oxygen molecules is identical to the intermolecular bonding. d. The molecular oxygen and atomic oxygen both have weak London dispersion forces. 24. What is the oxidation number of chlorine in ClO4–? a. -1 b. -3 c. +3 d. +7 25. Which one of the following is the change in oxidation number of Br in the following equation? 10 Cl– + 2 BrO3– + 12 H+ 5 Cl2 + Br2 + 6 H2O a. no change b. -1 0 c. +5 0 d. +5 -1 26. What is the formula of sodium sulfite? A. Na2SO3 B. Na2SO4 C. Na2S2O3 D. Na2S 27. What is the formula of copper(II) phosphate? A. Cu2(PO4)3 B. Cu3(PO4)2 C. Cu3PO4 D. CuPO4 28. Which one of the following types of radiation has the highest frequency? a. x-rays b. ultraviolet rays c. FM radio waves d. microwave radiation e. infrared radiation 29. What is the energy, in joules, of one photon of visible radiation with a wavelength of 464.1 nm? a. 1.026 x 10-48 J b. 2.100 x 1035 J c. 2.341 x 1011 J d. 4.280 x 10-19 J e. 4.280 x 10-12 J 30. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the energy level with n = 6 to the level with n = 3. a. 1.665 x 10-26 s -1 b. 1.824 x 10-15 s-1 c. 2.740 x 1014 s-1 d. 3.649 x 10-15 s-1 e. 9.132 x 1013 s-1 31. Which of the following organic compounds contains the greatest mole percentage of carbon? A. CH3COOH B. (CH3)2CO C. CH3CON(CH3)2 D. (CH3)3N 32. Which of the following statements is correct for an electron that has the quantum numbers n = 4 and m l = -2? A. the electron may be in a p orbital B. the electron may be in a d orbital C. the electron is in the second principal shell D. the electron must have a spin quantum number ms = + ½ 33. Given the data in the table below, H for the reaction rxn 4NH3 (g) 5O2 (g) 4NO(g) 6H2O(l) is __________ kJ. A) -1172 B) -150 C) -1540 D) -1892 E) The Hf of O2 (g) is needed for the calculation. 34. The Lewis structure of SO2 is Which of the following best describes its electron-pair geometry? A. tetrahedral B. trigonal planar C. pyramidal D. linear 35. The molecular geometries of some common compounds I to IV are as follows Compound Molecular Geometry I CHCl3 Tetrahedral II BCl3 Trigonal Planar III H2O Bent IV CO2 Linear A. All the compounds I, II, III and IV have a dipole moment. B. Only I and III have a dipole moment. C. Only III and IV have a dipole moment. D. Only III has a dipole moment. 36. Given the following at 25°C and 1.00 atm: ΔH0 1/2N2(g) + O2(g) → NO2(g) 33.2 kJ N2(g) + 2O2(g) → N2O4(g) 11.1 kJ Calculate the ΔH0 for the reaction below at 25°C. 2NO2(g) → N2O4(g) a. +11.0 kJ b. +44.3 kJ c. +55.3 kJ d. -22.1 kJ e. -55.3 kJ 37. The set of quantum numbers, n = 4, l = 3, ml = 2 A. describes an electron in a 3p orbital B. is not allowed C. describes an electron in a 4d orbital D. describes one of seven orbitals of a similar type 38. Which one of the following statements concerning SO32– and H2SO3 is correct? A. The oxidation number of S in SO32– and S in H2SO3 are identical. B. The oxidation number of S in SO32– is positive and of S in H2SO3 is negative. C. The oxidation number of S in SO32– is negative and of S in H2SO3 is positive. D. The oxidation numbers of S in both SO32– and H2SO3 are negative. 39. Which one of the statements concerning the following reaction is correct? Zn + Br2 ZnBr2 A. The reaction is a precipitation reaction. B. The oxidation number of Br is changed from 0 to +1. C. The oxidation number of Br is changed from 0 to -1. D. The oxidation number of Br is changed from 0 to -2. 