Name ______Date ______Pd. _____
Final Exam Review GuideChemistry 2015
In addition to completing this review, students should study notes, labs, and homework assignments from this semester.
Significant Figures and Measurement:
1. Identify the number of sig figs for the following:
- 4.70b. 30.5c. 0.005300
d. 0.3005e. 1000g = 1kgf. 32 people
2. Complete the following problems using sig figs:
a. 45.789 + 2.34 + 33.3 =b. 4.987 X 3.89 X 0.9322 =
c. 900/0.9100 = d. (45.11 + 101.2) / 4.57 =
3. Express the following as standard notation:
a. 5.04 x 1013 metersb. 4.6 x 10-8 grams
c. 4.30 x 10-5 secondsd. 9.2 x 107 centimeters
4. Express the following in scientific notation:
a. 0.00000305b. 604 585 000 000 000 000
5. Using a ruler, determine the length (in cm) of the lines below as accurately as possible.
Please include uncertainty and correct number of sig figs in your measurement.
- ______
b. ______
6. If given a picture of a graduated cylinder, thermometer, etc...be able to measure to the correct
number of significant figures. Review old homework for practice.
7. What is the formula for calculating percent error? The density of aluminum is 2.70 g/cm3. A
student measures the density of Al in the lab to be 2.65 g/cm3. What is her percent error?
Stoichiometry: Be sure to show all work; use units; use sig figs.
8. 1.0 mole = ______L_, ______particles_, ______(g)
1.0 mol 1.0 mol 1.0 mol
9. Calculate the molar mass of (NH4)2CO3: ______
10. You have 26.4 grams of ammonia (NH3). 11. You have 9.03 X 1023 molecules of water
a. How many moles of ammonia is this? a. How many moles of water is this?
b. How many molecules of ammonia is this? b. How many grams of water is this?
c. How many liters would this amount of gas c. How many liters would this amount
occupy at STP? of water vapor occupy at STP?
12. Does a mole of O2 contain the same number of molecules as the number of atoms in a mole of Ca?
13. Does a mole of O2 have the same mass as a mole of Ca? Explain.
14. If you have 9.45 X 1024 formula units of NaCl do you have ...
a. more than a moleb. less than a molec. 1 mole
15. If you have 1.65 moles of sodium do you have ....
a. more than 6.02 X 1023 atomsb. less than 6.02 X 1023 atoms
16. If you have 28 g of magnesium do you have ....
a. more than 1 moleb. less than 1 molec. 1 mole
17. If you have 12.5 L of nitrogen gas do you have...
a. more than 1 moleb. less than 1 molec.1 mole
18. Consider the following equation: ____ CH4 + ____ O2 → ____ CO2 + ____ H2O
c. How many grams of CO2 can be formed from 35.0 grams of CH4? Oxygen is in excess.
19. Hydrogen and oxygen fill a small pipette. When ignited, water and energy are produced and the
pipette flies across the room. If 2.5 X1021 molecules of water are produced...
a. How many liters of oxygen reacted? b. How many liters of hydrogen reacted?
20. Potassium chlorate decomposes to produce potassium chloride and oxygen gas.
2 KClO3 →2 KCl + 3 O2
a. Calculate the volume of oxygen produced from the decomposition of 75.0 g of potassium chlorate.
b. Calculate the mass of potassium chloride produced from 75.0 g of potassium chlorate.
21. A 33.0 g sample of calcium hydroxide is reacted with excess phosphoric acid, according to the following
balanced chemical equation:3Ca(OH)2+ 2 H3PO4 → Ca3(PO4)2+ 6 H2O
a. How many grams of calcium phosphate theoretically could be produced?
b. If 43.8 grams of calcium phosphate are actually obtained in a laboratory experiment, what is the
percent yield?
22. Using the balanced equation:SiO2(s) + 3C(s) → SiC(s) + 2CO(g)
Limiting Reactant= ______
Excess Reactant = ______
a. Draw 5 SiO2 molecules and 9 carbon
atoms on the reactant side.
b. Determine the LR and ER.
c. Draw the molecules present after the reaction.
23. Using the balanced equation:2NO + O2→ 2NO2
Limiting Reactant= ______
Excess Reactant = ______
a. Draw 4 NO molecules and 4 oxygen
molecules on the reactant side.
b. Determine the LR and ER.
c. Draw the molecules present after the reaction.
