Name: ______________________
Class: _________________
Date: _________
Unit 1 Review - Intro to Chemistry
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. A theory is a ____.
a. proposed explanation for an observation
b. well-tested explanation for a broad set of observations
c. summary of the results of many observations
d. procedure used to test a proposed explanation
____
2. Which step in the scientific method requires you to use your senses to obtain information?
a. revising a hypothesis
c. making an observation
b. designing an experiment
d. stating a theory
____
3. The step that usually comes last in solving numeric problems is ____.
a. calculate
c. evaluate
b. measure
d. analyze
____
4. An example of an extensive property of matter is ____.
a.
b.
temperature
pressure
c.
d.
mass
hardness
____
5. All of the following are physical properties of matter EXCEPT ____.
a. mass
c. melting point
b. color
d. ability to rust
____
6. Which of the following are considered physical properties of a substance?
a. color and odor
c. malleability and hardness
b. melting and boiling points
d. all of the above
____
7. A vapor is which state of matter?
a. solid
b. liquid
c.
d.
gas
all of the above
____
8. Which state of matter expands when heated and is easy to compress?
a. gas
c. solid
b. liquid
d. all of the above
____
9. Which of the following is a physical change?
a. corrosion
c.
b. explosion
d.
evaporation
rotting of food
____ 10. Which of the following is a heterogeneous mixture?
a. air
c. steel
b. salt water
d. soil
1
ID: A
Name: ______________________
ID: A
____ 11. Which of the following is true about homogeneous mixtures?
a. They are known as solutions.
b. They consist of two or more phases.
c. They have compositions that never vary.
d. They are always liquids.
____ 12. Separating a solid from a liquid by evaporating the liquid is called ____.
a. filtration
c. solution
b. condensation
d. distillation
____ 13. A substance that can be separated into two or more substances only by a chemical change is a(n) ____.
a. solution
c. mixture
b. element
d. compound
____ 14. What distinguishes a substance from a mixture?
a. Substances are compounds, and mixtures are not.
b. Mixtures are groupings of elements, and compounds are not.
c. Samples of the same substance can have different intensive properties.
d. Mixtures can be separated physically, while compounds cannot.
____ 15. The first figure in a properly written chemical symbol always is ____.
a. boldfaced
c. italicized
b. capitalized
d. underlined
____ 16. Which of the following is used for chemical symbols today?
a. drawings
c. letters
b. icons
d. numbers
____ 17. The chemical symbol for iron is ____.
a. fe
b. FE
c.
d.
Fe
Ir
____ 18. Which of the following represents a compound?
a. H
c. H2 O
b. H-3
d. O-16
____ 19. The
a.
b.
c.
d.
chemical formula of a compound does NOT indicate the ____.
identity of the elements in the compound
how elements are joined in the compound
the composition of the compound
relative proportions of the elements in the compound
____ 20. What must occur for a change to be a chemical reaction?
a. There must be a change in chemical properties.
b. There must be a change in physical properties.
c. The change must involve a change in mass.
d. The change must involve a change in volume.
____ 21. Which of the following is NOT a physical change?
a. grating cheese
c. fermenting of cheese
b. melting cheese
d. mixing two cheeses in a bowl
2
Name: ______________________
ID: A
____ 22. Which of the following indicates that a chemical change has happened during cooking?
a. The food darkens.
b. Bubbles form in boiling water.
c. Butter melts.
d. Energy is transferred from the stove to a pan.
____ 23. Which of the following does NOT indicate that a chemical change may have taken place?
a. fracture formation
c. precipitate formation
b. gas production
d. energy transfer
____ 24. The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific
notation?
a.
b.
1.54 × 10
12
1.54 × 10
−12
m
m
c.
d.
1.54 × 10
10
1.54 × 10
−10
m
m
____ 25. The expression of 5008 km in scientific notation is ____.
a.
b.
3
5.008 × 10 km
50.08× 10
−4
km
c.
d.
5.008 × 10
−3
km
4
5.008 × 10 km
____ 26. Which of the following measurements contains two significant figures?
a. 0.004 00 L
c. 0.000 44 L
b. 0.004 04 L
d. 0.004 40 L
____ 27. Which of the following measurements is expressed to three significant figures?
a.
b.
0.007 m
7077 mg
c.
d.
−7
7.30 × 10 km
0.070 mm
____ 28. How many significant figures are in the measurement 0.003 4 kg?
a. two
c. five
b. four
d. This cannot be determined.
