Chemistry Final Exam: Practice Problems
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1 Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence electron metal nonmetal metalloid Charles law Boyle s Law Gay-Lussac s law atm torr Combined Gas law Ideal Gas Law kpa ion ionic bond covalent bond Kelvin Celsius mole Avogadro s number endothermic exothermic octet rule solid liquid gas molar mass 1 empirical formula balanced equation heat temperature specific heat heat capacity Joule Calorie calorie Conservation of mass Conservation of energy diffusion effusion isotope(s) representative elements transition elements (metals) (Lewis) electron dot diagrams catalyst Problems/Concepts: Know (memorize) and be able to apply the following equivalents, relationships, formulas, etc.: P 1 V 1 = P 2 V 2 (Boyle s) V1 V = ---- (Charles ) T 1 T 2 Moles = mass (g) / molar mass P 1 P = (Gay-Lussac) T 1 T 2 P 1 x V 1 P 2 x V = (Combined) T 1 T 2 PV = nrt or n = PV/RT (remember R = 8.31) (Ideal) P total = P 1 + P 2 + P 3 + (partial pressure) J = 1 cal 1 J = cal q (heat in joules or calories) C = m T q = C m T q = s m T Molarity moles of solute = liters of solvent Moles of solute = Molarity (M) x Liters of solution Dilution: M 1 V 1 = M 2 V 2 or N 1 V 1 = N 2 V 2 D = m/v 1. Find the following temperatures in Kevin: a. 0 C = b. 23 C = c. 100 C = d C = 2. Find the following temperatures in C: a. 0 K = b. 100 K = c. 373 K = d. 273 K = 3. Define STP in K and mmhg K and kpa K and atm K and torr C and kpa C and mmhg C and torr C and atm 4. Which of the above is the SI unit for pressure? 5. How many atoms are in a mole of any element? 6. Which of the above have the same numerical value? 7. Fill in the blanks: 1 atm = mmhg = torr = kpa 8. What kinds of atoms form covalent bonds? 9. What kinds of atoms form ionic bonds?
2 Chemistry Final Exam: Practice Problems 10. Which of the following would form covalent (C), which would form ionic (I) bonds and which would not bond (N)? a. Ca & Cl b. S & O c. Mg & Fe d. C & H 11. What is meant by an atom s the ground state and atoms that have excited electrons? 12. How can you identify atoms that have the same number of electrons in their highest occupied energy (valence ) levels? 13. How can you identify atoms that have similar chemical properties? 14. Where are the metals located in the periodic table? 15. Where are the nonmetals located in the periodic table? 16. Where are the metalloids located in the periodic table? Describe each of the following types of chemical reactions: 17. Combination/Synthesis: 18. Decomposition: 19. Single replacement: 20. Double replacement: 21. Combustion: 22. In any period of the periodic table, what kind of changes occur as you go from left to right? a. (atomic radius) b. (ionization energy) c. (electronegativity) d. (metallic character) 23. What happens to atomic size (radius) as you go down a column (group) and why? / 24. What happens to atomic size (radius) as you go across a period and why? / 25. Which of the following elements would have the greatest atomic radius? a. P b. F c. Cl 26. Which of the following elements would have the greatest ionization energy? a. P b. F c. Cl 27. What do all acids contain? 28. What do all bases contain? 29. What is a salt? 30. Neutralization reaction result in what kinds of products? & 31. What term is used when a substance like CO2 turns directly from a solid to a gas? 32. A 47.7-g piece of copper increases from 25.0 C to 48.0 C when it absorbs 425 J of heat. What is the specific heat of copper? (show your work) 33. Circle which units can be used to measure heat flow: Joules moles degrees calories(c) kilocalories (C) 34. What is the octet rule? 35. If a compound s name ends with -ate or -ite it must contain. 2
3 In a graph below 36. Where is the substance only a solid? 37. Where is the substance only a liquid? 38. Where is the substance only a gas? 39. Where is the substance turning from liquid to gas? 40. Where is the substance solid to liquid? C D E A B 41. How do cations form and what type of element(s) form(s) them? 42. How do anions form and what type of element(s) form(s) them? 43. At STP what is the volume of 1 mole of any gas? 44. What is the relationship between the size of a gas molecule and diffusion and effusion? 45. At the same temperature and pressure, which gas will move fastest (and therefore diffuse or effuse faster)? a. H 2 b. O 2 c. N 2 d. Ar On a ph scale like the one above a. where would bases fall? b. where would neutral substances fall? c. where would bases fall? 47. If you decrease the volume of a container holding a gas without changing temperature of the gas what happens to its pressure. 48. At what temperature will water boil when the external pressure is mmhg? (Initial conditions are at STP) 49. If you triple the temperature of a gas in a rigid inflexible container, what happens to its pressure? 50. In terms of arrangement and movement of particles what is the difference between a solid, a liquid and a gas? 51. In terms of volume and shape what is the difference between a solid, a liquid and a gas? 52. The formation of aluminum oxide is expressed in the following reaction: Balance the equation: Al + O 2 Al 2 O 3 How many moles of aluminum are needed to form 3.7 moles of Al 2 O 3? 3
