chapter two measurements in chemistry fundamentals of general, organic & biological chemistry
TRANSCRIPT
Chapter Two
Measurements inChemistry
Fundamentals of General, Organic & Biological Chemistry
2
Stating a Measurement
In every measurement, a number is followed by a unit.
Observe the following examples of measurements:
number + unit35 m
0.25 L 225 lb 3.4 hr
3
The Metric System (SI)
The metric system is A decimal system
based on 10. Used in most of the
world. Used by scientists
and in hospitals.
4
Units in the Metric SystemIn the metric and SI systems, a basic unit identifies each type of measurement:
5
Length Measurement
In the metric system, length is measured in meters using a meter stick.
The metric unit for length is the meter (m).
6
Volume Measurement
Volume is the space occupied by a substance.
The metric unit of volume is the liter (L).
The liter is slightly bigger than a quart.
A graduated cylinder is used to measure the volume of a liquid.
7
Mass Measurement
The mass of an object is the quantity of material it contains.
A balance is used to measure mass.
The metric unit for mass is the gram (g).
8
In each of the following, indicate whether the unit describes 1) length 2) mass or 3) volume. ____ A. A bag of tomatoes is 4.6 kg.
____ B. A person is 2.0 m tall.
____ C. A medication contains 0.50 g Aspirin.
____ D. A bottle contains 1.5 L of water.
Learning Check
9
In each of the following, indicate whether the unit describes 1) length 2) mass or 3) volume.
2 mass A. A bag of tomatoes is 4.6 kg.
1 length B. A person is 2.0 m tall.
2 mass C. A medication contains 0.50 g
Aspirin.
3 volume D. A bottle contains 1.5 L of water.
Solution
10
Learning Check
Identify the measurement that has a metric unit. A. John’s height is
1) 1.5 yards 2) 6 feet 3) 2 meters
B. The volume of saline in the IV container is1) 1 liter 2) 1 quart 3) 2 pints
C. The mass of a lemon is1) 12 ounces 2) 145 grams 3) 0.6 pounds
11
Solution
A. John’s height is
3) 2 meters
B. The volume of saline in the IV container is
1) 1 liter
C. The mass of a lemon is
2) 145 grams
12
Scientific Notation
A number in scientific notation contains a coefficient and a power of 10.
coefficient power of ten coefficient power of ten
1.5 x 102 7.35 x 10-4
Place the decimal point after the first digit. Indicate the spaces moved as a power of ten.
52 000 = 5.2 x 104 0.00378 = 3.78 x 10-3
4 spaces left 3 spaces right
13
Learning Check
Select the correct scientific notation for each.
A. 0.000 008
1) 8 x 106 2) 8 x 10-6 3) 0.8 x 10-5
B. 72 000
1) 7.2 x 104 2) 72 x 103 3) 7.2 x 10-4
14
Solution
Select the correct scientific notation for each.
A. 0.000 008
2) 8 x 10-6
B. 72 000
1) 7.2 x 104
15
Learning Check
Write each as a standard number.
A. 2.0 x 10-2
1) 200 2) 0.02 3) 0.020
B. 1.8 x 105
1) 180 0002) 0.000018 3) 18 000
16
Solution
Write each as a standard number.
A. 2.0 x 10-2
3) 0.020
B. 1.8 x 105
1) 180 000
17
Measured Numbers
You use a measuring tool to determine a quantity such as your height or the mass of an object.
The numbers you obtain are called measured numbers.
18
. l2. . . . l . . . . l3 . . . . l . . . . l4. . cm
To measure the length of the blue line, we read the markings on the meter stick.
