1. Introductory Chemistry, 3rd Edition Nivaldo Tro
Chapter 2
Measurement and
Problem Solving
Roy Kennedy
Massachusetts Bay Community College
Wellesley Hills, MA
2009, Prentice Hall

2. Tro's "Introductory Chemistry", Chapter 2
What Is a Measurement?
Quantitative = quantity and it must have a unit
Comparison to an agreed upon standard.
accuracy
Tro's "Introductory Chemistry", Chapter 2

3. Scientists have measured the average global temperature rise over the past century to be 0.6 °C
Quantity is 0.6 the unit is °C
Comparison to an agreed upon standard is Celsius temperature scale.
Accuracy: The confidence in the measurement is determined by looking at the last digit, here it is in the 1/10th’s position, so the certain is plus and minus 1/10 or between 0.5 and 0.7 °C.

4. A way of writing large and small numbers.
Scientific Notation
A way of writing
large and small numbers.
Tro's Introductory Chemistry, Chapter 2

5. Tro's "Introductory Chemistry", Chapter 2
Big and Small Numbers
The sun’s
diameter is
1,392,000,000 m.
We commonly measure objects that are many times larger or smaller than our standard of comparison.
Writing large numbers of zeros is tricky and confusing.
Not to mention there’s the 8-digit limit of your calculator!
An atom’s
average diameter is m.
Tro's "Introductory Chemistry", Chapter 2

6. Tro's "Introductory Chemistry", Chapter 2
Exponents
When the exponent on 10 is positive, it means the number is that many powers of 10 larger.
Sun’s diameter = x 109 m = 1,392,000,000 m.
When the exponent on 10 is negative, it means the number is that many powers of 10 smaller.
Average atom’s diameter = 3 x 10-10m = m
Tro's "Introductory Chemistry", Chapter 2

7. Tro's "Introductory Chemistry", Chapter 2
Scientific Notation
To compare numbers written in scientific notation:
First compare exponents on 10.
If exponents are equal, then compare decimal numbers
1.23 x
10-8
Decimal part
Exponent part
Exponent
1.23 x 105 > 4.56 x 102
4.56 x 10-2 > 7.89 x 10-5
7.89 x 1010 > 1.23 x 1010
Tro's "Introductory Chemistry", Chapter 2

8. Writing a Number in Scientific Notation, Continued
12340
1. Locate the decimal point.
12340.
2. Move the decimal point to obtain a number between 1 and 10.
1.234
3. Multiply the new number by 10n .
Where n is the number of places you moved the decimal point.
1.234 x 104
4. If you moved the decimal point to the left, then n is +; if you moved it to the right, then n is − .
Tro's "Introductory Chemistry", Chapter 2

9. Writing a Number in Scientific Notation, Continued
1. Locate the decimal point.
2. Move the decimal point to obtain a number between 1 and 10.
1.2340
3. Multiply the new number by 10n .
Where n is the number of places you moved the decimal point.
x 104
4. If you moved the decimal point to the left, then n is +; if you moved it to the right, then n is − .
x 10-4
Tro's "Introductory Chemistry", Chapter 2

10. Writing a Number in Standard Form
1.234 x 10-6
Since exponent is -6, make the number smaller by moving the decimal point to the left 6 places.
When you run out of digits to move around, add zeros.
Add a zero in front of the decimal point for decimal numbers.
Tro's "Introductory Chemistry", Chapter 2

11. Practice—Write the Following in Scientific Notation, Continued
123.4 = x 102
= 1.45 x 105
25.25 = x 101
1.45 = 1.45 x 100
= x 100
= 2.34 x 10-3
= 1.23 x 10-2
= x 10-6
Tro's "Introductory Chemistry", Chapter 2

12. Practice—Write the Following in Standard Form, Continued
2.1 x 103 = 2100
9.66 x 10-4 =
6.04 x 10-2 =
4.02 x 100 = 4.02
3.3 x 101 = 33
1.2 x 100 = 1.2
Tro's "Introductory Chemistry", Chapter 2

13. Tro's "Introductory Chemistry", Chapter 2
Numbers
Exact
Measured: Significant Figures
Tro's "Introductory Chemistry", Chapter 2

