Name_________________________Period_____

Multiple Choice Final Exam Review Honors/Gifted Chemistry

The Mole Chapter 10

1. Determine the molar mass of sulfuric acid.

2. How many moles are in 100.0 g methanol, CH3OH?

3. Calculate the number of atoms in each of the following. a) 2.15 moles of gold, Au

b) 25.8 g mercury, Hg

4. What is an empirical formula?

5. Determine the empirical formula for each of the following:

a) Hydrogen peroxide, H2O2 b) Hexane, C6H14

6. One of the substances in a new alkaline battery is composed of 63.0 g manganese and 37.0 g oxygen by mass. Determine the empirical formula of the compound in the battery.

Stoichiometry Chapter 11

7. What is stoichiometry?

8. What law governs balancing equations and, ultimately, stoichiometry?

9. When solid copper is added to nitric acid, copper(II) nitrate, nitrogen

dioxide, and water are produced. Write the balanced chemical equation for the reaction. List six mole ratios for the reactions.

10. When an antacid tablet dissolves in water, the fizz is due to a reaction between sodium hydrogen carbonate (sodium bicarbonate, NaHCO3) and citric acid (H3C6H5O7).

3NaHCO3(aq) + H3C6H5O7(aq) → 3CO2(g) + 3H2O(l) + Na3C6H5O7(aq) How many moles of carbon dioxide can be produced if one tablet containing 0.0119 mol NaHCO3 is dissolved?

11. Carbon dioxide is released into the atmosphere through the combustion of octane (C8H18) in gasoline. Write the balanced chemical equation for the combustion of octane and calculate the mass of octane needed to release 5.00 mol CO2.

Name_________________________Period_____

12. Ammonium nitrate (NH4NO3), an important fertilizer, produces N2O gas and H2O when it decomposes. Determine the mass of water produced from the decomposition of 25.0 g of solid ammonium nitrate.

13. What is meant by limiting reactant? Excess reactant?

14. Photosynthesis reactions in green plants use carbon dioxide

and water to produce glucose (C6H12O6) and oxygen. Write the balanced chemical equation for the reaction. If a plant has 88.0 g carbon dioxide and 64.0 g water available for photosynthesis, determine the limiting reactant and the maximum mass of glucose produced.

If this process occurs (with the amounts listed above) and 54.0g of glucose is produced, what is the percent yield?

15. What is the formula used for calculating percent yield?

16. Pure zirconium is obtained using the two-step Van Arkel process. In the first step, impure zirconium and iodine are heated to produce zirconium iodide (ZrI4). In the second step, ZrI4 is decomposed to produce pure zirconium.

ZrI4(s) → Zr(s) + 2I2(g) Determine the percent yield of zirconium if 45.0 g ZrI4 is decomposed and 5.00 g pure Zr is obtained.

Solutions Chapter 14

17. What is the difference between solute and solvent? Identify the solute and solvent in a sugar-water solution.

18. Explain the difference between saturated, unsaturated and supersaturated.

19. What is the rule for dissolving?

20. What is a polar molecule?

21. What is the most common polar solvent?

22. Predict if the following substances are soluble or insoluble in water:

• Ionic compounds ___________ • Hydrocarbons ______________ • Sugars _________________

Name_________________________Period_____

• Diatomic molecules ________________

23. What happens to the solubility of solids as temperature increases? Gases?

24. A small crystal of solute is added to a solution. For each scenario listed below, determine what can be concluded about the original solution.

a) The crystal dissolves b) The crystal settles to the bottom c) The crystal causes a large amount of precipitate to

form

25. What is a colligative property?

26. Calculate the percent by mass of 3.55 g NaCl dissolved in 88.6 water.

27. What is the molarity of the following solution? a) 1.35 mol H2SO4 in 2.00 L of solution

b) 2.48 g CaF2 in 375 mL of solution

28. At 90°C, 10 g of potassium chlorate is dissolved in 100 g of water. Is this solution saturated, unsaturated, or supersaturated?

29. How many grams of sodium nitrate are needed to saturate 100 g of water at 10°C?

30. If 12g of solute are needed to saturate 100g of water, how man grams of solute would be needed to saturate 30g of water?