The first digit 2 plus the second digit 2.7
Estimating the third digit between 2.7–2.8gives a final length reported as
2.75 cm
or 2.76 cm
Reading a Meter Stick
Chapter 01 Slide 19
Accuracy – how close a measurement is to the true value
Precision – how close a set of measurements are to each other
accurate&
precise
precisebut
not accurate
not accurate&
not precise
20
good accuracygood precision
Mass of a Tennis Ball
21
good accuracypoor precision
Mass of a Tennis Ball
22
poor accuracypoor precision
Mass of a Tennis Ball
23
Known + Estimated Digits
In the length measurement of 2.76 cm,
the digits 2 and 7 are certain (known).
the third digit 5(or 6) is estimated (uncertain). all three digits (2.76) are significant including
the estimated digit.
24
Learning Check
. l8. . . . l . . . . l9. . . . l . . . . l10. . cm
What is the length of the red line?
1) 9.0 cm
2) 9.03 cm
3) 9.04 cm
25
Solution
. l8. . . . l . . . . l9. . . . l . . . . l10. . cm
The length of the red line could be reported as
2) 9.03 cm
or 3) 9.04 cm
The estimated digit may be slightly different.
Both readings are acceptable.
26
. l3. . . . l . . . . l4. . . . l . . . . l5. . cm
The first and second digits are 4.5. In this example, the line ends on a mark. Then the estimated digit for the hundredths
place is 0. We would report this measurement as 4.50 cm.
Zero as a Measured Number
27
Exact Numbers
An exact number is obtained when you count objects or use a defined relationship.Counting objects
2 soccer balls4 pizzas
Defined relationships1 foot = 12 inches1 meter = 100 cm
An exact number is not obtained with a measuring tool.
28
Learning Check
A. Exact numbers are obtained by 1. using a measuring tool
2. counting3. definition
B. Measured numbers are obtained by 1. using a measuring tool
2. counting3. definition
29
Solution
A. Exact numbers are obtained by
2. counting
3. definition
B. Measured numbers are obtained by
1. using a measuring tool
30
Learning Check
Classify each of the following as an exact (1) or a
measured (2) number.
A.__Gold melts at 1064°C.
B.__1 yard = 3 feet
C.__The diameter of a red blood cell is 6 x 10-4 cm.
D.__There are 6 hats on the shelf.
E.__A can of soda contains 355 mL of soda.
31
Classify each of the following as an exact (1) or a
measured(2) number.
A. 2 A measuring tool is required.
B. 1 This is a defined relationship.
C. 2 A measuring tool is used to determine
length.
D. 1 The number of hats is obtained by counting.
E. 2 The volume of soda is measured.
Solution
32
2.4 Measurement and Significant FiguresEvery experimental measurement, no matter how precise, has a degree of uncertainty to it because there is a limit to the number of digits that can be determined.
Chapter 01
Slide 33
Accuracy, Precision, and Significant Figures
length = 1.74 cm
0 1 2 43cm
1.7 cm < length < 1.8 cm
34
Rules for determining significant figures
1. Zeroes in the middle of a number are significant. 69.08 g has four significant figures, 6, 9, 0, and 8.
2. Zeroes at the beginning of a number are not significant. 0.0089 g has two significant figure, 8 and 9.
3. Zeroes at the end of a number and after the decimal points are significant. 2.50 g has three significant figures 2, 5, and 0.
25.00 m has four significant figures 2, 5, 0, and 0.
35
4. Zeroes at the end of a number and before an implied decimal points may or may not be significant. 1500 kg may have two, three, or four significant figures. Zeroes here may be part of the measurements or for simply to locate the unwritten decimal point.
36
Which of the following measurements has three significant figures?
a. 1,207 g
b. 4.250 g
c. 0.006 g
d. 0.0250 g
e. 0.03750 g
37
Which of the following measurements has three significant figures?
a. 1,207 g
b. 4.250 g
c. 0.006 g
d. 0.0250 g
e. 0.03750 g
38
Which of the following numbers contains four significant figures?
a. 230,110
b. 23,011.0
c. 0.23010
d. 0.0230100
e. 0.002301
39
Which of the following numbers contains four significant figures?
a. 230,110
b. 23,011.0
c. 0.23010
d. 0.0230100
e. 0.002301
40
2.6 Rounding off Numbers
Often calculator produces large number as a result of a calculation although the number of significant figures is good only to a fewer number than the calculator has produced – in this case the large number may be rounded off to a smaller number keeping only significant figures.