14. Exact Numbers vs. Measurements
Exact: Sometimes you can determine an exact value for a quality of an object.
Often by counting.
Pennies in a pile.
Sometimes by definition
1 ounce is exactly 1/16th of 1 pound.
Measured: Whenever you use an instrument to compare a quality of an object to a standard, there is uncertainty in the comparison.
Tro's "Introductory Chemistry", Chapter 2

15. Tro's "Introductory Chemistry", Chapter 2
Exact Numbers
Exact numbers have an unlimited number of significant figures.
A number whose value is known with complete certainty is exact.
From counting individual objects.
From definitions.
1 cm is exactly equal to 0.01 m.
$.05 = $
12 inches = ft
Tro's "Introductory Chemistry", Chapter 2

16. 4 fundamental measuring instruments
Length
Mass
Time
Temperature
Tro's "Introductory Chemistry", Chapter 2

17. How do we make a Measurement
Measurements are written to indicate the uncertainty in the measurement.
The system of writing measurements we use is called significant figures.
When writing measurements, all the digits written are known with certainty except the last one, which is an estimate.
45.872
Certain
Estimated
45.872
Tro's "Introductory Chemistry", Chapter 2

18. Reading a Measuring Instrument/Device
For any Digital Device record ALL the digits

19. Reading a Measuring Instrument/Device
Record all the numbers you can see
Make ONE Guess!

20. Skillbuilder 2.3—Reporting the Right Number of Digits
A thermometer used to measure the temperature of a backyard hot tub is shown to the right. What is the temperature reading to the correct number of digits?
Tro's "Introductory Chemistry", Chapter 2

21. Skillbuilder 2.3—Reporting the Right Number of Digits
A thermometer used to measure the temperature of a backyard hot tub is shown to the right. What is the temperature reading to the correct number of digits?
103.4 °F
Tro's "Introductory Chemistry", Chapter 2

22. What is the Length? We can see the markings between 1.6-1.7cm
We can’t see the markings between the .6-.7
We must guess between .6 & .7
We record 1.67 cm as our measurement

23. What is the length of the wooden stick?
1) cm
2) cm
3) cm

24. ?
8.00 cm or 3 (2.2/8)

25. Counting Significant Figures
All non-zero digits are significant.
1.5 has 2 significant figures.
Interior zeros are significant.
1.05 has 3 significant figures.
Trailing zeros after a decimal point are significant.
1.050 has 4 significant figures.
Tro's "Introductory Chemistry", Chapter 2

26. Counting Significant Figures, Continued
Leading zeros are NOT significant.
has 4 significant figures.
1.050 x 10-3
Zeros at the end of a number without a written decimal point are NOT significant
If 150 has 2 significant figures, then 1.5 x 102, but if 150 has 3 significant figures, then 1.50 x 102.
Tro's "Introductory Chemistry", Chapter 2

27. Tro's "Introductory Chemistry", Chapter 2
Example 2.4—Determining the Number of Significant Figures in a Number, Continued
How many significant figures are in each of the following numbers?
significant figures—leading zeros are not significant.
significant figures—trailing and interior zeros are significant.
significant figures—All digits are significant.
2.97 × significant figures—Only decimal parts count as significant.
1 dozen = 12 Unlimited significant figures—Definition
100, , no decimal
Tro's "Introductory Chemistry", Chapter 2

28. Determine the Number of Significant Figures,
12000
120.
12.00
1.20 x 103 2 3 4
0.0012
1201 2 3 4
Tro's "Introductory Chemistry", Chapter 2

29. How many sig figs? 6 3 5 2 4
All digits count
Leading 0’s don’t
Trailing 0’s do
0’s count in decimal form
0’s don’t count w/o decimal
0’s between digits count as well as trailing in decimal form
48000.
48000
3.982106

30. Tro's "Introductory Chemistry", Chapter 2
Rounding
When rounding to the correct number of significant figures, if the number after the place of the last significant figure is:
0 to 4, round down.
Drop all digits after the last significant figure and leave the last significant figure alone.
5 to 9, round up.
Drop all digits after the last significant figure and increase the last significant figure by one.
Tro's "Introductory Chemistry", Chapter 2

31. Examples of Rounding For example you want a 4 Sig Fig number
0 is dropped, it is <5
8 is dropped, it is >5; Note you must include the 0’s
5 is dropped it is = 5; note you need a 4 Sig Fig
780,582
1999.5
4965
780,600
2000.

