chem 106, prof. j.t. spencer 1 che 106: general chemistry u chapter one copyright © james t....
TRANSCRIPT
Chem 106, Prof. J.T. Spencer 11
CHE 106: General Chemistry
CHAPTER ONE
Copyright © James T. Spencer 1995 - 1999
All Rights Reserved
Chem 106, Prof. J.T. Spencer 22
What is ChemistryWhat is Chemistry– Study of the “Physical” Properties Matter (Form and Function)
– Study of How Matter Changes (Reactivity)
Benefits of ChemistryBenefits of Chemistry– Pharmaceuticals
– Enhanced food production (fertilizers, herbicides, etc...)
– Plastics and Polymers
Why Study ChemistryWhy Study Chemistry– Core requirement (?)
– Central Science
EmploymentEmployment– Many fields
MatterMatter
Chapt. 1.1
BIO
Physics Medicine
GEO Engr
CHEM
Law
also: environmental economics electronics agriculture politics etc...
S.U. B.S.
Chem 106, Prof. J.T. Spencer 33
Chemistry; Common ChemicalsChemistry; Common Chemicals
acetic acid .........................................acetic acid .........................................vinegarvinegarcalcium hypochloride ......................calcium hypochloride ......................bleaching powderbleaching powdercalcium sulfate .................................calcium sulfate ................................. plaster of parisplaster of pariscarbon tetrachloride .......................carbon tetrachloride ....................... cleaning fluidcleaning fluidferric oxide .......................................ferric oxide ....................................... iron rustiron rustgraphite ............................................graphite ............................................ pencil leadpencil leadmagnesium sulfate ..........................magnesium sulfate ..........................Epsom saltsEpsom saltsnaphthalene......................................naphthalene...................................... mothballsmothballssilicon dioxide...................................silicon dioxide................................... sandsandsodium bicarbonate .........................sodium bicarbonate .........................baking sodabaking sodasodium borate...................................sodium borate................................... boraxboraxsodium hydroxide ............................sodium hydroxide ............................ lyelyesulfuric acid......................................sulfuric acid...................................... battery acidbattery acidsucrose...............................................sucrose............................................... cane sugarcane sugar
Chem 106, Prof. J.T. Spencer 44
Chemistry; Chemical ProductionChemistry; Chemical Production
Sulfuric Nitrogen Oxygen Ethylene Lime AmmoniaPropylene NaOH PhosphoricChlorine0
20
40
60
80
100
Bil
lion
s of
lbs
HH22SOSO44
NN22
OO22 CC22HH44
CaOCaO NHNH33
CC33HH66 NaOHNaOHHH33POPO44
ClCl22
19951995Chemical and Engineering NewsChemical and Engineering News
Chem 106, Prof. J.T. Spencer 55
Nanoscale Chemistry
Use simpler molecular units are molecular-architectural elements
Chem 106, Prof. J.T. Spencer 66
Nanoscale Chemistry
Chem 106, Prof. J.T. Spencer 77
Nanosystems
Chem 106, Prof. J.T. Spencer 88
Nanomachines
red blood cell
Interstellar Space Travel - Significant concepts in this area include: launch vehicles, the space elevator, interplanetary transportation, the swarm concept, smart dust, extraterrestrial materials utilization, terraforming, suspended animation, space telescopes and virtual sample return.Human Therapeutics - Nanotechnology has caused scientists to re-examine the problems of the human body from the perspective of atomic- engineering. By assuming a nanotechnological
point of view, the resolution of therapeutic ailments becomes simple.Nano-Robots and Nano-Computers with advanced Artificial Intelligence - Nanotechnology will operate under the control of nano-sized computers which will manage the process of Molecular Manufacturing. In order to achieve this, it will be necessary to devise advanced Artificial Intelligence that will be able to automate and regulate Molecular Manufacturing systems.
Chem 106, Prof. J.T. Spencer 99
Matter; A ReviewMatter; A Review
Chapt. 1.2
Definition of MatterDefinition of Matter– anything that occupies space and has mass
StatesStates– gas (vapor); no fixed volume or shape, compressable
– liquid; fixed volume no fixed shape, mostly incompressable
– solid; fixed volume and shape, incompressable
FormsForms– Substances (pure or single); has a fixed composition and distinct
properties. Most things encountered are mixtures of substances.
PropertiesProperties– Physical Properties; can be measured without changing the substance,
i.e., color, density, melting point, etc...