41
Rules for Rounding off Numbers: Rule 1 (For multiplication and divisions): The answer can’t have more significant figures than either of the original numbers.
42
Rule 2 (For addition and subtraction): The answer should have minimum decimal places.
43
How many significant figures should be shown for the calculation?
1 2 3 4 5
1.25 0.45
2.734
44
How many significant figures should be shown for the calculation?
1 2 3 4 5
1.25 0.45
2.734
45
How many significant figures are there in the following number: 1.200 X 109?
1. 4
2. 3
3. 2
4. 1
5. Cannot deduce from given information.
46
Correct Answer:
Zeros that fall both at the end of a number and after the decimal point are always significant.
1.200 109
1. 4
2. 3
3. 2
4. 1
5. Cannot deduce from given information.
47
6.220 1.0
+ 125
How many significant figures are there in the following summation:
1. 22. 33. 44. 55. 6
48
6.220 1.0
+ 125 132.220
Correct Answer:
In addition and subtraction the result can have no more decimal places than the measurement with the fewest number of decimal places.
1. 22. 33. 44. 55. 6
49
How many significant figures are there in the result of the following multiplication:
(2.54) (6.2) (12.000)
1. 22. 33. 44. 5
50
Correct Answer:
In multiplication and division the result must be reported with the same number of significant figures as the measurement with the fewest significant figures.
(2.54) (6.2) (12.000) = 188.976 = 190
1. 22. 33. 44. 5
51
2.7 Problem Solving: Converting a Quantity from One Unit to Another
Factor-Label-Method (Unit Conversion Factor): A quantity in one unit is converted to an equivalent quantity in a different unit by using a conversion factor that expresses the relationship between units.
52
53
When solving a problem, set up an equation so that all unwanted units cancel, leaving only the desired unit. For example, we want to find out how many kilometers are there in 26.22 mile distance. We will get the correct answer if we multiply 26.22 mi by the conversion factor km/mi.
54
In working a problem, start with the initial unit.
Write a unit plan that converts the initial unit to the final unit.
Unit 1 Unit 2 Select conversion factors that cancel the
initial unit and give the final unit.Initial x Conversion = Final
unit factor unitUnit 1 x Unit 2 = Unit 2
Unit 1
Problem Setup
55
Setting up a Problem
How many minutes are 2.5 hours?Solution: Initial unit = 2.5 hrFinal unit = ? minUnit Plan = hr min
Setup problem to cancel hours (hr). Inital Conversion Final
unit factor unit2.5 hr x 60 min = 150 min (2 SF)
1 hr
56
A rattlesnake is 2.44 m long. How long is the snake in cm?
1) 2440 cm
2) 244 cm
3) 24.4 cm
Learning Check
57
A rattlesnake is 2.44 m long. How long is the snake in centimeters?
2) 244 cm
2.44 m x 100 cm = 244 cm
1 m
Solution
58
Often, two or more conversion factors are required to obtain the unit of the answer.
Unit 1 Unit 2 Unit 3 Additional conversion factors are placed in
the setup to cancel the preceding unitInitial unit x factor 1 x factor 2 = Final unit
Unit 1 x Unit 2 x Unit 3 = Unit 3 Unit 1 Unit 2
Using Two or More Factors
59
How many minutes are in 1.4 days?Initial unit: 1.4 days
Unit plan: days hr min
Set up problem: 1.4 days x 24 hr x 60 min = 2.0 x 103 min
1 day 1 hr 2 SF Exact Exact = 2 SF
Example: Problem Solving
60
Be sure to check your unit cancellation in the setup.
What is wrong with the following setup?1.4 day x 1 day x 1 hr 24 hr 60 min Units = day2/min is Not the final unit needed Units don’t cancel properly.