32. Multiplication and Division with Significant Figures
When multiplying or dividing measurements with significant figures, the result has the same number of significant figures as the measurement with the fewest number of significant figures.
× , × = = 45
3 sig. figs sig. figs sig. figs. 2 sig. figs.
÷ 6.10 = =
4 sig. figs sig. figs sig. figs.
Tro's "Introductory Chemistry", Chapter 2

33. Tro's "Introductory Chemistry", Chapter 2
Determine the Correct Number of Significant Figures for Each Calculation and
1.01 × 0.12 × ÷ 96 = = 0.068
56.55 × ÷ = = 1.52
Result should
have 2 sf.
7 is in place
of last sig. fig.,
number after
is 5 or greater,
so round up.
3 sf
2 sf
4 sf
2 sf
4 sf
Result should
have 3 sf.
1 is in place
of last sig. fig.,
number after
is 5 or greater,
so round up.
3 sf
6 sf
Tro's "Introductory Chemistry", Chapter 2

34. Addition/Subtraction ‑

35. Addition and Subtraction with Significant Figures
When adding or subtracting measurements with significant figures, the result has the same number of decimal places as the measurement with the fewest number of decimal places.
= = 9.21
2 dec. pl dec. pl dec. pl. 2 dec. pl.
= =
1 dec. pl dec. pl dec. pl.
Tro's "Introductory Chemistry", Chapter 2

36. Tro's "Introductory Chemistry", Chapter 2
Determine the Correct Number of Significant Figures for Each Calculation and Round and Report the Result, Continued
– 1.22 = =
0.764 – – 5.98 = =
3 dp
Result should
have 1 dp.
8 is in place
of last sig. fig.,
number after
is 5 or greater,
so round up.
1 dp
2 dp
Result should
have 2 dp.
6 is in place
of last sig. fig.,
number after
is 4 or less,
so round down.
3 dp
3 dp
2 dp
Tro's "Introductory Chemistry", Chapter 2

37. Addition and Subtraction
Look for the last important digit
.71
82000 .1
= .713 = =
10 – =
__ ___ __

38. Tro's "Introductory Chemistry", Chapter 2
Both Multiplication/Division and Addition/Subtraction with Significant Figures
When doing different kinds of operations with measurements with significant figures, evaluate the significant figures in the intermediate answer, then do the remaining steps.
Follow the standard order of operations.
Please Excuse My Dear Aunt Sally.
× ( – ) =
2 dp dp
× = 12
4 sf dp & 2 sf 2 sf
Tro's "Introductory Chemistry", Chapter 2

39. Tro's "Introductory Chemistry", Chapter 2
Example 1.6—Perform the Following Calculations to the Correct Number of Significant Figures, Continued b)
Tro's "Introductory Chemistry", Chapter 2

40. Tro's "Introductory Chemistry", Chapter 2
Basic Units of Measure
Tro's "Introductory Chemistry", Chapter 2

41. Tro's "Introductory Chemistry", Chapter 2
Units
Units tell the standard quantity to which we are comparing the measured property.
Without an associated unit, a measurement is without meaning.
Scientists use a set of standard units for comparing all our measurements.
So we can easily compare our results.
Each of the units is defined as precisely as possible.
Tro's "Introductory Chemistry", Chapter 2

42. The Standard Units
Scientists generally report results in an agreed upon International System.
The SI System
Aka Système International
Quantity
Unit
Symbol
Length
meter m
Mass
kilogram
Kg/g
Volume
liter L
Time
second s
Temperature
kelvin K

43. Volume
1 mL = 1 cm3

44. Related Units in the SI System
All units in the SI system are related to the standard unit by a power of 10.
The power of 10 is indicated by a prefix.
Tro's "Introductory Chemistry", Chapter 2

45. Common Prefixes in the SI System
Symbol
Decimal
Equivalent
Power of 10
mega- M
1,000,000
Base x 106
kilo- k
1,000
Base x 103
deci- d
0.1
Base x 10-1
centi- c
0.01
Base x 10-2
milli- m
0.001
Base x 10-3
micro-
Base x 10-6
nano- n
Base x 10-9
Pico- p
Base x 10-12