31. Which substance shows the larges increase in solubility as the temperature is increased?

Acids & Bases Chapter 18

32. According to Arrhenius, acids donate _______________ ions in solution, while bases donate _______________ ions in solution.

33. According to the Brønsted-Lowry model of acids and bases, acids are considered hydrogen __________ and bases are hydrogen _______________.

34. Identify the conjugate acid-base pairs in the following

equations.

Name_________________________Period_____

a) HCOOH(aq) + H2O(l) ↔ HCOO-(aq) + H3O+(aq)

b) NH3(aq) + H2O(l) ↔ NH4

+(aq) + OH-(aq)

35. Acids taste __________ and bases taste __________. 36. Acids have a pH range from __________, with _____ being the

strongest. Bases have a pH range from __________, with _____ being the strongest.

37. Distinguish between a strong acid/base and a weak acid/base. Which would cause a light bulb to glow more brightly?

38. Name the following substances and indicate whether they are an acid or base.

a) HCl b) NaOH c) H3PO4 d) Mg(OH)2

39. An aqueous solution tastes sour and turns litmus red. Is the solution acidic or basic?

40. pH + pOH = _____ 41. What is a neutralization reaction? 42. Predict the products of the following neutralization reaction:

H2SO4 + NaOH → __________ + __________ 43. In a titration 33.21 mL of 0.3020M rubidium hydroxide solution

is required to exactly neutralize 20.00 mL hydrofluoric acid solution. What is the molarity of the hydrofluoric acid solution?

44. If an acid has a [H+] = 1.2 x 10-4 M, determine [OH-], pH and pOH.

45. A solution has a pH of 10. It would be __________ times more _______(acidic or basic) than a solution with a pH of 7.

46. What is the relationship between [H+] and [OH-] for a) An acidic solution? b) A basic solution? c) A neutral solution?

Thermochemistry Chapter 16

47. What is specific heat? What is this value for water?

48. What is the formula for calculating heat gained/lost in a chemical reaction?

49. Explain the difference between exothermic and endothermic

reactions.

Name_________________________Period_____

50. In which type of reaction is energy a reactant? In which type is

energy a product?

51. If q or ΔH is “+”, the reaction is endo/exo. If q is “–”, the reaction is endo/exo.

52. How much heat is absorbed by a 2000 g sample of granite as energy from the sun causes its temperature to change from 10°C to 29°C? The specific heat of granite is 0.803 J/g⋅°C.

53. The temperature of a piece of copper with a mass of 95.4 g

increases from 25.0°C to 48.0°C when the metal absorbs 849 J of heat. What is the specific heat of copper?

54. A piece of metal with a mass of 23 grams is heated to 100.0˚C and dropped into 35mL of water at 15.0˚C. If the final temperature of the lead and water is 18.2˚C, what is the specific heat of the metal?

55. Use the graph below and determine the activation energy and the ∆H for the forward reaction. Is the process endo or exothermic?

56. Draw an energy diagram for an exothermic reaction. Label ALL

parts.

57. What is entropy?

58. Identify the name of the following phase/state changes and label each as exothermic or endothermic.

Process Name of Phase

Endothermic or

Change in

Name_________________________Period_____

Change Exothermic entropy ∆S

Positive or negative

1. C3H8 (g) → C3H8 (l)

2. CO2 (s) → CO2 (g)

3. C10H8 (s) → C10H8 (l)

4. H2O (l) → H2O (s)

59. Use the heating curve below to answer the following questions.

a. What phases are present at each segment? b. Where is kinetic energy increasing?_____ c. What is the melting pt? _______ d. What is the boiling pt? ________ e. Where is potential energy increasing? ______

60. 2C5H10(g) + 10O2(g) 10H2O(g) + 5CO2(g) + 7018 kJ

a) How much heat is released if 23.0 grams of butane () is burned?

b) If 176 kJ of heat are released, how many grams of butane were burned?

c) What is the sign of ∆H?_____ What is the sign of ∆S? ______

d) When will this reaction be spontaneous?