The units in the conversion factors must cancel to give the correct unit for the answer.
Check the Unit Cancellation
61
An adult human has 4650 mL of blood. How many gallons of blood is that?
Unit plan: mL qt gallon
Equalities: 1 quart = 946 mL
1 gallon = 4 quarts
Learning Check
62
Unit plan: mL qt gallon
Setup:
4650 mL x 1 qt x 1 gal = 1.23 gal
946 mL 4 qt
3 SF exact exact 3 SF
Solution
63
Identify the initial and final units. Write out a unit plan. Select appropriate conversion factors. Convert the initial unit to the final unit. Cancel the units and check the final unit. Do the math on a calculator. Give an answer using significant figures.
Typical Steps in Problem Solving
64
If a ski pole is 3.0 feet in length, how long is the ski pole in mm?
Learning Check
65
3.0 ft x 12 in x 2.54 cm x 10 mm =
1 ft 1 in. 1 cm
Check factor setup: Units cancel properly
Check final unit: mm
Calculator answer: 914.4 mm
Final answer: 910 mm (2 SF rounded)
Solution
66
If your pace on a treadmill is 65 meters per minute, how many minutes will it take for you to walk a distance of 7500 feet?
Learning Check
67
7500 ft x 12 in. x 2.54 cm x 1 m
1 ft 1 in. 100 cm
x 1 min = 35 min 65 m final answer (2 SF)
Solution
68
Clinical Factors
Conversion factors are also possible when working with medications.
A drug dosage such as 20 mg Prednisone per tablet can be written as
20 mg Prednisone and 1 tablet
1 tablet 20 mg Prednisone
69
Learning Check
The dosage ordered is 400 mg of Erythromycin four times a day (q.i.d)*. If the oral suspension contains 200 mg Erythromycin/5 mL, how many mL will be given each time?
1) 5 mL
2) 10 mL
3) 40 mL
*:Latin quater in die
70
Solution
The dosage ordered is 400 mg of Erythromycin four times a day (q.i.d). If the oral suspension contains 200 mg Erythromycin/5 mL, how many mL will be given each time?
2) 10 mL
400 mg x 5 mL = 10 mL
200 mg
71
Temperature Scales
Temperature is measured using the Fahrenheit, Celsius, and Kelvin temperature scales.
The reference points are the boiling and freezing points of water.
72
A. What is the temperature of freezing water?
1) 0°F 2) 0°C 3) 0 K
B. What is the temperature of boiling water?
1) 100°F 2) 32°F 3) 373 K
C. How many Celsius units are between the boiling and freezing points of water?
1) 100 2) 180 3) 273
Learning Check
73
A. What is the temperature of freezing water?
2) 0°C
B. What is the temperature of boiling water?
3) 373 K
C. How many Celsius units are between the
boiling and freezing points of water?
1) 100
Solution
74
On the Fahrenheit scale, there are are 180°F between the freezing and boiling points and on the Celsius scale, there are 100 °C. 180°F = 9°F = 1.8°F 100°C 5°C 1°C
In the formula for Fahrenheit, the value of 32 adjusts the zero point of water from 0°C to 32°F.
°F = 9/5 T°C + 32
or °F = 1.8 T°C + 32
Fahrenheit Formula
75
The equation for Fahrenheit is rearranged to calculate T°C.
°F = 1.8 T°C + 32 Subtract 32 from both sides and divide by 1.8.
°F – 32 = 1.8T°C ( +32 – 32)°F – 32 = 1.8 T°C
1.8 1.8°F – 32 = T°C
1.8
Celsius Formula
76
A person with hypothermia has a body temperature of 34.8°C. What is that temperature in °F? °F = 1.8 (34.8°C) + 32 exact tenth's exact
= 62.6 + 32= 94.6°F
tenth’s
Solving A Temperature Problem
77
The normal temperature of a chickadee is 105.8°F. What is that temperature in °C?