____ 29. How many significant figures are in the measurement 40,500 mg?
a. two
c. four
b. three
d. five
____ 30. How many significant figures are in the measurement 811.40 grams?
a. two
c. four
b. three
d. five
____ 31. What quantity is represented by the metric system prefix deci-?
a. 1000
c. 0.1
b. 100
d. 0.01
____ 32. What is the metric system prefix for the quantity 0.000 001?
a. centic. kilob. decid. micro-
3
Name: ______________________
ID: A
____ 33. Which of the following volumes is the smallest?
a. one microliter
c. one milliliter
b. one liter
d. one deciliter
Prefix
mega (M)
kilo (k)
Commonly Used Metric Prefixes
Meaning
1 million times larger than the unit it precedes
1000 times larger than the unit it precedes
10
3
10
deci (d)
10 times smaller than the unit it precedes
10
−1
centi (c)
100 times smaller than the unit it precedes
10
−2
milli (m)
micro (µ)
1000 times smaller than the unit it precedes
1 million times smaller than the unit it precedes
10
−6
10
nano (n)
1000 million times smaller than the unit it precedes
10
−9
pico (p)
1 trillion times smaller than the unit it precedes
10
−12
Factor
6
−3
____ 34. A train travels at a speed of 30 miles per hour. If 1 mile = 1.6 kilometers, how fast is the train traveling
in kilometers per minute?
a. 0.4 km/min
c. 0.8 km/min
b. 0.6 km/min
d. 1.0 km/min
____ 35. The density of mercury is 5,427 kg/(m3 ). If the density of water is 1.0 g/mL, will mercury float or sink in
water?
a. Mercury will float because the density of mercury is 0.005427 g/mL, which is less
than the 1.0 g/mL density of water.
b. Mercury will float because the density of mercury is 0.05427 g/mL, which is less than
the 1.0 g/mL density of water.
c. Mercury will sink because the density of mercury is 5.427 g/mL, which is greater than
the 1.0 g/mL density of water.
d. Mercury will sink because the density of mercury is 5,427 g/mL, which is greater than
the 1.0 g/mL density of water.
____ 36. Density is found by dividing ____.
a. mass by volume
b. volume by mass
c.
d.
mass by area
area by mass
3
____ 37. What is the density of an object having a mass of 8.0 g and a volume of 25 cm ?
a.
0.32 g/cm
b.
2.0 g/cm
3
3
3
c.
3.1 g/cm
d.
200 g/cm
3
____ 38. What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
a. 0.23 mL
c. 479 mL
b. 4.34 mL
d. none of the above
4
Name: ______________________
ID: A
____ 39. If the temperature of a piece of steel decreases, what happens to its density?
a. The density decreases.
b. The density increases.
c. The density does not change.
d. The density first increases, then decreases.
____ 40. What SI unit is used to measure the number of representative particles in a substance?
a. kilogram
c. kelvin
b. ampere
d. mole
____ 41. Avogadro's number of representative particles is equal to one ____.
a. kilogram
c. kelvin
b. gram
d. mole
____ 42. How many moles of tungsten atoms are in 4.8 × 10
a.
b.
2
8.0 × 10 moles
1
8.0 × 10 moles
c.
d.
____ 43. How many moles of silver atoms are in 1.8 × 10
a.
3.0 × 10
−4
b.
3.3 × 10
−3
20
25
atoms of tungsten?
1.3 × 10
−1
moles
1.3 × 10
−2
moles
atoms of silver?
c.
3.0 × 10
2
d.
1.1 × 10
44
____ 44. How many atoms are in 0.075 mol of titanium?
a.
1.2 × 10-25
c.
6.4 × 10
2
b.
2.2 × 10
24
d.
4.5 × 10
22
c.
3.49 × 10
−24
1.26 × 10
24
____ 45. How many molecules are in 2.10 mol CO 2 ?
a.
b.
2.53 × 10
24
3.79 × 10
24
molecules
molecules
d.
molecules
molecules
____ 46. How many atoms are in 3.5 moles of arsenic atoms?
a.
b.
5.8 × 10
−24
1
atoms
7.5 × 10 atoms
c.
d.
2.1 × 10
24
atoms
1.7 × 10
23
atoms
____ 47. Which of the following is NOT a true about atomic mass?
a. The atomic mass is 12 g for magnesium.
b. The atomic mass is the mass of one mole of atoms.
c. The atomic mass is found by checking the periodic table.
d. The atomic mass is the number of grams of an element that is numerically equal to
the mass in amu.
