MOD Chemistry I Level Final Exam Review
Name: __________________________________
Directions: Define each of the following key terms.
Key terms
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Qualitative
Quantitative
Chemical change
Physical change
Law of Conservation of Mass
Physical change
Chemical change
Mass
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Volume
Density
Precision
Accuracy
Temperature
Heat
Specific Heat
Absolute Zero
1. Classify each of the following as a chemical or physical change.
a. Dissolving salt in water:
b. Boiling water:
c. Ethanol evaporating:
d. Methane gas burning in the presence of oxygen:
e. Melting ice:
2. Does the particle drawing below illustrate a physical or chemical change?
Before
After
3. Does the particle drawing below illustrate a physical or chemical change?
Before
After
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4. TRUE or FALSE: During chemical and physical changes, mass always changes.
Directions: Given this graph, answer questions #5- 9.
Length in centimeters vs Length in inches
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y = 2.54x
Length (cm)
10
8
6
4
2
0
0
0.5
1
1.5
2
2.5
3
3.5
4
4.5
Length (in)
5. Which variable is the independent variable?
6. Which variable is the dependent variable?
7. What should the value of the y-intercept be? Why should it be that value?
8. Write the mathematical model/equation (y = mx +b) that describes your graph.
Be sure to:
 Substitute variable names for x and y.
 Abbreviate variable names.
 Include a value for slope.
 Include units for slope.
9. Write a “For Every” statement to relate the two variables of this graph in a scientific sentence.
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Directions: Given this graph of mass vs volume data, answer questions #10-14.
Substance
A
Substance
B
From the graph, estimate:
10. The mass of 4 mL of substance A:
11. The volume of 10 g of substance B:
12. Calculate the density of substance A and substance B. Show all your work and include appropriate
units.
13. Draw particle pictures comparing the volume of Solid A and Solid B when their mass is 40 g.
Substance A
Substance B
14. Determine whether substance A and B will sink or float when placed in a bucket of water.
A: sink float
B: sink
float
(circle correct response)
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15. Suppose you have two materials with different densities. In the boxes below, draw a diagram of
how matter might be packed differently in each material.
Less Dense Material
More Dense Material
16. Suppose you have two materials with the same density. In the boxes below, draw a diagram of
how matter might be packed in each material.
Same Density
Same Density
17. Suppose you have two materials with different densities. In the boxes below, draw a diagram of
how matter might be packed differently in each material.
Less Density
More Density
Directions: Predict the effect of changing P, V or T on any of the other variables.
18. When pressure increases, volume ________________
19. When pressure increases, temperature __________________.
20. When volume increases, temperature __________________.
21. When temperature increases, pressure__________________.
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Directions: Use the graphs below to answer questions #22-24:
22. Which graph above describes the relationship between pressure and volume?
23. Which graph above represents the relationship between pressure and absolute temperature?
24. Which graph above represents the relationship between the volume of a gas and the Celsius
temperature?
25. Draw particle pictures to represent the relationship between volume and pressure. When the
volume is 10 mL, the pressure is 200 kPa. When the volume decreases to 5 mL, the pressure
increases to 400 kPa. Assume constant n and T.
Before
After
26. Draw particle pictures to represent the relationship between volume and temperature. When the
volume is 12 mL the temperature is 180 K. When the volume increased to 20 mL, the temperature
increased to 300 K. Assume constant P and n.
Before
After
27. Draw particle pictures to represent the relationship between pressure and temperature. When the
temperature is 300 K, the pressure is 6 atm. When the temperature is increased to 400 K, the
pressure increases to 8 atm. Assume constant V and n.
Before
After
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Directions: Complete the following tables. Show work to justify your answers and include correct
units to receive full credit.
28.
A container of carbon dioxide has a volume of 375 cm3 and a pressure of 18 psi. If the container
is crushed down to a volume of 125 cm3, what is the new pressure? Include particle pictures
before and after.
Before:
P
T
V
After
n
Initial
Final
Effect
29.
The tire pressure is 30 psi when the car is in the driveway at 27 oC. Due to the friction between a
tire and the road surface, the temperature of the air inside a tire increases as one drives. What is
the pressure when the temperature of the air inside the tire increases to 57 oC? Include particle
pictures before and after.
Before:
P
T
V
After
n
Initial
Final
Effect
30. A gas in a sealed container exerts a pressure of 6.0 atm at 127oC. What is the new pressure when
the temperature inside the containers reaches 27oC? Include particle pictures before and after.
Before:
P
T
V
n
Initial
Final
Effect
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After
Directions: Ethanol, a clear, colorless liquid, is used as an alcohol fuel (often mixed with gasoline) and
in a wide variety of industrial processes. Ethanol is also used in antifreeze products for its low freezing
point.
D
31. According to this graph, when is ethanol a solid?
a) A
b) B
c) C
d) D
32. According to this graph, when is ethanol a liquid?
a) A
b) B
c) C
d) D
33. According to this graph, in what region is ethanol changing from a liquid to a gas?
a) A
b) B
c) C
d) D
34. According to this graph, what is the boiling point for ethanol?
a) -115 °C
b) 75 °C
c) 100 °C
35. According to this graph, at what time would ethanol be completely a liquid?
a) 50 seconds
b) 100 seconds
c) 200 seconds
Directions: A sample of water is heated from a liquid at 40oC to a gas at 110oC. Exam the following
heat curve and answer the questions below.
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36. For section QR of the graph, state what is happening to the water particles as heat is added.
37. For section RS of the graph, state what is happening to the water particles as heat is added.
Directions: Use the following choices for questions #38-42.
