Final Exam Review 2015 HONORS Chemistry Name ______________________________
For problems, you must show all work INCLUDING a formula, filling in the formula, the answer and unit for full credit.
Unit 1: Math and Moles: There will be 20 questions on your final from this section.
Define and give an example of each
Word
Define
1.
Accuracy
2.
Precision
3.
Qualitative
4.
Quantitative
5.
Physical Properties
6.
Extrinsic Properties
7.
Intrinsic Properties
8.
Chemical Properties
9.
Chemical changes
Example
10. Physical changes
11. Density
12. Mole
13. Molar mass
14. Molar Volume
15. Avogadro’s Number
16. Particles (in mole
conversions)
17. Atom (in mole
conversions)
18. Molecule (in mole
conversions)
19. Formula Unit (in
mole conversions)
20. Ion (in mole
conversions)
21. Molecular Formula
22. Empirical Formula
(word definition)
Number =
23. List the metric conversions for your class. ( ___ m= ____ km; etc.)
Convert the following:
24. 456 m to cm
25. 90.8 mm to m
26. 459 km to m
27. 0.158 um to Gm
28. List and define the parts of the scientific method.
29. Describe how to solve a density problem when you are given mass and volume and want density.
30. A box has a mass of 15.0 g and a volume of 45.0 mL. What is the density?
31. Describe how to solve a density problem when you want mass and are given density and volume.
32. A box has a density of 25.0 g/mL and a volume of 5.0 mL. What is the mass?
33. Describe how to solve a density problem when you want volume and are given mass and density.
34. A box has a density of 50.0 g/mL and a mass of 10.0 g. What is the volume?
35. Describe how to find the molar mass and what unit you would use.
36. Find the molar mass of: H2O, Zn3(PO4)2, C6H12O6
37. Describe how to find the % by mass given the formula.
38. Find the % by mass for each element in H2O, Zn3(PO4)2, C6H12O6
39. Describe how to convert from grams to moles.
40. Convert 16.0 g of helium to moles.
41. Convert 9.01 g of water to moles.
42. Describe how to convert from moles to grams.
43. Convert 5.6 moles of ZnCl2 to grams.
44. Convert .086 moles of lead (II) chloride to grams.
45. Describe how to convert from moles to particles.
46. Convert 1.5 moles of zinc acetate to particles (make sure to specify the particle!).
47. Convert 0.52 moles of carbon dioxide to particles.
48. Describe how to convert from particles to moles.
49. Convert 5 atoms of lithium to moles.
50. Convert 0.75 atoms of vanadium to moles.
51. Describe how to convert from moles to volume.
52. Convert 75 moles of helium to volume.
53. Convert 0.412 moles of hydrochloric acid (g) to volume.
54. Describe how to convert from volume to moles.
55. Convert 44.8 L of oxygen gas to moles
56. Convert 0.75 L iodine gas to moles
57. Describe how to convert from molar mass to molar volume.
58. Convert 100.0g hydrogen gas to liters.
59. Convert 0.89 g astatine gas to liters.
60. Describe how to convert from molar volume to molar mass.
61. Describe how to find empirical formula.
62. A compound is 94.1 % oxygen & the rest hydrogen. Find the empirical formula.
63. A compound if 53.0% aluminum & the rest oxygen. Find the empirical formula.
64. Describe how to find molecular formula.
65. A compound has a molar mass of 100. The mystery compound has the formula X 2Z4. If the empirical formula mass is
found to be 20, what is the molecular formula? (The most important person in the room is …)
66. A compound has a molar mass of 150. The mystery compound has the formula X4Z6. If the empirical formula mass is
found to be 50, what is the molecular formula? (The most important person in the room is …)
Unit 2: Thermo There will be 10 questions on your final from this section.
Define the following words and give an example of each.
Word
Definition
67. Endothermic
68. Exothermic
69. Phase Diagram
70. Heating Curve
Example
For each of the following phase changes, define it and tell if the process is endothermic or exothermic.
Phase change
Definition
Endothermic or exothermic
71. Deposition
72. Fusion
73. Condensation
74. Sublimation
75. Solidification
76. Vaporization
77. Label 1-5 of the phase diagram.
78. At 0C and 8 atm, what is the phase of matter?
79. In a thermo-chemical equation, the heat is on the right in a
2
1
3
___ reaction and the left in a ____ reaction.
5
80. In a thermo-chemical equation, the delta H is positive in a
___ reaction and negative in a ____ reaction.
4
81. 500 g of a metal is heated to 150C. When transferred to 200 g of
water, the water T rises from 20C to 50C. Assume no heat is lost.
The specific heat of water is 4.184 J/gC.
Find the specific heat of the metal.
82. Draw graphs of endothermic reaction and an exothermic reaction. In each graph, label the both axis, products,
reactants, & activation energy.
83. If the temperature of 600 g of ethanol (CH3CH2OH) decreases to 50 C from 150 C, how much energy was
released? The specific heat of ethanol is 2.44 J/g C.
84. Find the specific heat of an object with a mass of 250g that had a decrease of 10 C when 150 J of energy was
removed.
85. Describe in words what happens when you add a catalyst to a reaction.
86. Label the heating curve below. Make sure to label the axes, the states of matter, the phase changes, endo and exo
thermic and the boiling point and freezing point of water.
87. Explain why the temperature doesn’t change during a phase change on a heating curve.
88. Calculate the heat required to change 75.0 g of ice at -15.8 C to steam at 145 C.
(cwater=4.184 J/gC; cice = 2.06 J/gC; csteam= 2.06 J/gC;  Hvap = 40.7kJ/mol;  Hfus = 6.01 kJ/mol)
89. Find the H of the reaction below using:
C(s) + O2(g) CO2 (g) H = -393.5 kJ
H2 (g) + ½ O2 (g)  H2O (l)H=-285.5kJ
2C2H2(g) + 5O2(g)  4CO2(g) + H2O(l)
H = -2598.8 kJ
Target: C2H2 (g)  2 C(s) + H2 (g) H = ?
90. How much heat is evolved when 50.6 g oxygen is burned according to this equation? C(s) + O2(g) CO2 (g) H = -393.5 kJ
91. Calculate the heat required to freeze 456.36 g of liquid ethanol (C 2H5OH) at its freezing point.
( Hvap = 38.6kJ/mol;  Hfus = 4.94 kJ/mol)
92. If the T of 67.00 g of gold decreases from 150.0 to 70.0C, how much heat has been released? (specific heat of gold is 0.13 J/gC).
93. 46 g of metal is heated to 190C. When transferred to 50.0g H2O in a calorimeter, the water T raises from 25.6C to 35.3C.
Assume no heat is lost. Find the specific heat of the metal.
94. Find the Hrxn for 2F2 (g) + 2H2O (l)  4HF (g) + O2 (g) Hrxn=?
Given: F2(g) = 0kJ/mol; H2O (l)= -571.6 kJ/mol; HF(g)= -542.2kJ/mol; O2 (g)= 0kJ/mol
95. Find the Hrxn for 2F2 (g) + 2H2O (l)  4HF (g) + O2 (g) Hrxn=?
Given:F2(g) = 0kJ/mol; H2O (l)= -571.6 kJ/mol; HF(g)= -542.2kJ/mol; O2 (g)= 0kJ/mol
96. Write the thermochemical equation using the following information: H2O2(l) →2H2(g)+ O2(g) Hrxn = +188 kJ/mol Is this an
exothermic or endothermic equation? How do you know?
97. What is the specific heat of a metal with a temperature of a 50.0g sample is increased by 15.0 oC when 45.8 J of heat is added?
Unit 3: Nomenclature & Bonding There will be 10 questions on your final from this section.
Word
Define
98. Ionic Bond
99. Ion
100. Anion
101. Cation
102. Covalent Bond
103. Polar
104. Nonpolar
105. Metallic
106. Write the rules for writing and naming ionic compounds
107. Write the rules for writing and naming covalent compounds
108. Write the rules for writing and naming acidic compounds
109. Name the Following
110. Write formulas for the following:
111.
sodium fluoride
112. aluminum trichloride
113. carbon dioxide
114.
silver sulfate
115.
nitrogen dioxide
116.
lithium sulfide
117.
dinitrogen trisulfide
118.
Nitric acid
119.
Phosphorous acid
120.
Calcium phosphide
Example
121.
Sulfuric acid
Name the following compounds and molecules.
122. PbCl4
123. P4I7
124. AgCl
125. N6O10
126. H3PO4
127. CaS
128. (NH4)2SO3
129. Al2(CO3)3
130. HCl
131. KClO4
132. Si4Cl10
Unit 4 Reactions: There will be 10 questions on your final from this section.
Define the following and given an example:
Word
Definition
Generic Example:
Example
A + B  AB
133. Reactant
X
134. Product
X
135. Yield
X
136. Synthesis
137. Single Replacement
138. Decomposition
139. Double displacement
140. Combustion
141. Redox reaction
142. Oxidized
143. Reduced
144. Oxidizing agent
145. Reducing agent
146. Using a balanced chemical equation, how can you tell what the state of matter is? How do you show solid, liquid, gas &
aqueous in a balanced chemical equation? Give an example of each.
147. List the seven indicators of a chemical reaction.
148. List and give formulas of 7 Diatomic Elements
149. Balance the following equations and give the type of reaction.
150. ____________________
Sn +
P  Sn3P2
151. ____________________
AgNO3
+
Zn