5
Name: ______________________
ID: A
____ 48. What is true about the molar mass of chlorine gas?
a. The molar mass is 35.5 g.
b. The molar mass is 71.0 g.
c. The molar mass is equal to the mass of one mole of chlorine atoms.
d. none of the above
____ 49. What is the molar mass of (NH 4 ) 2 CO 3 ?
a.
b.
144 g
138 g
c.
d.
96 g
78 g
____ 50. What is the mass in grams of 5.90 mol C 8 H 18 ?
a.
b.
0.0512 g
19.4 g
c.
d.
389 g
673 g
____ 51. What is the number of moles in 432 g Ba(NO 3 ) 2 ?
a.
b.
0.237 mol
0.605 mol
c.
d.
1.65 mol
3.66 mol
____ 52. What is the number of moles of beryllium atoms in 36 g of Be?
a. 0.25 mol
c. 45.0 mol
b. 4.0 mol
d. 320 mol
____ 53. How many moles of CaBr 2 are in 5.0 grams of CaBr 2 ?
1
a.
2.5 × 10
−2
mol
c.
4.0 × 10 mol
b.
4.2 × 10
−2
mol
d.
1.0 × 10 mol
c.
d.
2.2 g
3.0 g
3
____ 54. What is the mass of silver in 3.4 g AgNO 3 ?
a.
b.
0.025 g
0.64 g
____ 55. What is the mass of oxygen in 250 g of sulfuric acid, H 2 SO 4 ?
a.
b.
0.65 g
3.9 g
c.
d.
6
16 g
160 g
ID: A
Unit 1 Review - Intro to Chemistry
Answer Section
MULTIPLE CHOICE
1. ANS: B
PTS: 1
DIF: L1
REF: p. 23
OBJ: 1.3.2 Identify three steps in the scientific method.
STA: CLE3221.Inq.1 | CLE3221.Inq.2 | 3221.Inq.2 | 3221.Inq.3 | 3221.1 | SPI3221.T/E.1 |
SPI3221Inq.3 | SPI3221Inq.2
2. ANS: C
PTS: 1
DIF: L2
REF: p. 22
OBJ: 1.3.2 Identify three steps in the scientific method.
STA: CLE3221.Inq.1 | CLE3221.Inq.2 | 3221.Inq.2 | 3221.Inq.3 | 3221.1 | SPI3221.T/E.1 |
SPI3221Inq.3 | SPI3221Inq.2
3. ANS: C
PTS: 1
DIF: L2
REF: p. 29
OBJ: 1.4.2 Describe three steps for solving numeric problems
STA: CLE3221.Math.2
4. ANS: C
PTS: 1
DIF: L1
REF: p. 39
OBJ: 2.1.1 Identify the properties of matter as extensive or intensive.
STA: CLE3221.2.1 | CLE3221.Inq.2
5. ANS: D
PTS: 1
DIF: L1
REF: p. 40
OBJ: 2.1.2 Define physical property and list several common physical properties of substances.
STA: CLE3221.2.1 | 3221.2.1
6. ANS: D
PTS: 1
DIF: L2
REF: p. 40
OBJ: 2.1.2 Define physical property and list several common physical properties of substances.
STA: CLE3221.2.1 | 3221.2.1
7. ANS: C
PTS: 1
DIF: L1
REF: p. 42
OBJ: 2.1.3 Differentiate among the three states of matter. STA: CLE3221.2.3 | SPI3221.2.6
8. ANS: A
PTS: 1
DIF: L2
REF: p. 42
OBJ: 2.1.3 Differentiate among the three states of matter. STA: CLE3221.2.3 | SPI3221.2.6
9. ANS: C
PTS: 1
DIF: L2
REF: p. 42
OBJ: 2.1.4 Describe a physical change.
STA: CLE3221.2.1 | 3221.2.9 | 3221.2.9 | SPI3221.2.4
10. ANS: D
PTS: 1
DIF: L1
REF: p. 45
OBJ: 2.2.2 Distinguish between homogeneous and heterogeneous samples of matter.
STA: CLE3221.2.1 | 3221.2.1 | SPI3221.2.1
11. ANS: A
PTS: 1
DIF: L1
REF: p. 45
OBJ: 2.2.2 Distinguish between homogeneous and heterogeneous samples of matter.
STA: CLE3221.2.1 | 3221.2.1 | SPI3221.2.1
12. ANS: D
PTS: 1
DIF: L2
REF: p. 46
OBJ: 2.2.3 Describe two ways that components of mixtures can be separated.