A. increasing
B. decreasing
C. the same
D. zero
38. During region B the thermal energy (ETH) is ______.
39. During region C the thermal energy (ETH) is ______.
40. During region A the phase energy (EPH) is ______.
41. During region C of the graph, the energy being absorbed is:
a. increasing the speed of the water particles
b. increasing the distance between the water particles
c. decreasing the speed of the water particles
42. During region B of the graph, the energy being absorbed is:
a. increasing the speed of the water particles
b. increasing the distance between the water particles
c. decreasing the speed of the water particles
43. Use an energy bar chart to represent the ways energy is stored and transferred as a cup of hot
chocolate cools while sitting on the counter. Identify and circle the correct region on the cooling
curve and include initial and final particle pictures.
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Particle Picture
Particle Picture
(Initial)
(Final)
44. Use an energy bar chart to represent the ways energy is stored and transferred when an ice cube
melts. Identify and circle the correct region on the heating curve and include initial and final
particle pictures.
Particle Picture
Particle Picture
(Initial)
(Final)
45. One of the ice cubes described in the previous question is in placed in a glass of room temperature
(25 ˚C) soda. Do separate bar charts for the ice cube and the soda.
Ice Cube
Soda
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Directions: Use the Energy Bar graph below for questions #46-30.
46. What phase of matter is represented in the final conditions?
a. Solid
b. Liquid
c. Gas
47.
How would you describe the motion and arrangement of the particles from the initial to final
conditions?
a. Particles move slower and closer together .
b. Particles move faster and farther apart.
c. Particles move at the same speed and the same spacing.
d. Not enough information.
48. Which term best describes what happens to this substance?
a. Melting
b. Freezing
c. Condensing
49.
d. Plasma
d. Boiling
What do you need to draw on the system circle between the energy bar graphs to represent the
correct energy flow?
a. An arrow into the system circle with 2 bars.
b. An arrow into the system circle with 4 bars.
c. An arrow out the system circle with 2 bars.
d. An arrow out the system circle with 4 bars.
Directions: For problems #50-52, include a sketch or either a heating or cooling curve. Show all work
in your calculations, including the formula and units used.
50. Calculate the Joules of energy needed to heat 460 g of water from 5°C to 95°C.
51. How much energy is released when cooling 100 g of water from 25 °C to 7.5 °C?
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52. Determine the amount of energy released when freezing 55 g of water.
53. A 60 g metal rod with an initial temperature of 75 °C gives off 1584 J of energy when placed in a
calorimeter filled with water. The final temperature of both water and metal is 15 °C. Calculate
the specific heat of the metal.
54. A piece of iron has a total mass of 48.0 grams. How many moles of iron atoms do
they contain?
55. A raindrop has a mass of 6.01g. How many moles of water (H2O) does a raindrop
contain?
56. How many molecules of water would you need to have 32.0 moles of H2O?
57. One box of Morton’s Salt contains 1.41 x 1023 “formula units” of NaCl. How many
moles of sodium chloride (NaCl) is this?
58. Calculate the mass percent % of oxygen, hydrogen, and carbon in baking soda
(sodium bicarbonate, NaHCO3).
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59. How many molecules of CO2 gas (carbon dioxide) are contained in a flask holding
55.0g of gas? CAUTION: This requires 2 differrent ratio calculation. 
60. A flask contains 73.4 g of ammonia, NH3.
a. How many moles of ammonia does it contain?
b. How many molecules are present in the sample?
61 a. How many particles are in 1 mole of anything?
b. Write a “For every… statement” for the number of atoms in 1 mole of gold.
62. Why do 1 mole of silver and 1 mole of platinum not have the same mass?
63. Draw a particle picture for solid iron, liquid water (H2O), and oxygen gas (O2).
64. Review and understand the Particle Picture T-notes worksheet on elements, compounds, and
mixture (both types of mixtures), atom, molecule, diatomic, monatomic. Be able to draw a particle
picture for each definition 
A
B
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C
D
E
AB
List all that apply:
1. Contains only diatomic elements.
2. Contains only compounds.
3. This box contains a pure compound.
4. Contains only elements (monatomic and diatomic).
5. This box contains a mixture of elements.
6. Contains only monatomic elements.
7. This box contains only a mixture of compounds
8. Contains only molecules.
9. This box contains a mixture of elements but no molecules.
10. Represents a mixture.
11. Contains a mixture of two monatomic elements.
65. Understand the separation techniques difference between mixtures versus compound. (Ws #1)
66. Distinguish between pure substance and mixtures
 A _________ substance has a definite set of characteristic properties (density, mp, bp), whereas a
_________ exhibits properties that are a mixture of the properties of the substance they contain.
 A pure substance is composed of one ________of particle, whereas mixtures contain more than one
kind of __________.
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67. Describe how one could use differences in characteristic properties to separate the components of a
mixture. Give 3 common examples used at home; type of separation technique ; and what physical
property makes this technique possible.
a.
b.
c.
68. Sketch particle diagrams that distinguish compounds, elements and mixtures
Compound
Element
Mixture
69. Distinguish elements from compounds in terms of differences in their properties.
70. What is a diatomic element? Give 2 examples.
71. A container contains 57.6 g of baking soda (NaHCO3). 27.4% of that mass is sodium (Na). How much
mass of sodium is that?
72. A similar chemical analysis is performed on a 500.0 g sample of the sugar isolated from a sample of
pure sugar cane. Analysis shows this sample contains 211.0 g of carbon, 32.5 g of hydrogen, and 256.5
g of oxygen. Determine the percent composition by mass of each element in the sugar cane sample.
73. A compound is composed of 7.20 g of carbon, 1.20 g of hydrogen, and 9.60 g of oxygen. The molar
mass of the compound in 180 g/mol. Determine the empirical and molecular formulas of this
compound.
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