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Introductory Chemistry , 3 rd Edition Nivaldo Tro. Chapter 2 Measurement and Problem Solving. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA. 2009, Prentice Hall. What Is a Measurement?. Quantitative observation. Comparison to an agreed upon standard. - PowerPoint PPT Presentation
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Roy KennedyMassachusetts Bay Community College
Wellesley Hills, MA
Introductory Chemistry, 3rd EditionNivaldo Tro
Chapter 2Measurement andProblem Solving
2009, Prentice Hall
Tro's "Introductory Chemistry", Chapter 2
2
What Is a Measurement?
• Quantitative observation.
• Comparison to an agreed upon standard.
• Every measurement has a number and a unit.
Tro's "Introductory Chemistry", Chapter 2
3
A Measurement
• The unit tells you to what standard you are comparing your object.
• The number tells you:1.What multiple of the standard the object
measures.
2. The uncertainty in the measurement.
Tro's "Introductory Chemistry", Chapter 2
4
Scientists have measured the average global temperature rise over the past
century to be 0.6 °C
• °C tells you that the temperature is being compared to the Celsius temperature scale.
• 0.6 tells you that:1. The average temperature rise is 0.6
times the standard unit of 1 degree Celsius.
2. The confidence in the measurement is such that we are certain the measurement is between 0.5 and 0.7 °C.
Tro's Introductory Chemistry, Chapter 2
5
Scientific Notation
A way of writing
large and small numbers.
Tro's "Introductory Chemistry", Chapter 2
6
Big and Small Numbers
• 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!
The sun’sdiameter is
1,392,000,000 m.
An atom’s average diameter is0.000 000 000 3 m.
Tro's "Introductory Chemistry", Chapter 2
9
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
Exponent1.23 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
11
123401. Locate the decimal point.
12340.2. Move the decimal point to obtain a number between 1 and 10.
1.2343. 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 − .
1.234 x 104
Writing a Number in Scientific Notation, Continued
Tro's "Introductory Chemistry", Chapter 2
12
Writing a Number in Scientific Notation, Continued0.00012340
1. Locate the decimal point.0.00012340
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.1.2340 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 − .
1.2340 x 10-4
Tro's "Introductory Chemistry", Chapter 2
13
Writing a Number in Standard Form1.234 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.
000 001.2340.000 001 234
Tro's "Introductory Chemistry", Chapter 2
15
Practice—Write the Following in Scientific Notation, Continued
123.4 = 1.234 x 102
145000 = 1.45 x 105
25.25 = 2.525 x 101
1.45 = 1.45 x 100
8.0012 = 8.0012 x 100
0.00234 = 2.34 x 10-3
0.0123 = 1.23 x 10-2
0.000 008706 = 8.706 x 10-6
Tro's "Introductory Chemistry", Chapter 2
16
Practice—Write the Following in Standard Form, Continued
2.1 x 103 = 2100
9.66 x 10-4 = 0.000966
6.04 x 10-2 = 0.0604
4.02 x 100 = 4.02
3.3 x 101 = 33
1.2 x 100 = 1.2
Tro's "Introductory Chemistry", Chapter 2
19
Numbers
1. Exact2. Measured: Significant Figures
Tro's "Introductory Chemistry", Chapter 2
20
Exact Numbers vs. Measurements• Exact: Sometimes you can determine an exact
value for a quality of an object.A. Often by counting.
• Pennies in a pile.
B. 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.
Name the 4 measuring instruments
1. Length
2. Mass
3. Time
4. Temperature
Tro's "Introductory Chemistry", Chapter 2
21
Tro's "Introductory Chemistry", Chapter 2
22
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
CertainEstimated
45.872
Reading a Measuring Instrument/Device
For any Digital Device record ALL the digits
24
Reading a Measuring Instrument/Device
1. Record all the numbers you can see
2. Make ONE Guess!
25
Tro's "Introductory Chemistry", Chapter 2
26
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
27
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
28
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
What is the length of the wooden stick?1) 4.5 cm 2) 4.54 cm 3) 4.547 cm
30
8.00 cm or 3 (2.2/8)?
Tro's "Introductory Chemistry", Chapter 2
32
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
33
Counting Significant Figures, Continued
• Leading zeros are NOT significant. 0.001050 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
34
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.• 20@ $.05 = $1.0000000000000• 12 inches = 1.000000000000000000000000 ft
Tro's "Introductory Chemistry", Chapter 2
35
Example 2.4—Determining the Number of Significant Figures in a Number, Continued
• How many significant figures are in each of the following numbers?