1) 73.8 °C
2) 58.8 °C
3) 41.0 °C
Learning Check
78
3) 41.0 °C
°C = (°F – 32)
1.8
= (105.8 – 32)
1.8
= 73.8°F
1.8° = 41.0°C
Solution
79
A pepperoni pizza is baked at 455°F. What temperature is needed on the Celsius scale?
1) 437 °C
2) 235°C
3) 221°C
Learning Check
80
A pepperoni pizza is baked at 455°F. What temperature is needed on the Celsius scale?
2) 235°C
(455 – 32) = 235°C 1.8
Solution
81
On a cold winter day, the temperature is –15°C.
What is that temperature in °F?
1) 19°F
2) 59°F
3) 5°F
Learning Check
82
3) 5°F
°F = 1.8(–15°C) + 32
= – 27 + 32
= 5°F
Note: Be sure to use the change sign key on your calculator to enter the minus – sign. 1.8 x 15 +/ – = –27
Solution
83
2.10 Energy and HeatEnergy: Capacity to do work or supply energy.Classification of Energy:1. Potential Energy: stored energy. Example: a coiled spring have potential
energy waiting to be released. 2. Kinetic Energy: energy of motion.
Example, when the spring uncoil potential energy is converted to the kinetic energy.
84
Learning Check
Identify the energy as 1) potential or 2) kinetic
A. Roller blading.
B. A peanut butter and jelly sandwich.
C. Mowing the lawn.
D. Gasoline in the gas tank.
85
Solution
Identify the energy as 1) potential or 2) kinetic
A. Roller blading. (2 kinetic)
B. A peanut butter and jelly sandwich. (1 potential)
C. Mowing the lawn. (2 kinetic)
D. Gasoline in the gas tank. (1 potential)
86
Energy has many forms: Mechanical Electrical Thermal (heat) Chemical Solar (light) Nuclear
Forms of Energy
87
Heat energy flows from a warmer object to a colder object.
The colder object gains energy when it is heated.
During heat flow, the loss of heat by a warmer object is equal to the heat gained by the colder object.
Heat
88
Heat is measured in calories or joules.
1 kilocalorie (kcal) = 1000 calories (cal)
1 calorie = 4.18 Joules (J)
1 kJ = 1000 J
Some Equalities for Heat
89
Specific heat is the amount of heat (calories or Joules) that raises the temperature of 1 g of a substance by 1°C.
Specific Heat
90
A. A substance with a large specific heat 1) heats up quickly 2) heats up slowly
B. When ocean water cools, the surrounding air 1) cools 2) warms 3) stays the same
C. Sand in the desert is hot in the day and cool at night. Sand must have a
1) high specific heat 2) low specific heat
Learning Check
91
A. A substance with a large specific heat
2) heats up slowly
B. When ocean water cools, the surrounding air
2) warms
C. Sand in the desert is hot in the day and cool
at night. Sand must have a
2) low specific heat
Solution
92
When 200 g of water are heated, the water temperature rises from 10°C to 18°C.
If 400 g of water at 10°C are heated with the same amount of heat, the final temperature would be1) 10 °C 2) 14°C 3) 18°C
200 g400 g
Learning Check
93
When 200 g of water are heated, the water temperature rises from 10°C to 18°C.
If 400 g of water at 10°C are heated with the same amount of heat, the final temperature would be2) 14°C
200 g400 g
Solution
94
To calculate the amount of heat lost or gained by a substance, we need the Specific Heat of substance, T, and the mass of the substance.
Heat = g x T x cal (or J) = cal ( or J) g °C
Calculation with Specific Heat
95
A hot-water bottle contains 750 g of water at 65°C. If the water cools to body temperature (37°C), how many calories of heat could be transferred to sore muscles?
The temperature change is 65°C - 37°C = 28°C.heat (cal) = g x T x Sp. Ht. (H2O)
750 g x 28°C x 1.00 cal g°C
= 21 000 cal
Sample Calculation for Heat
96
How many kcal are needed to raise the temperature of 120 g of water from 15.0°C to 75.0°C?