40. What is the molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen and 48.68% fluorine if the molar mass of this compound is 156.12 g? a. C3H4F2 b. C5H10F5 c. C6H8F4 d. C6H6F3 41. If 2.68 g of hydrated sodium sulfate, Na2SO4·nH2O, on heating produces 1.26 g of water, what is the empirical formula of this compound? (a) Na2SO4·H2O (b) 2Na2SO4·H2O (c) Na2SO4·7H2O (d) 9Na2SO4·8H2O 42. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms. (a) 1 (b) 5 (c) 6 (d) 9 43. What would be the volume in liters of 640 g of oil if the density of the oil is 0.8 g/mL? (a)800 liters (b)0.8 liter (c)512 liters (d)0.5 liters 44. Five 1 peseta coins from Spain were dropped into a graduated cylinder containing 20.20 mL of water. The volume of the water increased to 22.05 mL. A single coin had a mass of 0.99 gram. What is the identity of the metal used for the Spanish 1 peseta coins? density of aluminum = 2.7 g/mL density of zinc = 7.1 g/mL density of copper = 9.0 g/mL density of silver = 10.0 g/mL (a)aluminum (b)zinc (c)copper (d)silver 45. The mass of a metal cylinder was determined on an analytical balance to be 50.208 g. The volume of the cylinder was measured and determined to be 5.6 mL. The density of the metal cylinder, expressed to the proper number of significant figures, is... (a)8.9657 g/mL (b)9.0 g/mL (c)0.11153 g/mL (d)0.11 g/mL 46. Two students, Garrison and Isabella, determined the mass of an object on two different balances. The accepted mass of the object was 2.355 g. Garrison obtained values of 2.531 g, 2.537 g, 2.535 g and 2.533 g. Isabella obtained values of 2.350 g, 2.404 g, 2.296 g and 2.370 g. Which statement best describes the results that were obtained by Garrison and Isabella. (a)Garrison obtained the better accuracy. (b)Isabella obtained the better accuracy. (c)Garrison obtained the better precision. (d)Isabella obtained the better precision. 47. The molecule N2 is isoelectronic with... (a)O2 (b)F2 (c)NO (d)CN- 48. In which of the following compounds does ionic bonding predominate? (a)NH4Cl (b)CO2 (c)CH4 (d)LiBr 49. When two ionic compounds are dissolved in water, an exchange reaction can... (a)never occur since all ions in water are "spectator ions". (b)occur if two of the ions form an insoluble ionic compound, which precipitates out of solution. (c)occur if the ions react to form a gas, which bubbles out of the solution. (d)occur only if the ions form covalent bonds with each other. (e) both b and c. 50. Which of the following chemical equations correctly represents the reaction between calcium hydroxide and hydrochloric acid? 51. What is the balanced net ionic equation for the reaction of CaCl2 and AgNO3? 52. 74. A new element, Tyserium (Ty), has recently been discovered and consists of two isotopes. One isotope has a mass of 331 g/mol and is 35.0 % abundant. The other isotope is 337 g/mole and is 65.0 % abundant. What is the mass of Ty as it appears on the periodic table? a. 332 g/mol b. 333 g/mol c. 334 g/mol d. 335 g/mol e. 336 g/mol 53. If 64 grams of O2 react with 45 grams of C2H6, how many grams of CO2 will be formed? The formula mass of O2 = 32 amu, C2H6 = 30 and the formula mass of CO2 = 44 amu. The balanced chemical equation is given in the previous problem. (a) 132 grams (b) 66 grams (c) 50 grams (d) 44 grams 54. How many milliliters of 2 M NaCl solution are required to make 1 liter of 0.4 M NaCl solution? (a) 5,000 mL (b) 800 mL (c) 200 mL (d) 0.2 mL 55. If an air bag in a car needs 44.8 L of gas when filled, how many grams of NaN 3 are needed to fill the bag with nitrogen gas at standard temperature and pressure? Remember that one mole of any gas will occupy 22.4 L at STP. The balanced chemical is... (a) 56 grams (b) 87 grams (c) 130 grams (d) 1.3 grams 56. How many grams of NaOH are needed to make 100 milliliters of a 0.2 molar solution of NaOH? (a) 0.02 grams (b) 0.8 grams (c) 20 grams (d) 800 grams 57. How many grams of NaHCO3 (baking soda) would you need to neutralize 500 mL of battery acid (H 2SO4) that has been spilled on your garage floor? Assume that the concentration of the battery acid is 12 molar. The balanced chemical equation is... (a) 1,008,000 grams (b) 1,008 grams (c) 504 grams (d) 252 grams 58. When 157.0 grams of CaSO4 are dissolved in enough water to yield a volume of 7.25x102 milliliters of solution. The molarity of this solution will be... (a) 0.0016 M  (b) 0.837 M (c) 1.15 M (d) 1.59 M 59. How many grams of carbon are needed to completely react with 75.2 g of SiO 2? The balanced chemical equation is... (a) 3.76 g (b) 15.1 g (c) 36.0 g (d) 45.1 g 60. In an acid-base titration, 42.90 mL of 0.825 M H2SO4 was required to neutralize 75.0 mL of NaOH solution. What is the molarity of the NaOH solution? (a) 0.0009 M (b) 0.071 M (c) 0.472 M (d) 0.944 M 61. If you react 1.00 L of ethane at STP with 3.00 L of oxygen at STP, how many grams of carbon dioxide will be formed? One mole of any gas occupies 22.4 L at STP. The balanced chemical equation is... (a) 1.96 g (b) 3.37 g (c) 3.93 g (d) 5.89 g 62. What is the percent yield of water if 0.90 g of water is obtained when 29.0 g of butane is burned in excess oxygen? The balanced chemical equation is... (a) 0.02% (b) 2% (c) 10% (d) 36% 63. If 1.45 J of heat are added to a 2.00 g sample of aluminum metal and the temperature of the metal increases by 0.798 oC, what is the specific heat of aluminum? (a) 0.579 J/g deg (b) 0.909 J/g deg (c) 1.68 J/g deg (d) 3.63 J/g deg 64. Water has a specific heat of 4.184 J/g deg while glass (Pyrex) has a specific heat of 0.780 J/g deg. If 10.0 J of heat is added to 1.00 g of each of these, which will experience the larger increase of temperature? (a)glass (b) water (c) They both will experience the same change in temperature since only the amount of a substance relates to the increase in temperature. 65. The heat of combustion for 1 mole of carbon to carbon dioxide is -410 kJ. How many kJ of heat would be liberated from the complete combustion of 60.0 g of carbon? (a) -82 kJ (b) -2050 kJ (c) -24,600 kJ 7. 66. Given the following data at 1 atm of pressure and 25.0 oC... ∆Hoformation = +64.4 kJ/mole for Cu2+ ∆Hoformation = -152.4 kJ/mole for Zn2+ ∆Hoformation = 0 for both Zn and Cu because these are in the most stable state. Calculate the standard heat of reaction for... (a) -217 kJ/mole (b) +217 kJ/mole (c) -88.0 kJ/mole (d) +88.0 kJ/mole 67.What is the energy of one mole of light that has a wavelength of 400 nm? (a) 4.97 x 10-28 J (b) 4.97 x 10-19 J (c) 2.99 x 10-4 J (d) 2.99 x 105 J 68. Which of the following ions has the smallest diameter? (a) O2- (b) Na+ (c) F- (d)Al3+ 69. Which of the following elements has the greatest electronegativity? (a) Si (b) P (c) N (d) O 70. Which element would have the greater difference between the first ionization energy and the second ionization energy? (a) potassium (b) calcium (c) Both should have the same differences because they are in the same period of the periodic table.  1 D 26 A 51 D 2 E 27 B 52 D 3 D 28 A 53 C 4 D 29 D 54 C 5 C 30 C 55 B 6 C 31 C 56 B 7 A 32 B 57 B 8 D 33 A 58 D 9 C 34 B 59 D 10 D 35 B 60 D 11 A 36 E 61 C 12 B 37 D 62 B 13 D 38 A 63 B 14 B 39 C 64 A 15 A 40 C 65 B 16 A 41 C 66 A 17 C 42 D 67 B 18 D 43 B 68 D 19 C 44 A 69 D 20 D 45 B 70 A 21 B 46 C 22 C 47 D 23 B 48 D 24 D 49 E 25 C 50 A