0.0035 2 significant figures—leading zeros are not significant.
1.080 4 significant figures—trailing and interior zeros are significant.
2371 4 significant figures—All digits are significant.
2.97 × 105 3 significant figures—Only decimal parts count as significant.
1 dozen = 12 Unlimited significant figures—Definition
100,000 1, no decimal
Tro's "Introductory Chemistry", Chapter 2
36
Determine the Number of Significant Figures,
• 12000
• 120.
• 12.00
• 1.20 x 103
• 0.0012
• 0.00120
• 1201
• 1201000
2
3
4
3
2
3
4
4
How many sig figs?
45.8736
.000239
.00023900
48000.
48000
3.982106
1.00040
6
3
5
5
2
4
6
•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
•All digits count
•0’s between digits count as well as trailing in decimal form
Tro's "Introductory Chemistry", Chapter 2
38
Rounding• When rounding to the correct number of significant
figures, if the number after the place of the last significant figure is:
1. 0 to 4, round down. Drop all digits after the last significant figure and leave
the last significant figure alone. Add insignificant zeros to keep the value, if necessary.
2. 5 to 9, round up. Drop all digits after the last significat figure and
increase the last significant figure by one. Add insignificant zeros to keep the value, if necessary.
Examples of RoundingFor example you want a 4 Sig Fig number
4965.03
780,582
1999.5
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
4965
780,600
2000.
Tro's "Introductory Chemistry", Chapter 2
43
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.
5.02 × 89,665 × 0.10 = 45.0118 = 45 3 sig. figs. 5 sig. figs. 2 sig. figs. 2 sig.
figs.
5.892 ÷ 6.10 = 0.96590 = 0.966 4 sig. figs. 3 sig. figs. 3 sig. figs.
Tro's "Introductory Chemistry", Chapter 2
44
Determine the Correct Number of Significant Figures for Each Calculation and
1. 1.01 × 0.12 × 53.51 ÷ 96 = 0.067556 = 0.068
2. 56.55 × 0.920 ÷ 34.2585 = 1.51863 = 1.52
3 sf 2 sf 4 sf 2 sf Result should have 2 sf.
7 is in place of last sig. fig., number after
is 5 or greater, so round up.
4 sf 3 sf 6 sf Result should have 3 sf.
1 is in place of last sig. fig., number after
is 5 or greater, so round up.
Addition/Subtraction
25.5 32.72 320
+34.270 ‑ 0.0049 + 12.5
59.770 32.7151 332.5
59.8 32.72 330
Tro's "Introductory Chemistry", Chapter 2
46
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.
5.74 + 0.823 +2.651 = 9.214 = 9.21 2 dec. pl. 3 dec. pl. 3 dec. pl. 2 dec. pl.
4.8 - 3.965 = 0.835 = 0.8 1 dec. pl 3 dec. pl. 1 dec. pl.
Tro's "Introductory Chemistry", Chapter 2
47
Determine the Correct Number of Significant Figures for Each Calculation and
Round and Report the Result, Continued
1. 0.987 + 125.1 – 1.22 = 124.867 = 124.9
2. 0.764 – 3.449 – 5.98 = -8.664 = -8.66
3 dp 1 dp 2 dp Result should have 1 dp.
8 is in place of last sig. fig., number after
is 5 or greater, so round up.
3 dp 3 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.
__ ___ __
Addition and Subtraction
.56 + .153 = .713
82000 + 5.32 = 82005.32
10.0 - 9.8742 = .12580
10 – 9.8742 = .12580
.71
82000
.1
0
Look for the last important digit
Tro's "Introductory Chemistry", Chapter 2
49
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.