61. When will the following reaction be spontaneous and why? Co(s) + S(s) + 2O2(g) →CoSO4(s) ∆H=-888.3 kJ/mol

Kinetics & Equilibrium Chapter 16-17

62. List the three states of matter in order of increasing molecular motion.

Name_________________________Period_____

63. Describe the arrangement of particles in a: a) solid. b) liquid. c) gas.

64. List four ways to increase the rate of a reaction.

65. How do you increase the surface area of a substance?

66. What is a catalyst? How does a catalyst work?

67. Write a rate law that is 2nd order with respect to [A] and 1st order with respect to [B].

a) If both [A] and [B] are tripled, what happens to the

rate?

68. Use the following data to determine the rate law for the reaction aA + bB → products.

Experimental Initial Rates for aA + bB → products

Trial Initial [A] (M)

Initial [B] (M)

Initial Rate (mol/(L�s))

1 0.100 0.100 2.00 × 10-3 2 0.200 0.100 4.00 × 10-3 3 0.200 0.200 16.0 × 10-3

69. What is chemical equilibrium?

70. State LeChatelier’s Principle.

71. If pressure on a gaseous system is increased, which way will the system shift?

72. If temperature of a system in increases, which way will the

system shift?

73. Use LeChatelier’s principle to predict how each of the following changes would affect this equilibrium? How would this change the concentration of H2?

H2(g) + CO2(g) ↔ H2O(g) + CO(g) + heat a) Adding H2O(g) to the system b) Removing CO(g) from the system

Name_________________________Period_____

c) Increasing the temperature of the system d) Decreasing the pressure of the system

74. Use the balanced equation from the question above to answer this question.

a) At equilibrium [H2] = 0.100 M, [CO2] = 0.0200 M, [H2O] = 0.025, and [CO] = 0.00032 M. Calculate Keq.

b) Now that you know the equilibrium constant, calculate the molarity of H2 if [CO2] = 0.0800 M, [H2O] = 0.0070, and [CO] = 0.002 M

Gases Chapter 13

75. What temperature scale has absolute zero as its starting point?

76. What is the value of absolute zero? What happens to

molecular motion at this temperature? 77. How is Celsius converted to Kelvin? What is -65°C on the

Kelvin scale?

78. Complete the following table involving gas laws. Gas Law Variables

Involved Mathematical

Equation Direct/Inve

rse Relationsh

ip

Example

Boyle’s Law

Charles’ Law

Gay-Lussac’s

Combined Gas Law

----- ------

Ideal Gas Law (Avogadro)

----- -----

Graham’s Law

79. A sample of oxygen gas occupies a volume of 250. mL at 740

torr pressure. What volume will it occupy at 800. torr pressure?

Name_________________________Period_____

80. A sample of nitrogen occupies a volume of 250 mL at 25°C.

What volume will it occupy at 95°C?

81. The pressure in an automobile tire is 1.88 atm at 25.0°C. What will be the pressure if the temperature warms up to 37.0°C?

82. A sample of nitrogen gas is stored in a 500.0 mL flask at 108 kPa and 10.0°C. The gas is transferred to a 750.0-mL flask at 21°C. What is the pressure of nitrogen in the second flask?

83. 1 mole of any gas will occupy __________ L at STP. 84. Carbon monoxide, CO, is a product of incomplete combustion of

fuels. Find the volume that 42 g of carbon monoxide gas occupies at STP.

85. What volume will 2.0 moles of nitrogen occupy at 720 mmHg

and 20°C?

86. When iron rusts, it undergoes a reaction with oxygen to form iron(III) oxide. Calculate the volume of oxygen gas at STP that is required to completely react with 52.0 g of iron.

87. What is the volume of 4.5 grams of chlorine gas at STP?

88. What volume of oxygen gas is needed for the complete combustion of 4.00L propane gas (C3H8)? Assume constant conditions.

89. Answer the following questions in regards to the following three balloons - Balloon A contains helium, balloon B contains nitrogen, and balloon C contains propane – all with the same volume and at the same conditions. a. Which one has the highest kinetic energy – why? b. Which one has the highest density – why? c. Which one would effuse at the fastest rate – why? 90. State Graham’s Law and give the equation.