1) 1.8 kcal
2) 7.2 kcal
3) 9.0 kcal
Learning Check
97
How many kcal are needed to raise the temperature of 120 g of water from 15.0°C to 75.0°C?
2) 7.2 kcal
Learning Check
98
In chemical reactions, the potential energy is often converted into heat. Reaction products have less potential energy than the reactants – the products are more stable than the reactants.
Stable products have very little potential energy remaining as a result have very little tendency to undergo further reaction.
SI unit of energy is Joules (J) and the metric unit of energy is calorie (cal).
99
2.11 Density
Density relates the mass of an object with its volume. Density is usually expressed in units as - Gram per cubic centimeter (g/cm3) for solids, and Gram per milliliter (g/mL) for liquids.
Density = Mass (g)
Volume (mL or cm3)
100
Osmium is a very dense metal. What is its density in g/cm3 if 50.00 g of the metal occupies a volume of 2.22 cm3?
1) 2.25 g/cm3
2) 22.5 g/cm3
3) 111 g/cm3
Learning Check
101
Place the mass of the osmium metal in the numerator of the density setup and its volume in the denominator.
D = mass = 50.00 g volume 2.22 cm3
calculator = 22.522522 g/cm3
final answer = 22.5 g/cm3
Solution
102
Density Using Volume Displacement
The volume of zinc is calculated from the displaced volume 45.0 mL - 35.5 mL = 9.5 mL = 9.5 cm3
Density zinc = mass = 68.60 g = 7.2 g/cm3
volume 9.5 cm3
103
What is the density (g/cm3) of 48 g of a metal if the metal raises the level of water in a graduated cylinder from 25 mL to 33 mL?
1) 0.2 g/ cm3 2) 6 g/cm3 3) 252 g/cm3
25 mL 33 mL
object
Learning Check
104
2) 6 g/cm3
Calculate the volume difference. 33 mL – 25 mL = 8 mL
Convert the volume in mL to cm3.
8 mL x 1 cm3 = 8 cm3
1 mL
Set up the density calculationDensity = mass = 48 g = 6 g = 6 g/cm3
volume 8 cm3 cm3
Solution
105
Sink or Float
Ice floats in water because the density of ice is less than the density of water. Aluminum sinks because it has a density greater than the density of water.
106
Which diagram correctly represents the liquid layers in the cylinder? Karo (K) syrup (1.4 g/mL), vegetable (V) oil (0.91 g/mL,) water (W) (1.0 g/mL)
1 2 3
K
K
W
W
W
V
V
V
K
Learning Check
107
1) vegetable oil 0.91 g/mL
water 1.0 g/mL
Karo syrup 1.4 g/mLK
W
V
Solution
108
Density represents an equality for a substance. The mass in grams is for 1 mL. For a substance with a density of 3.8 g/mL, the equality is:
3.8 g = 1 mL
For this equality, we can write two conversion factors.
Conversion 3.8 g and 1 mL factors 1 mL 3.8 g
Density as a Conversion Factor
109
The density of octane, a component of gasoline, is 0.702 g/mL. What is the mass, in kg, of 875 mL of octane?
1) 0.614 kg
2) 614 kg
3) 1.25 kg
Learning Check
110
1) 0.614 kg
Unit plan: mL g kg
Equalities: density 1 mL = 0.702 g
and 1 kg = 1000 g
Setup: 875 mL x 0.702 g x 1 kg = 0.614 kg 1 mL 1000 g
density metric factor factor
Solution
111
If blood has a density of 1.05 g/mL, how many liters of blood are donated if 575 g of blood are given?