3.489 × (5.67 – 2.3) = 2 dp 1 dp
3.489 × 3.37 = 12 4 sf 1 dp & 2 sf 2 sf
- n
Tro's "Introductory Chemistry", Chapter 2
50
Example 1.6—Perform the Following Calculations to the Correct Number of Significant Figures,
Continued652.065219.04555.30015.45120.010.1 a)
4.9 8730.4
5820.100
1.105
355.0
5379904.5233.4526755.45299870.3562.4 c)
1.0142.002.855.084.14 d)
b)
Tro's "Introductory Chemistry", Chapter 2
51
Basic Units of Measure
Tro's "Introductory Chemistry", Chapter 2
52
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
53
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
Volume liter L
Time second s
Temperature kelvin K
Tro's "Introductory Chemistry", Chapter 2
61
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
62
Common Prefixes in the SI System
Prefix SymbolDecimal
EquivalentPower 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- or mc 0.000 001 Base x 10-6
nano- n 0.000 000 001 Base x 10-9
Measurements and SI
Tro's "Introductory Chemistry", Chapter 2
63
M 1,000,000
k 1,000
d 0.1
c 0.01
m 0.001
or mc 0.000 001
n 0.000 000 001
gram g
meter m
liter L
seconds s
Kelvin K
Measurements and SI
Tro's "Introductory Chemistry", Chapter 2
64
m 0.001
liter L
(m = .001)L
mL = .001L or 1000 mL = L
Tro's "Introductory Chemistry", Chapter 2
65
Prefixes Used to Modify Standard Unit• kilo = 1000 times base unit = 103
1 kg = 1000 g = 103 g
• deci = 0.1 times the base unit = 10-1
1 dL = 0.1 L = 10-1 L; 1 L = 10 dL
• centi = 0.01 times the base unit = 10-2
1 cm = 0.01 m = 10-2 m; 1 m = 100 cm
• milli = 0.001 times the base unit = 10-3
1 mg = 0.001 g = 10-3 g; 1 g = 1000 mg
• micro = 10-6 times the base unit1 m = 10-6 m; 106 m = 1 m
• nano = 10-9 times the base unit1 nL = 10-9L; 109 nL = 1 L
Volume
1 mL = 1 cm3
Tro's "Introductory Chemistry", Chapter 2
67
Common Units and Their Equivalents
Length
1 kilometer (km) = 0.6214 mile (mi)
1 meter (m) = 39.37 inches (in.)
1 meter (m) = 1.094 yards (yd)
1 foot (ft) = 30.48 centimeters (cm)
1 inch (in.) = 2.54 centimeters (cm) exactly
Tro's "Introductory Chemistry", Chapter 2
71
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
72
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 :
unit desired unit related
unit desired
unitstart
unit relatedunitstart
unit desired unitstart
unit desiredunitstart
Tro's "Introductory Chemistry", Chapter 2
73
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
in1
cm54.2cm54.2
in1
Tro's "Introductory Chemistry", Chapter 2
75
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
76
Systematic Approach, Continued4. Design a solution map for the problem.
Order conversions to cancel previous units orarrange 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
77
Solution Maps and Conversion Factors
• Convert inches into centimeters.1. Find relationship equivalence: 1 in = 2.54 cm
2. Write solution map.
inin cmcm
3. Change equivalence into conversion factors with starting units on the bottom.
in 1
cm 2.54
Tro's "Introductory Chemistry", Chapter 2
78
Example 2.8:• Convert 7.8 km to miles
Tro's "Introductory Chemistry", Chapter 2
79
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
80
• Write down the quantity to find and/or its units.
Find: ? miles
Information
Given: 7.8 kmExample:Convert 7.8 km to miles.
Tro's "Introductory Chemistry", Chapter 2
81
• Collect needed conversion factors:
1 mi = 0.6214 km
Information
Given: 7.8 km
Find: ? mi
Example:Convert 7.8 km to miles.
Tro's "Introductory Chemistry", Chapter 2
82
• Write a solution map for converting the units:
InformationGiven: 7.8 kmFind: ? miConversion Factor:
1 mi = 0.6214 km
Example:Convert 7.8 km to miles.
km mi
km 1
mi .62140
Tro's "Introductory Chemistry", Chapter 2
83
• Apply the solution map:
InformationGiven: 7.8 kmFind: ? miConversion Factor:1 mi = 0.6214 kmSolution Map: km mi
Example:Convert 7.8 km to miles.
km 1
mi .62140
mi km 1
mi 0.6214km 7.8
= 4.84692 mi
= 4.8 mi
• Significant figures and round:
2 significant figures
2 significant figures
Tro's "Introductory Chemistry", Chapter 2
84
• Check the solution:
InformationGiven: 7.8 kmFind: ? miConversion Factor: 1 mi = 0.6214 kmSolution Map: km mi
Example:Convert 7.8 km to miles.
km 1
mi .62140
7.8 km = 4.8 mi
The units of the answer, mi, are correct.The magnitude of the answer makes sense
since kilometers are shorter than miles.