4 53. Acetylene gas (C 2 H 2 ) is produced by adding water to calcium carbide (CaC 2 ). CaC 2 + 2H 2 O C 2 H 2 + Ca(OH) How many grams of acetylene are produced by adding water to 5.00 g CaC 2? 55. What is molar mass? 56. What is and how do you calculate the molar mass of CuSO 4? 57. How can molar mass of a compound be determined? 58. What is the molar mass of C 6 H 12 O 6 (glucose)? 59. What is the empirical formula for glucose in then above question? 60. Balance the following chemical equations: a. Mg (s) + HCI (aq) MgCl 2 (aq) + H 2 (g) b. Al + H SO 2 4 Al (SO ) H 2 c. Fe + O 2 Fe 2 O How many moles are present in 34 g of Cu(OH) 2? 62. How many moles of hydrogen molecules (H 2 ) are there in 2.45 x molecules of CH 4? 63. How many moles of aluminum are needed to react completely with 1.2 mol of FeO below? (Show your work) 2Al + 3FeO 3Fe + Al 2 O How much heat is required to raise the temperature of 68.0 g of iron from 30.0 C to 55.0 C? (Show your work) (Specific heat of iron = 0.44 J/g C) 65. Given the reaction at STP: 2KClO 3 (s) 2KCl (s) + 3O 2 (g) What is the total number of liters of O 2 (g) produced from the complete decomposition of mole of KClO 3 (s)? (Show your work) 4
5 Given the reaction: 2Al 2 O 3 4Al + 3O What is the total volume of oxygen released when 1.00 mole of Al 2 O 3 decomposes? (Show your work) 67. What is the electron configuration for a phosphorus atom? 68. What is the correct e- configuration for an argon atom? 69. How many covalent bonds formed in the compound CO 2? 70. A gas has a volume of 50 L at a temperature of 200 C. What will the new volume of the gas be if the temperature is reduced to 100 C? 71. Draw Lewis Dot Structure for the following atoms: a. Ca b. Xe c. Ga d. Al 72. How many milliliters of 0.50 M HCI are needed to exactly neutralize 20 milliliters of 1.0 M KOH? 73. How many moles of a gas will a 1000 ml flask hold at 65.0 C and a pressure of 56 kpa? 74. What is the correct formula for the following acids? a. sulfuric acid b. nitric acid 75. Given the reaction: 4Al + 3O 2 2Al 2 O 3 How many moles of aluminum are needed to form 3.7 mol Al 2 O 3? (Show your work) 76. The energy absorbed when a substance dissolves in water and the surroundings cool down may be expressed as? a. Degrees b. Kilocalories c. Moles d. Grams per mole 77. If 148 grams of calcium hydroxide [Ca(OH) 2 ] are used to prepare a 4.00 M solution, what volume in ml of solution can be made? 5
6 The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride. 5F 2 (g) + 2NH 3 (g) N 2 F 4 (g) + 6HF(g) 78. If you have 66.6 g NH 3, how many grams of F 2 are required for complete reaction? (Show your work) 79. A solution with a ph between 7 and 14 would be a(n). 80. A solution with a ph between 0 and 7 would be a(n). 81. A solution with a ph of exactly 7.0 would be. 82. What is the molarity of a 500 ml solution that contains grams of NaCl? 83. A 2.4 g sample of a metal requires 6 J of energy to change its temperature from 18 C to 30 C. What is the specific heat of the sample? 84. Define a base: 85. Define an acid: 86. Define a salt: 87. What are the names for the following groups? IA IIA 1B - 7B VIIA VIIIA 88. What is the ph of a solution with a hydrogen ion concentration of 0.1 moles per liter? 89. What is the ph of a solution with a hydrogen ion concentration of 0.05 moles per liter? Given the structural formula for ethyne: H C C H, What is the total number of electrons shared between the two carbon atoms? 91. List at least 5 properties of acids and 5 properties of bases. Acid a. b. c. d. e. 92. Make a sketch below of the following orbitals (see chapter 5.1) s p d 93. Aluminum and hydrochloric acid are mixed resulting in the formation of aluminum chloride and hydrogen gas. Write the balanced equation for this reaction below: Base 6
7 At STP, what is the total number of liters of hydrogen gas produced when 6.00 moles of hydrochloric acid solution is completely consumed? 94. The temperature of a piece of lead with a mass of 110 g changes from 28.0 C to 48.0 C when the metal absorbs 283J of heat. What is the specific heat of the lead? 95. How many milliliters of 2 M HCI are needed to exactly neutralize 40 milliliters of 6 M Ca(OH) 2? 96. What is the poh of a solution if the [H + ] = 1 x 10-6 moles /L? 97. Hydrogen peroxide (H 2 O 2 ) decomposes into water and oxygen gas. Write a balanced equation of this reaction below: If 3.0 moles of hydrogen peroxide decomposes, what volume of oxygen gas is produced? 98. Balance the following equation: C 2 H 6 (g) + O 2 (g) CO 2 (g) + H 2 O (g) How many grams of O 2 (g) are needed to react completely with 2 moles of C 2 H 6 (g)? 99. What are the principle contributions of each of the following scientists to the creation of the modern model of the atom? (You may use pictures in as well as words in your answer.) JJ Thomson Ernest Rutherford Niels Bohr Modern Quantum (wave) Model 7
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