46. Measurements and SI gram g meter m liter L seconds s Kelvin K M
1,000,000 k
1,000 d
0.1 c
0.01 m
0.001 n p
gram g
meter m
liter L
seconds s
Kelvin K

47. Tro's "Introductory Chemistry", Chapter 2
Measurements and SI
liter L m
0.001
(m = .001)L
mL = .001L
or mL = L
Tro's "Introductory Chemistry", Chapter 2

48. Prefixes Used to Modify Standard Unit
kilo = 1000 times base unit = 103
k= or k = 103
1 kg = 103g
nano = 10-9 times the base unit
n= or n = 10-9
1 nL = 10-9L
Tro's "Introductory Chemistry", Chapter 2

49. Tro's "Introductory Chemistry", Chapter 2
Units
Always write every number with its associated unit.
Always include units in your calculations.
You can do the same kind of operations on units as you can with numbers.
cm × cm = cm2
cm + cm = 2cm
cm ÷ cm = 1
Using units as a guide to problem solving is called dimensional analysis.
Tro's "Introductory Chemistry", Chapter 2

50. Problem Solving and Dimensional Analysis, Continued
Arrange conversion factors so the starting unit cancels.
Arrange conversion factor so the starting unit is on the bottom of the conversion factor.
May string conversion factors.
So we do not need to know every relationship, as long as we can find something else the starting and desired units are related to :
Tro's "Introductory Chemistry", Chapter 2

51. Problem Solving and Dimensional Analysis
Many problems in chemistry involve using relationships to convert one unit of measurement to another.
Conversion factors are relationships between two units.
May be exact or measured.
Both parts of the conversion factor have the same number of significant figures.
Conversion factors generated from equivalence statements.
e.g., 1 inch = 2.54 cm can give or
Tro's "Introductory Chemistry", Chapter 2

52. Tro's "Introductory Chemistry", Chapter 2
Systematic Approach
1. Write down the given amount and unit.
2. Write down what you want to find and unit.
3. Write down needed conversion factors or equations.
a. Write down equivalence statements for each relationship.
b. Change equivalence statements to conversion factors with starting unit on the bottom.
Tro's "Introductory Chemistry", Chapter 2

53. Systematic Approach, Continued
4. Design a solution map for the problem.
Order conversions to cancel previous units or
arrange equation so the find amount is isolated.
5. Apply the steps in the solution map.
Check that units cancel properly.
Multiply terms across the top and divide by each bottom term.
6. Determine the number of significant figures to report and round.
7. Check the answer to see if it is reasonable.
Correct size and unit.
Tro's "Introductory Chemistry", Chapter 2

54. Tro's "Introductory Chemistry", Chapter 2
Conversion Factors
Convert inches into centimeters.
1. Find relationship equivalence: 1 in = 2.54 cm
2. Write solution map. in cm
3. Change equivalence into conversion factors with starting units on the bottom.
Tro's "Introductory Chemistry", Chapter 2

55. Tro's "Introductory Chemistry", Chapter 2
Example 2.8:
Convert 7.8 km to miles
Tro's "Introductory Chemistry", Chapter 2

56. Example: Convert 7.8 km to miles.
Write down the given quantity and its units.
Given: 7.8 km
Tro's "Introductory Chemistry", Chapter 2

57. Example: Convert 7.8 km to miles.
Information
Given: 7.8 km
Write down the quantity to find and/or its units.
Find: ? miles
Tro's "Introductory Chemistry", Chapter 2

58. Example: Convert 7.8 km to miles.
Information
Given: 7.8 km
Find: ? mi
Collect needed conversion factors:
1 km = mile
Tro's "Introductory Chemistry", Chapter 2

59. Example: Convert 7.8 km to miles.
Information
Given: 7.8 km
Find: ? mi
Conversion Factor:
1 km = mile
Write a solution map for converting the units: km mi
Tro's "Introductory Chemistry", Chapter 2

60. Example: Convert 7.8 km to miles.
Information
Given: 7.8 km
Find: ? mi
Conversion Factor:1 km = mile
Solution Map: km  mi
2 significant figures
Apply the solution map:
= mi
Significant figures and round:
2 significant figures
= 4.8 mi
Tro's "Introductory Chemistry", Chapter 2