Tro's "Introductory Chemistry", Chapter 2
86
Practice—Convert 30.0 g to Ounces(1 oz. = 28.32 g)
Convert 30.0 g to Ounces
Units and magnitude are correct.
Check:• Check.
Round:• Significant figures and round.
Solution:• Follow the solution map to Solve the problem.
Solution Map:
• Write a Solution Map.
1 oz = 28.35 gConversion Factor:
• Write down the appropriate Conversion Factors.
oz.Find:• Write down the quantity you want to Find and unit.
30.0 gGiven:• Write down the Given quantity and its unit.
g oz
g 28.35
oz 1
oz 1.05820 g 28.35
oz 1g 30.0
3 sig figs
3 sig figs= 1.06 oz
Tro's "Introductory Chemistry", Chapter 2
89
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
90
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
91
• Write down the quantity to find and/or its units.
Find: ? cups
Information
Given: 0.75 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?
Tro's "Introductory Chemistry", Chapter 2
92
• Collect needed conversion factors:
4 cu = 1 qt
1.057 qt = 1 L
Information
Given: 0.75 L
Find: ? cu
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
93
• Write a solution map for converting the units:
InformationGiven: 0.75 LFind: ? cuConversion Factors:
4 cu = 1 qt; 1.057 qt = 1 L
L qt
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?
cu
L 1
qt .0571qt 1
cu 4
Tro's "Introductory Chemistry", Chapter 2
94
qt 1
cu 4
L 1
qt .0571L 750 .
• Apply the solution map:
= 3.171 cu
= 3.2 cu
• Significant figures and round:
InformationGiven: 0.75 LFind: ? cuConversion Factors: 4 cu = 1 qt; 1.057 qt = 1 LSolution Map: L qt cu
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?
L 1
qt .0571
qt 1
cu 4
2 significant figures
2 significant figures
Tro's "Introductory Chemistry", Chapter 2
95
• Check the solution:
0.75 L = 3.2 cu
The units of the answer, cu, are correct.The magnitude of the answer makes sense
since cups are smaller than liters.
InformationGiven: 0.75 LFind: ? cuConversion Factors:4 cu = 1 qt; 1.057 qt = 1 LSolution Map: L qt cu
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?
L 1
qt .0571
qt 1
cu 4
Tro's "Introductory Chemistry", Chapter 2
100
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
101
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
102
• Write down the quantity to find and/or its units.
Find: ? m2
Information
Given: 2,659 cm2
Example:A circle has an area of 2,659 cm2. What is the area in square meters?
Tro's "Introductory Chemistry", Chapter 2
103
• Collect needed conversion factors:
1 cm = 0.01m
Information
Given: 2,659 cm2
Find: ? m2
Example:A circle has an area of 2,659 cm2. What is the area in square meters?
Tro's "Introductory Chemistry", Chapter 2
104
• Write a solution map for converting the units:
cm2 m2
2
cm 1
m .010
InformationGiven: 2,659 cm2
Find: ? m2
Conversion Factor:1 cm = 0.01 m
Example:A circle has an area of 2,659 cm2. What is the area in square meters?
Tro's "Introductory Chemistry", Chapter 2
105
• Apply the solution map:2
2
2-42 m
cm 1
m 101cm 2,659
= 0.265900 m2
= 0.2659 m2
• Significant figures and round:
InformationGiven: 2,659 cm2
Find: ? m2
Conversion Factor:1 cm = 0.01 mSolution Map: cm2 m2
Example:A circle has an area of 2,659 cm2. What is the area in square meters? 2
cm 1
m .010
4 significant figures
4 significant figures
Tro's "Introductory Chemistry", Chapter 2
108
Practice—Convert 30.0 cm3 to ft3
(1 cm = 1 x 10-2 m) (in class)
Convert 30.0 cm3 to m3
Units and magnitude are correct.
Check:7. Check.
30.0 cm3 = 3.00 x 10−5 m3Round:6. Significant figures and round.
Solution:5. Follow the solution map to Solve the problem.
Solution Map:
4. Write a Solution Map.
(1 cm = 0.01 m)3Conversion Factor:
3. Write down the appropriate Conversion Factors.
? m3Find:2. Write down the quantity you want to Find and unit.
