Chemistry 2nd Semester Exam Study Guide
Chapter 8 CHEMICAL EQUATIONS AND REACTIONS
1.
2.
3.
4.
The Law of Conservation states that the total mass of the reactants must be_____?
Define coefficient.
To balance a chemical equation, it may be necessary to adjust the _______.
Write the word equation that shows the reaction of carbon and oxygen producing
carbon dioxide. (**HINT oxygen is written as: O2)
5. Balance the following equations and give the type:
Mg + O2  MgO
FeCl3 + Ca(OH)2  Fe(OH)3 + CaCl3
CaO + H2O  Ca(OH)2
6. Define Synthesis reaction and give the general formula.
7. Define decomposition reaction and give the general formula.
8. Define single displacement reaction and give the general formula.
9. Define double displacement reaction and give the general formula.
10. Define combustion reaction and give an example.
Chapter 9 STOICHIOMETRY
11. The coefficients in a chemical equation represent the relative numbers of ______ of
reactants and products.
12. A ________ chemical equation allows one to determine the mole ratio of any two
substances in the reaction.
13. To balance a chemical equation, it may be necessary to adjust the _____.
14. A chemical equation is ______ when the same number of each kind of atom appears in
the reactants and in the products.
15. In the reaction represented by the equation N2 + 3H2  2NH3, what is the mole ratio of
nitrogen to ammonia?
16. In the reaction represented by the equation 2Al2O3  4Al + 3O2, what is the mole ratio
of aluminum to oxygen?
17. In the reaction represented by the equation C + 2H2  CH4, what is the mole ratio of
hydrogen to methane?
18. The Haber process for producing ammonia commercially is represented by the equation
N2(g) + 3H2(g)  2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia
gas, how many moles of nitrogen gas are required?
19. In the equation 2KClO3  2KCl + 3O2, how many moles of oxygen are produced when
3.0 mol of KClO3 decompose completely?
20. For the reaction represented by the equation 2H2 + O2  2H2O, how many grams of
water are produced from 6.00 mol of hydrogen?
Chapter 10 STATES OF MATTER
21. According to the kinetic-molecular theory, particles of matter are in ______ motion.
22. The __________________ theory explains the behavior of solids, liquids and gases.
23. According to the kinetic-molecular theory, which is the most significant difference
between gases and liquids?
24. What determines the average kinetic energy of the molecules of any gas?
25. By which process do gases take the shape of their container?
26. According to the kinetic-molecular theory, how does a gas expand?
27. What happens to the volume of a gas during compression?
28. Which best describes the particles of a liquid compared to those of a gas?
29. The particles in a liquid are usually ______ in liquids that gases.
30. Describe vaporization.
31. What term best describes the process by which particles escape from the surface of a nonboiling liquid and enter the gas state?
32. A solid forms when the average energy of a substance's particles _____.
33. Which of these can happen due to decreasing the average energy of a liquid's particles?
(freezing, melting, vaporization, or a random arrangement)
34. Forces holding particles together are strongest in a (solid, liquid, or gas)
35. The energy of the particles in a solid is ____ than the energy of the particles in liquids
and gases.
36. The compressibility of solids is generally _____ than the compressibility of liquids and
gases.
37. ______ have a definite volume because the particles do not have a tendency to change
positions.
38. What is the process of a substance changing from a solid to a vapor without passing
through the liquid phase?
Chapter 11 GASES
39. What is STP? Give the values.
40. A pressure of 745 mm Hg equals
41. Convert the pressure 0.75 atm to mm Hg
42. Convert the pressure 2.50 atm to kPa.
43. A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant
temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm
Hg?
44. At 7.0C, the volume of a gas is 49 mL. At the same pressure, its volume is 74 mL at
what temperature?
45. The pressure of a sample of gas at 10.0C increases from 700. mm Hg to 900. mm Hg.
What is the new temperature?
46. The volume of a sample of oxygen is 300.0 mL when the pressure is 1.00 atm and the
temperature is 27.0C. At what temperature is the volume 1.00 L and the pressure 0.500
atm?
Chapter 12 SOLUTIONS
47. Which of the following has components in a non-uniform arrangement? Homogeneous
mixture or Heterogeneous mixture
48. A (heterogeneous or homogeneous) mixture always contains two or more substances that
are visibly distinguishable.
49. Which of the following is a heterogeneous mixture?
Water, whole wheat bread, sugar, sugar water solution
50. Which of the following is a homogeneous mixture?
Water, whole wheat bread, sugar, sugar water solution
51. All of the following are homogeneous mixtures except
Soil, gasoline, a sugar water solution, a salt water solution
52. Water in air is an example of which solute-solvent combination?
53. Carbon dioxide dissolved in water is an example of which solute-solvent combination?
54. Sugar dissolved in water is an example of which solute-solvent combination?
55. Oxygen in nitrogen is an example of which solute-solvent combination?
56. Which mixture contains visible particles that settle out unless the mixture is stirred?
Suspension, colloid, solution, homogeneous mixture
57. Which mixture contains particles that are in a dispersed phase and do not settle out?
Suspension, colloid, solution, homogeneous mixture
58. A metal solution is a(n)
Colloid, suspension, emulsion, alloy
59. List 3 things that will increase the rate of dissolving a solid in water.
60. ______ the temperature decreases the average kinetic energy of solvent molecules.
61. True or False. Stirring increases the rate of dissolution because it brings fresh solvent into
contact with the solute
62. Which of the following will dissolve most rapidly?
Sugar cubes in hot water
Sugar cubes in cold water
Powdered sugar in cold water
Powdered sugar in hot water
63. Which of the following will dissolve most slowly?
Small salt crystals in unstirred water
Small salt crystals in stirred water
Large salt crystals in unstirred water
Large salt crystals in stirred water
64. Raising the collision rate between solute and solvent (increases, decreases) the rate of
dissolution.
65. Raising solvent temperature causes solvent-solute collisions to become (more, less)
frequent and (more, less) energetic.
66. Which of the following is at equilibrium when undissolved solute is visible?
(An unsaturated solution, a saturated solution, a supersaturated solution)
67. If the amount of solute present in a solution at a given temperature is less than the
maximum amount that can dissolve at that temperature, the solution is said to be
(unsaturated, saturated, supersaturated)
68. Which of the following is likely to produce crystals if disturbed?
(An unsaturated solution, a saturated solution, a supersaturated solution)
69. As temperature increases, solubility of gases in liquids (increases, decreases).
70. Which of the following expresses concentration?
Molality, molarity, moles of solute per liter of solution, all listed
71. Which of the following is expressed in grams of solute instead of moles of solute?
Molarity, molality, neither
72. What is the molarity of a solution that contains 0.409 mol KCl in 8.98 L solution?
73. What is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg water? (molar
mass of KNO3 = 101.11 g/mol)