1) 0.548 L
2) 1.25 L
3) 1.83 L
Learning Check
112
1) 0.548 L
Unit Plan: g mL L
575 g x 1 mL x 1 L = 0.548 L 1.05 g 1000 mL
density metric factor factor
Solution
113
Density Using Volume Displacement
The volume of zinc is calculated from the displaced volume 45.0 mL - 35.5 mL = 9.5 mL = 9.5 cm3
Density zinc = mass = 68.60 g = 7.2 g/cm3
volume 9.5 cm3
114
A group of students collected 125 empty aluminum cans to take to the recycling center. If 21 cans make 1.0 pound of aluminum, how many liters of aluminum (D=2.70 g/cm3) are obtained from the cans?
1) 1.0 L 2) 2.0 L 3) 4.0 L
Learning Check
115
1) 1.0 L
125 cans x 1.0 lb x 454 g x 1 cm3
21 cans 1 lb 2.70 g
x 1 mL x 1 L = 1.0 L 1 cm3 1000 mL
Solution
116
You have 3 metal samples. Which one will displace the greatest volume of water?
1 2 3
25 g of aluminum2.70 g/mL
45 g of gold19.3 g/mL
75 g of lead11.3 g/mL
Learning Check
117
1)
Calculate the volume for each metal and select the metal that has the greatest volume.
1) 25 g x 1 mL = 9.3 mL aluminum2.70 g
2) 45 g x 1 mL = 2.3 mL gold19.3 g
3) 75 g x 1 mL = 6.6 mL lead11.3 g
Solution
25 g of aluminum2.70 g/mL
118
2. 12 Specific Gravity
Specific Gravity (sp gr): density of a substance divided by the density of water at the same temperature. Specific Gravity is unitless. At normal temperature, the density of water is close to 1 g/mL. Thus, specific gravity of a substance at normal temperature is equal to the density.
Density of substance (g/ml)
Density of water at the same temperature (g/ml)Specific gravity =
119
The specific gravity of a liquid can be measured using an instrument called a hydrometer, which consists of a weighted bulb on the end of a calibrated glass tube, as shown in the following Fig 2.6. The depth to which the hydrometer sinks when placed in a fluid indicates the fluid’s specific gravity.
120
Learning Check
Corn oil has a density of 0.92 g/mL. What is the specific gravity of corn oil?
1) 0.92 2) 0.92 g 3) 1.1
121
Solution
Corn oil has a density of 0.92 g/mL. What is the specific gravity of corn oil?
1) 0.92
specific gravity = 0.92 g/mL = 0.92
1.00 g/mL
122
Learning Check
A bone sample has a mass of 52 g. If bone has a specific gravity of 1.8, what is the volume in milliliters of the bone sample?
1) 1.8 mL 2) 29 mL 3) 94 mL
123
Solution
2) 29 mLConvert the specific gravity to its densityusing the density of water1.8 x 1.00 g/mL = 1.8 g/mL
Use the density factor to cancel the initial unit.Volume = 52 g x 1 mL = 29 mL
1.8 g
124
Chapter Summary
Physical quantity, a measurable properties, is described by both a number and a unit.
Mass, an amount of matter an object contains, is measured in kilograms (kg) or grams (g).
Volume is measured in cubic meters (m3) or in liter (L) or milliliters (mL).
Temperature is measured in Kelvin (K) in SI system and in degrees Celsius (oC) in the metric system.
125
Chapter Summary Contd.
Measurement of small or large numbers are usually written in scientific notation, a product of a number between 1 and 10 and a power of 10.
A measurement in one unit can be converted to another unit by multiplying by a conversion factor.
Energy: the capacity to supply heat or to do work.
Potential energy – stored energy. kinetic energy – energy of moving particles.
126
Chapter Summary Contd. Heat: kinetic energy of moving particles in a
chemical reaction. Temperature: is a measure of how hot or cold an
object is. Specific heat: amount of heat necessary to raise
the temperature of 1 g of the substance by 1oC. Density: grams per milliliters for a liquid or
gram per cubic centimeter for a solid. Specific gravity: density of a liquid divided by
the density of water.
127
End of Chapter 2