Zn (NO3)2 +
Ag
152. ____________________
H2CO3 
153. ____________________
C2H6
+
H2O

154. ____________________
Na +
155. ____________________
MnCl 2 +
CO2 + H2O

O2
CO2
+
NaOH +
H2
AgNO3  Mn(NO3)2
156. ______________________
CaCO3
+
HCl
157. _____________________
C4H10 +
O2 

CaCl2
H2O
+
+
AgCl
H2CO3
CO2 + H2O
Predict the products, write and balance the following equations. Give the type of reaction.
158. Sodium + chlorine gas 
159. Aluminum oxide decomposes
160. copper + nickel (III) nitrite 
161. silver nitrate + potassium acetate
162. Combustion of C2H6O
163. Which of the questions 150-162 are redox? Identify what is being oxidized, reduced, the oxidizing agent and the reducing
agent.
164. Assign oxidation numbers
a.
KCl
b. Ca(ClO4)2
Unit 5 Stoichiometry – there will only be 6 questions from this section because we have not completed this unit
165.
Write the balanced chemical equation for the production of water from its elements.
Use this equation for the remaining questions.
166.
How many moles of hydrogen are needed to completely react 4.5 moles of oxygen gas?
167.
How many grams of water are produced when 3.0 moles of hydrogen gas completely react with excess
oxygen?
168.
How many moles of water are produced when 95 g of oxygen gas react completely?
169.
How many grams of oxygen are needed to completely react with 800. g of hydrogen gas?
170.
What volume of hydrogen gas is needed to produce 450 g of water?