61. Practice—Convert 30.0 g to Ounces (1 oz. = 28.35 g)
Tro's "Introductory Chemistry", Chapter 2

62. Units and magnitude are correct.
Convert 30.0 g to Ounces
Write down the Given quantity and its unit.
Given:
30.0 g
3 sig figs
Write down the quantity you want to Find and unit.
Find:
oz.
Write down the appropriate Conversion Factors.
Conversion Factor:
1 oz = g
Write a Solution Map.
Solution
Map: g oz
Follow the solution map to Solve the problem.
Solution:
Significant figures and round.
Round:
= 1.06 oz
3 sig figs
Check.
Check:
Units and magnitude are correct.

63. Tro's "Introductory Chemistry", Chapter 2
Example 2.10:
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Tro's "Introductory Chemistry", Chapter 2

64. Tro's "Introductory Chemistry", Chapter 2
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Write down the given quantity and its units.
Given: 0.75 L
Tro's "Introductory Chemistry", Chapter 2

65. Tro's "Introductory Chemistry", Chapter 2
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Information
Given: 0.75 L
Write down the quantity to find and/or its units.
Find: ? cups
Tro's "Introductory Chemistry", Chapter 2

66. Tro's "Introductory Chemistry", Chapter 2
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Information
Given: 0.75 L
Find: ? cu
Collect needed conversion factors:
4 cu = 1 qt
1.057 qt = 1 L
Tro's "Introductory Chemistry", Chapter 2

67. Tro's "Introductory Chemistry", Chapter 2
Information
Given: 0.75 L
Find: ? cu
Conversion Factors:
4 cu = 1 qt;
1.057 qt = 1 L
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Write a solution map for converting the units: L qt cu
Tro's "Introductory Chemistry", Chapter 2

68. Tro's "Introductory Chemistry", Chapter 2
An Italian recipe for making creamy pasta sauce calls for 0.75 L of cream. Your measuring cup measures only in cups. How many cups should you use?
Information
Given: 0.75 L
Find: ? cu
Conversion Factors:
4 cu = 1 qt; qt = 1 L
Solution Map: L  qt  cu
2 significant figures
Apply the solution map:
= cu
Significant figures and round:
2 significant figures
= 3.2 cu
Tro's "Introductory Chemistry", Chapter 2

69. Tro's "Introductory Chemistry", Chapter 2
Example 2.12:
A circle has an area of 2,659 cm2. What is the area in square meters?
Tro's "Introductory Chemistry", Chapter 2

70. Tro's "Introductory Chemistry", Chapter 2
Example: A circle has an area of 2,659 cm2. What is the area in square meters?
Write down the given quantity and its units.
Given: 2,659 cm2
Tro's "Introductory Chemistry", Chapter 2

71. Tro's "Introductory Chemistry", Chapter 2
Example: A circle has an area of 2,659 cm2. What is the area in square meters?
Information
Given: 2,659 cm2
Write down the quantity to find and/or its units.
Find: ? m2
Tro's "Introductory Chemistry", Chapter 2

72. Tro's "Introductory Chemistry", Chapter 2
Example: A circle has an area of 2,659 cm2. What is the area in square meters?
Information
Given: 2,659 cm2
Find: ? m2
Collect needed conversion factors:
1 cm = 0.01m
Tro's "Introductory Chemistry", Chapter 2

73. Tro's "Introductory Chemistry", Chapter 2
Example: A circle has an area of 2,659 cm2. What is the area in square meters?
Information
Given: 2,659 cm2
Find: ? m2
Conversion Factor:
1 cm = 0.01 m
Write a solution map for converting the units:
cm2 m2
Tro's "Introductory Chemistry", Chapter 2

74. Tro's "Introductory Chemistry", Chapter 2
Example: A circle has an area of 2,659 cm2. What is the area in square meters?
Information
Given: 2,659 cm2
Find: ? m2
Conversion Factor:1 cm = 0.01 m
Solution Map: cm2  m2
4 significant figures
Apply the solution map:
= m2
Significant figures and round:
4 significant figures
= m2
Tro's "Introductory Chemistry", Chapter 2