STA: CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.Inq.3 | 3221.Inq.5 | SPI3221Inq.2 | SPI3221Inq.3
13. ANS: D
PTS: 1
DIF: L2
REF: p. 48
OBJ: 2.3.1 Explain the difference between an element and a compound.
STA: CLE3221.2.1 | 3221.2.1 | SPI3221.2.1
14. ANS: D
PTS: 1
DIF: L3
REF: p. 50 | p. 51
OBJ: 2.3.2 Distinguish between a substance and a mixture.
STA: CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.2.1 | 3221.Inq.5 | SPI3221.T/E.1
1
ID: A
15. ANS: B
PTS: 1
DIF: L1
REF: p. 51
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given
their symbols.
STA: SPI3221.1.2
16. ANS: C
PTS: 1
DIF: L1
REF: p. 51
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given
their symbols.
STA: SPI3221.1.2
17. ANS: C
PTS: 1
DIF: L1
REF: p. 51
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given
their symbols.
STA: SPI3221.1.2
18. ANS: C
PTS: 1
DIF: L1
REF: p. 51
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given
their symbols.
STA: SPI3221.1.2
19. ANS: B
PTS: 1
DIF: L2
REF: p. 52
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given
their symbols.
STA: SPI3221.1.2
20. ANS: A
PTS: 1
DIF: L1
REF: p. 53
OBJ: 2.4.1 Describe what happens during a chemical change.
STA: CLE3221.2.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.2.9 | 3221.2.9 | SPI3221.2.4
21. ANS: C
PTS: 1
DIF: L2
REF: p. 53
OBJ: 2.4.1 Describe what happens during a chemical change.
STA: CLE3221.2.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.2.9 | 3221.2.9 | SPI3221.2.4
22. ANS: A
PTS: 1
DIF: L2
REF: p. 54
OBJ: 2.1.4 Describe a physical change. | 2.4.1 Describe what happens during a chemical change.
STA: CLE3221.2.1 | CLE3221.2.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.2.9 | SPI3221.2.4
23. ANS: A
PTS: 1
DIF: L2
REF: p. 54
OBJ: 2.1.4 Describe a physical change. | 2.4.2 Identify four possible clues that a chemical change has
taken place.
STA: CLE3221.2.1 | CLE3221.2.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.2.9 | 3221.Inq.3 |
SPI3221.2.4
24. ANS: D
PTS: 1
DIF: L1
REF: p. 63
OBJ: 3.1.1 Convert measurements to scientific notation.
STA: CLE3221.Math.1 | 3221.Math.1 | SPI3221.Math.5
25. ANS: A
PTS: 1
DIF: L1
REF: p. 63
OBJ: 3.1.1 Convert measurements to scientific notation.
STA: CLE3221.Math.1 | 3221.Math.1 | SPI3221.Math.5
26. ANS: C
PTS: 1
DIF: L1
REF: p. 66
OBJ: 3.1.2 Distinguish among the accuracy, precision, and error of a measurement.
STA: CLE3221.Math.1 | CLE3221.Inq.3 | CLE3221.Inq.4 | 3221.Inq.12 | 3221.Inq.4 | 3221.Inq.6 |
SPI3221Inq.3 | SPI3221Inq.6
27. ANS: C
PTS: 1
DIF: L2
REF: p. 66
OBJ: 3.1.2 Distinguish among the accuracy, precision, and error of a measurement.
STA: CLE3221.Math.1 | CLE3221.Inq.3 | CLE3221.Inq.4 | 3221.Inq.12 | 3221.Inq.4 | 3221.Inq.6 |
SPI3221Inq.3 | SPI3221Inq.6
28. ANS: A
PTS: 1
DIF: L1
REF: p. 66
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: CLE3221.Math.1 | CLE3221.Inq.3 | 3221.Inq.7 | 3221.Inq.11
2
ID: A
29. ANS: B
PTS: 1
DIF: L1
REF: p. 66
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: CLE3221.Math.1 | CLE3221.Inq.3 | 3221.Inq.7 | 3221.Inq.11
30. ANS: D
PTS: 1
DIF: L1
REF: p. 66
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: CLE3221.Math.1 | CLE3221.Inq.3 | 3221.Inq.7 | 3221.Inq.11
31. ANS: C
PTS: 1
DIF: L1
REF: p. 74
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: CLE3221.Math.1 | 3221.Math.8 | SPI3221.Math.4
32. ANS: D
PTS: 1
DIF: L1
REF: p. 74
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: CLE3221.Math.1 | 3221.Math.8 | SPI3221.Math.4
33. ANS: A
PTS: 1
DIF: L1
REF: p. 74 | p. 75
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: CLE3221.Math.1 | 3221.Math.8 | SPI3221.Math.4
34. ANS: C
PTS: 1
DIF: L2
REF: p. 86
OBJ: 3.3.2 Apply the techniques of dimensional analysis to a variety of conversion problems. | 3.3.4
Convert complex units, using dimensional analysis.