Gas Laws
Constants: / Direct or Indirect? / Explain / Graph:Temp. and moles of gas
24. Complete the chart for: Pressure and Volume
25. Complete the chart for: Volume and Temperature
Constants: / Direct or Indirect? / Explain / Graph:Pressure and moles of gas
26. Complete the chart for: Pressure and Temperature
Constants: / Direct or Indirect? / Explain / Graph:Volume and moles of gas
27. Complete the chart for: Volume and Moles
Constants: / Direct or Indirect? / Explain / Graph:Pressure and temperature
28. What will be the initial temperature (in C) of a 3.0L container if its final temperature is 62C and
the size of the container is 6.2L?
29.Ammonia gas occupies a volume of 450. ml at a pressure of 720. mmHg. What volume will it
occupy at standard pressure (1.00 atm)?
30.How many moles of O2 gas are in a 50.0 L tank at 22.0 °C if the pressure reads 2000.0 psi?
(Conversion factor: 1.0 atm = 14.69 psi)
31. If 2.00 mol of gas occupies 4.50L at STP. How much of the same gas will occupy 3.00L at STP?
32. The air in a steel-belted tire is at a pressure of 29.8 psi at a temperature of 20.0°C. After the tire
is driven fast on a hot road, the temperature in the tire is 48°C. What is the tire’s new pressure?
33. A 2.0 liter container of nitrogen had a pressure of 3.2 atm. What volume would be necessary to
decrease the pressure to 1.0 atm?
34. Freon gas has a volume of 2.23 L, a pressure of 4.85 kPa, and a temperature of 1.00°C. Calculate
the volume at a pressure of 1.38 kPa and a temperature of 6.00 °C.
35. A gas occupies a volume of 3.5L at 35C. What will be the volume (in mL) of the gas when the
temperature is changed 53C?
36. What pressure will be exerted by 1.34 moles of NO2 gas that is contained in a 9.22 L vessel at
32.0 °C?
37. A sample of nitrogen is at 122°C and 1.07 atm. After cooling, the pressure is measured to be
0.880 atm. What is the new temperature in degrees Celsius?
38. If the initial volume of hydrogen gas is 10.0 ml at a pressure of 75.6 kPa and 60.0 °C, what is the
new volume at STP?
39. a. Be able to explain how gas laws and the relationship between pressure, volume, temperature,
and number of moles of gas apply to real world applications. Examples: Hot air balloons, scuba
diving, drinking through a straw, breathing, suction cups, vacuum cleaners, aerosol cans, etc...
b. With what two states of matter are you unlikely to have any personal experiences? Why?
40. Give two different ways to express STP.
41. How many liters of CO2 gas will form if 24 L of oxygen gas react (with excess CH4) at STP?
CH4 (g) + 2 O2 (g) CO2 (g) + H2O (g)
42. Finish these relationships
- 520 mmHg = ______atm
- 25.0 psi = ______kPa
- ______torr = 0.75 atm
- ______mmHg = 125 kPa
43. Finish these conversions:
a. ______C = 225 K
b. 12C = _____ K
44. When a gas is cooled (at constant volume) what happens to the
a. gas pressure
b. gas temperature
c. number of gas particles
Thermochemistry
45. Define specific heat (capacity).
46. Note these specific heats:
granite = 0.803 J/g°C; stainless steel = 0.51 J/g°C; zinc = 0.386 J/g°C; silver = 0.233 J/g°C
a. You have equal masses of each of the four substances at the same temperature, which would hold
the most heat? Explain.
b. If you have equal masses of each of the four substances above and supplied the same amount of kJ
of heat to each one, which would reach the highest temperature? Explain.
47. Calculate the energy required (in joules) to heat 29.2 g of Al from 27.2C to 41.5C. The specific
heat of Al is 0.91 J/g°C.
48. In lab, 1.3 grams of substance A went from 25°C to 46°C when 12 J of energy was transferred to
it. What is the specific heat capacity of substance A?
49. A 5.63 gram sample of substance B (specific heat capacity = 0.13 J/g°C) started at 21°C. If 8.1
joules of energy were added to the sample, what would the final temperature of the sample be?
50. Below is data collected in a lab in which a metal is heated and then placed in a calorimeter filled
with water. Find the specific heat of the unknown solid using the data. (The specific heat capacity
for water is 4.184 J/g°C)
Mass of the solid………………………………………………………………………………..49.51 g
Volume of water in the calorimeter (for water 1g/1mL)………………………………….....50.0 mL
Starting temperature of water in calorimeter………………………………………………...24.4°C
Highest temperature of water in calorimeter after the solid was immersed in it ………...27.2°C
Starting temperature of the metal…....……………………………………………………....100.0°C
51. Explain why the growing season in northern Ohio (which borders Lake Erie) is slightly longer than
in central Ohio (i.e. Columbus)(Think about the specific heat of water).
52. The amount of heat released from food when it burns can be determined in the laboratory. A frito chip is placed under a calorimeter filled with water and burned. The following data is collected.