30.0 cm3Given:1. Write down the Given quantity and its unit.
cm3 m3
3
cm 1
m .010
35-3
3631 m 103
cm 1
m 101cm 103.00
3 sig figs
3 sig figs
Tro's "Introductory Chemistry", Chapter 2
110
Density
Tro's "Introductory Chemistry", Chapter 2
114
Density• Ratio of mass:volume.• Its value depends on the kind of material, not the
amount.• 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!
Volume
MassDensity
Tro's "Introductory Chemistry", Chapter 2
117
Platinum has become a popular metal for fine jewelry. 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 0.556 cm3 of water. Is the ring made of platinum? (Density Pt = 21.4 g/cm3)
Tro's "Introductory Chemistry", Chapter 2
118
She places the ring on a balance and finds it has a mass of 5.84 grams. She then finds that the ring displaces 0.556 cm3 of water. Is the ring made of
platinum? (Density Pt = 21.4 g/cm3)
Given: Mass = 5.84 grams
Volume = 0.556 cm3
Find: Density in grams/cm3
Equation:
Solution Map:
m and V d
dV
m
m, V dd
V
m
Tro's "Introductory Chemistry", Chapter 2
119
She places the ring on a balance and finds it has a mass of 5.84 grams. She then finds that the ring displaces 0.556 cm3 of water. Is the ring made of
platinum? (Density Pt = 21.4 g/cm3)
Apply the Solution Map:
33 cmg 10.5
cm 0.556
g 5.84
dV
m
Since 10.5 g/cm3 21.4 g/cm3, the ring cannot be platinum.
m, V dd
V
m
Tro's "Introductory Chemistry", Chapter 2
120
Practice—What Is the Density of Metal if a 100.0 g Sample Added to a Cylinder of Water Causes the Water Level to Rise from 25.0 mL to 37.8 mL?
Find Density of Metal if 100.0 g Displaces Water from 25.0 to 37.8 mL
Units and magnitude are correct.
Check:7. Check.
7.8125 g/cm3 = 7.81 g/cm3Round:6. Significant figures and round.
Solution:
V = 37.8-25.0 = 12.8 mL
5. Follow the solution map to Solve the problem.
Solution Map:
4. Write a Solution Map.
CF & Equation:
d, g/cm3Find:2. Write down the quantity you want to Find and unit.
m =100.0 gdisplaces 25.0 to 37.8 mL
Given:1. Write down the Given quantity and its unit.
3 sig figs
3 significant figures
m, V d
V
m d
V
m d 1 mL = 1 cm3
33
g/cm 2518.7cm 12.8
g 0.100d
33
cm .821mL 1
cm 1mL 12.8
3. Write down the appropriate Conv. Factor and Equation.
Tro's "Introductory Chemistry", Chapter 2
122
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 Pbx
Tro's "Introductory Chemistry", Chapter 2
123
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 0.752 g/cm3. What is the volume?
• Given: 60.0 kg
• Find: Volume in cm3
• Conversion factors: 0.752 g/cm3
1000 grams = 1 kg
Solution Map:
kg g cm3
kg 1
g 1000
g .7520
cm 1 3
Tro's "Introductory Chemistry", Chapter 2
124
Measurement and Problem Solving:Density as a Conversion Factor,
Continued
343
cm107.98 g 0.752
cm 1
kg 1
g 1000kg 60.0
Solution Map:
kg g cm3
kg 1
g 1000
g .7520
cm 1 3
Tro's "Introductory Chemistry", Chapter 2
125
Practice—What Volume Does 100.0 g of Marble Occupy? (d = 4.00 g/cm3)
What Volume Does 100.0 g of Marble Occupy?
Units and magnitude are correct.
Check:7. Check.
25 cm3 = 25.0 cm3Round:6. Significant figures and round.
Solution:5. Follow the solution map to Solve the problem.
Solution Map:
4. Write a Solution Map.
CF & Equation:
3. Write down the appropriate Conv. Factor and Equation.
V, cm3Find:2. Write down the quantity you want to Find and unit.
m =100.0 gGiven:1. Write down the Given quantity and its unit.
4 sig figs
3 significant figures
m V
g 4.00
cm 1 3
33
cm 25g 4.00
cm 1g 100.0
4.00 g = 1 cm33 sig figs
Tro's "Introductory Chemistry", Chapter 2
128
Example 2.17:• A 55.9 kg person displaces 57.2 L of water when
submerged in a water tank. What is the density of the person in g/cm3?