STA: 3221.Math.2 | CLE3221.Math.1 | CLE3221.Math.2 | 3221.Math.9 | 3221.Inq.9 | SPI3221.Math.1
| SPI3221.Math.4
35. ANS: C
PTS: 1
DIF: L3
REF: p. 86
OBJ: 3.3.2 Apply the techniques of dimensional analysis to a variety of conversion problems. | 3.3.4
Convert complex units, using dimensional analysis.
STA: 3221.Math.2 | CLE3221.Math.1 | CLE3221.Math.2 | 3221.Math.9 | 3221.Inq.9 | SPI3221.Math.1
| SPI3221.Math.4
36. ANS: A
PTS: 1
DIF: L1
REF: p. 90 | p. 91
OBJ: 3.4.1 Calculate the density of a material from experimental data.
STA: CLE3221.Math.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.Math.3 | 3221.Math.7 | 3221.Inq.3 |
SPI3221.Math.5
37. ANS: A
PTS: 1
DIF: L2
REF: p. 90 | p. 91
OBJ: 3.4.1 Calculate the density of a material from experimental data.
STA: CLE3221.Math.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.Math.3 | 3221.Math.7 | 3221.Inq.3 |
SPI3221.Math.5
38. ANS: B
PTS: 1
DIF: L2
REF: p. 91
OBJ: 3.4.1 Calculate the density of a material from experimental data.
STA: CLE3221.Math.2 | CLE3221.Inq.2 | CLE3221.Inq.3 | 3221.Math.3 | 3221.Math.7 | 3221.Inq.3 |
SPI3221.Math.5
39. ANS: B
PTS: 1
DIF: L1
REF: p. 91
OBJ: 3.4.2 Describe how density varies with temperature.
STA: CLE3221.2.2 | SPI3221.2.5
40. ANS: D
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
41. ANS: D
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
42. ANS: B
PTS: 1
DIF: L2
REF: p. 290 | p. 291
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
3
ID: A
43. ANS: A
PTS: 1
DIF: L2
REF: p. 290 | p. 291
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
44. ANS: D
PTS: 1
DIF: L2
REF: p. 291 | p. 292
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
45. ANS: D
PTS: 1
DIF: L2
REF: p. 291 | p. 292
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
46. ANS: C
PTS: 1
DIF: L2
REF: p. 291 | p. 292
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: CLE3221.3.3 | 3221.3.6 | 3221.3.12 | 3221.Math.1
47. ANS: A
PTS: 1
DIF: L2
REF: p. 294
OBJ: 10.1.3 Distiguish between the atomic mass of an element and its molar mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | 3221.3.6 | 3221.Math.7 | SPI3221.3.1 | SPI3221.Math.5
48. ANS: B
PTS: 1
DIF: L2
REF: p. 294
OBJ: 10.1.3 Distiguish between the atomic mass of an element and its molar mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | 3221.3.6 | 3221.Math.7 | SPI3221.3.1 | SPI3221.Math.5
49. ANS: C
PTS: 1
DIF: L2
REF: p. 295 | p. 296
OBJ: 10.1.4 Describe how the mass of a mole of a compound is calculated.
STA: CLE3221.Math.1 | CLE3221.Math.2 | 3221.3.6 | 3221.Math.7 | SPI3221.3.1 | SPI3221.Math.5
50. ANS: D
PTS: 1
DIF: L2
REF: p. 297 | p. 298
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
51. ANS: C
PTS: 1
DIF: L2
REF: p. 299
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
52. ANS: B
PTS: 1
DIF: L2
REF: p. 299
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
53. ANS: A
PTS: 1
DIF: L2
REF: p. 299
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
54. ANS: C
PTS: 1
DIF: L2
REF: p. 298
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
4
ID: A
55. ANS: D
PTS: 1
DIF: L2
REF: p. 298
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance,
and moles to mass.
STA: CLE3221.Math.1 | CLE3221.Math.2 | CLE3221.Inq.2 | 3221.3.6 | 3221.3.12 | 3221.Math.13 |
SPI3221.3.5 | SPI3221.Math.5
5