Assume all the heat from the chip is absorbed by the water in the calorimeter.
Total mass of chip burned
/2.5 g
Mass of water in calorimeter
/115.5 g
Initial temperature of water
/24.3˚C
Final temperature of water
/87.4˚C
a. How many Joules of heat did the mass of chip that burned release?
b. How many kJ is this?
53. Define endothermic and exothermic reaction and label the boxes to show how heat flows.
Surroundings Surroundings
Feels hot or cold? Feels hot or cold?
∆H = + or - ∆H = + or -
54. Draw a potential energy diagram for the following data.
Label the diagram.
Energy needed to break the bonds(Activation Energy): / 40 kJEnergy released when bonds form: / 18 kJ
What is the ∆H:
55. Draw a potential energy diagram for the following data.
Label the diagram.
Energy needed to break the bonds(Activation Energy): / 35 kJEnergy released when bonds form: / 50 kJ
What is the ∆H:
56. When bonds are broken, energy is ______; when bonds form, energy is ______.
57. For the reactions that follow use the bond energies to calculate the change in enthalpy (∆H) for the reactions.
Determine if the reaction is endothermic or exothermic.
C2H4 + F2⇒ C2H2F2 + H2
2NBr3 + 3F2 ⇒ 2NF3 + 3Br2
58. Sketch a potential energy diagram for an endothermic and exothermic reaction. Label the following in
each diagram: exothermic, endothermic, Label the reactants and products in each diagram using: strong
bonds, weak bonds, more stable bonds, less stable bonds, high potential energy, low potential energy.
Reaction Rates and Equilibrium
59.a. What does the Collision Theory say?
b. What is needed for an effective collision?
60.a. What is a catalyst?
b. Draw a potential energy diagram showing how a catalyst changes the reaction rate.
61. Complete the following chart:
Draw a picture that illustrates low and high surface area. / Effect on reaction rate and why?Low SA / High SA
Draw a picture that illustrates low and high temperature. / Effect on reaction rate and why?
Low Temp / High Temp
Draw a picture that illustrates low and high concentration. / Effect on reaction rate and why?
Low conc / High conc
62. The following questions refer to the reversible reaction
a. At what minute was equilibrium established?
b. How does the shape of the graph indicate that the
equilibrium has been established?
c. Look closely at the slope of the graphs. Write a
balanced equation to represent this reaction.
63. Explain what is means when a reaction has reached equilibrium.
64. Why is equilibrium called a dynamic state?
65. What does Le Chatelier's Principle state?
66. Use the following equation for the following questions:
CO (g) + H2O (g) CO2(g) + H2 (g) ∆ H= -27.6 kJ
Which direction will the reaction shift if:
a. carbon dioxide is addedb. heat is addedc. the pressure decreases
d. water is removede. CO is addedf. the temperature drops
Acids and Bases:
67. Write the balanced ionization or dissociation equation for the following acids and bases.
State whether the compound is an acid or a base.
a. HC2H3O2b. KOH
c. Ca(OH)2d. HNO3
e. H2CO3f. H3PO4
g. HClh. Al(OH)3
68. What is the difference between a strong acid and a weak acid? A weak base and a strong base?
69. If the [H+] is 4.5 X 10-9 what is the [OH-]?
Is this solution an acid or a base?How do you know?
70. Draw a pH scale and label the following: Increasing [H+], acidic, Increasing [OH-], basic, neutral.
71. If the [OH-] is 4.3 X 10-8 what is the pH?Acid or base?
72. If the [H+] is 5.2 X 10-10 what is the pH?Acid or base?
73. If the pH = 4.6, what is the [H+] concentration?
74. Complete the chart.
[H+] / [OH-] / pH / Acid/base/neutral1.6 X 10-3 / 6.3 X 10-11
6.75
75. What is a neutralization reaction?
76. Complete the neutralization reactions below. Balance the equations.
HNO3 + Ca(OH)2 →
HCl + KOH →
77. What is the purpose of a titration?
78. An sample of 25 mL of HCl has been titrated with a 14 mL of NaOH that had a concentration of 5.55 M.
What is the concentration of the acid?
79. After adding 56 mL of a 2.15 M KOH, a 110 mL sample of HNO3 turns pink.
What is the molarity of the HNO3?
80. In the lab 0.650 moles of NaCl are dissolved in 75.0 mL of water. Calculate the molarity of the
NaCl solution.
81. 15 g of NaCl are dissolved in a volume of 75 mL. What is the molarity of the solution?
82. How many grams of NaOH would you need to add to 5.0 liters of water to make a 3.0 M
solution?
Good Luck on your Chemistry Exam!