75. Practice—Convert 30.0 cm3 to ft3 (1 cm = 1 x 10-2 m) (in class)
Tro's "Introductory Chemistry", Chapter 2

76. Units and magnitude are correct.
Convert 30.0 cm3 to m3
Write down the Given quantity and its unit.
Given:
30.0 cm3
3 sig figs
Write down the quantity you want to Find and unit.
Find:
? m3
Write down the appropriate Conversion Factors.
Conversion Factor:
(1 cm = 0.01 m)3
Write a Solution Map.
Solution
Map:
cm3 m3
Follow the solution map to Solve the problem.
Solution:
Significant figures and round.
Round:
30.0 cm3 = 3.00 x 10−5 m3
3 sig figs
Units and magnitude are correct.
Check.
Check:

77. Tro's "Introductory Chemistry", Chapter 2
Density
Inverse relationship between mass and volume.
Solids = g/cm3
1 cm3 = 1 mL
Liquids = g/mL
Gases = g/L
Volume of a solid can be determined by water displacement—Archimedes Principle.
Density : solids > liquids > gases
Except ice is less dense than liquid water!
Tro's "Introductory Chemistry", Chapter 2

78. Platinum has become a popular metal for fine jewelry and costs more than gold. A man gives a woman an engagement ring and tells her that it is made of platinum. Noting that the ring felt a little light, the woman decides to perform a test to determine the ring’s density before giving him an answer about marriage. She places the ring on a balance and finds it has a mass of 5.84 grams. She then finds that the ring displaces cm3 of water. Is the ring made of platinum? (Density Pt = 21.4 g/cm3)

79. Tro's "Introductory Chemistry", Chapter 2
Data: She places the ring on a balance and finds it has a mass of 5.84 grams. She then finds that the ring displaces cm3 of water. Is the ring made of platinum? (Density Pt = 21.4 g/cm3)
Given: Mass = 5.84 grams
Volume = cm3
Find: Density in grams/cm3
Equation:
Solution Map:
m and V  d
m, V d
Tro's "Introductory Chemistry", Chapter 2

80. Tro's "Introductory Chemistry", Chapter 2
Apply the Solution Map:
Since 10.5 g/cm3  21.4 g/cm3, the ring cannot be platinum.
Tro's "Introductory Chemistry", Chapter 2

81. Tro's "Introductory Chemistry", Chapter 2
Practice—What Is the Density of Metal if a g Sample Added to a Cylinder of Water Causes the Water Level to Rise from 25.0 mL to 37.8 mL?
Tro's "Introductory Chemistry", Chapter 2

82. Find Density of Metal if 100.0 g Displaces Water from 25.0 to 37.8 mL
Write down the Given quantity and its unit.
Given:
m =100.0 g
displaces 25.0 to 37.8 mL
3 sig figs
Write down the quantity you want to Find and unit.
Find:
d, g/cm3
CF & Equation:
Write down the appropriate Conv. Factor and Equation.
1 mL = 1 cm3
Write a Solution Map.
Solution
Map:
m, V d
Follow the solution map to Solve the problem.
Solution:
V = = 12.8 mL
Significant figures and round.
Round:
g/cm3 = 7.81 g/cm3
3 significant figures
Check.
Check:
Units and magnitude are correct.

83. Density as a Conversion Factor
Can use density as a conversion factor between mass and volume!
Density of H2O = 1 g/mL \ 1 g H2O = 1 mL H2O
Density of Pb = 11.3 g/cm3 \ 11.3 g Pb = 1 cm3 Pb
How much does 4.0 cm3 of lead weigh? =
4.0 cm3 Pb
11.3 g Pb
1 cm3 Pb
45 g Pb x
Tro's "Introductory Chemistry", Chapter 2

84. Measurement and Problem Solving: Density as a Conversion Factor
The gasoline in an automobile gas tank has a mass of 60.0 kg and a density of g/cm3. What is the volume?
Given: kg
Find: Volume in cm3
Conversion factors:
0.752 g/cm3
1000 grams = 1 kg
Solution Map: kg g
cm3
Tro's "Introductory Chemistry", Chapter 2

85. Tro's "Introductory Chemistry", Chapter 2
Measurement and Problem Solving: Density as a Conversion Factor, Continued
Solution Map: kg g
cm3
Tro's "Introductory Chemistry", Chapter 2