– Chemical Properties; the way a substance changes (reacts), i.e., combustion
Chem 106, Prof. J.T. Spencer 1010
Matter; Elements and CompoundsMatter; Elements and Compounds
Chapt. 1.2
SubstancesSubstances– Elements - substances which cannot be decomposed into simpler
substances (see periodic table)
– Compounds- substances which can be separated into two or more elements
ElementsElements– 110 Known (periodic table to be revisited)
– make up all matter and composed of “subatomic particles”
– symbols used for abbreviations (from older or common names)
CompoundsCompounds– Elements combined in a definite proportion by mass (law of definite
proportion)
– properties different than consititutent elements
Water; example of mixtures, compound and elements?Water; example of mixtures, compound and elements?
Chem 106, Prof. J.T. Spencer 1111
Matter; Elements and Periodic TableMatter; Elements and Periodic Table
See Website: http://the-tech.mit.edu/Chemicool
Periodic TablePeriodic Table
Chem 106, Prof. J.T. Spencer 1212
Matter; A ReviewMatter; A Review
Chapt. 1.2
Mixtures; combinations of substancesMixtures; combinations of substances
– MixtureMixture- combination of two or more substances in which each retains its own chemical identity (and properties). Vary widely by composition (infinite possibilities of combining ratios), can be separated using the different physical properties of the component substances.
– Homogeneous Homogeneous - appears the same throughout (solutions), liquid, gas and solid solutions are possible.
– Heterogeneous Heterogeneous - mixtures which do not have the same (uniform) appearance throughout.
Chem 106, Prof. J.T. Spencer 1313
Salt and Sand Mixture Ink from Cabbage Juicesolubility and filtrationsolubility and filtration chromatography chromatography
Water from Salt Water Iron and Gold Mixturedistillationdistillation magnetic propertiesmagnetic properties
melting point melting point differencesdifferences
chem. reactivity chem. reactivity (acids)(acids)
Iodine from Copper Chloridesolubility and filtrationsolubility and filtration
Matter; A ReviewMatter; A Review
Chapt. 1.2
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Chem 106, Prof. J.T. Spencer 1414
Matter; A ReviewMatter; A Review
Chapt. 1.2
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Filtration Sand from SaltSand from Salt
Filter
Everyday ExamplesEveryday Examples;Auto Oil FilterAuto Air FilterAquarium Water FilterSpaghetti StrainerWindow ScreensRegistrar
Flow
Chem 106, Prof. J.T. Spencer 1515
Matter; A ReviewMatter; A Review
Chapt. 1.2
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Distillation Water from Salt WaterWater from Salt Water
NaCl(aq)
NaCl(s) + H2O(l)
Chem 106, Prof. J.T. Spencer 1616
Matter; A ReviewMatter; A Review
Chapt. 1.2
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Chromatograpgy Dyes from M&M’sDyes from M&M’s
Before After
Dyes
Chem 106, Prof. J.T. Spencer 1717
Matter; A ReviewMatter; A Review
Chapt. 1.3
ChangesChanges
– Physical - Changes in appearance but not identity, i.e., evaporation, melting (all changes of state)
– Chemical - transformation into a different substance
Chemical ChangesChemical Changes Physical ChangesPhysical Changes
burning burning meltingmelting CC66HH1212OO66 + 6O + 6O22 6CO 6CO22 + 6H + 6H22OO H H22O(s)O(s) HH22O(l)O(l)
chemical reactionschemical reactions sublimationsublimation NaOH + HCl HNaOH + HCl H22O + NaCl O + NaCl H H22O(s)O(s) HH22O(g)O(g)
corrosioncorrosion dissolutiondissolution 4Fe + 3O4Fe + 3O22 2 Fe 2 Fe22OO3 3 H H22O(l ) + NaCl(s)O(l ) + NaCl(s) NaCl(aq)NaCl(aq)
Chem 106, Prof. J.T. Spencer 1818
MatterMatter
MatterMatter
Uniform ?Uniform ?HeterogeneousHeterogeneousMixtureMixture
HomogeneousHomogeneous
Can be separatedCan be separatedby physical methodsby physical methodsPure SubstancePure Substance
HomogeneousHomogeneousMixture (solution)Mixture (solution)
Decomposed ?Decomposed ?
CompoundCompoundElementElement
YesYesNoNo
NoNo
NoNo
YesYes
YesYes
Chem 106, Prof. J.T. Spencer 1919
ObservationsObservationsand Experimentsand Experiments
Patterns and Patterns and TrendsTrends
Form and testForm and testhypothesishypothesis
TheoryTheory
Scientific MethodScientific Method
Chem 106, Prof. J.T. Spencer 2020
Observations to TheoryObservations to Theory
ObservationsObservations Theory Theory
Chem 106, Prof. J.T. Spencer 2121
Observations to TheoryObservations to Theory
ObservationsObservations Theory Theory
Chem 106, Prof. J.T. Spencer 2222
Observations to TheoryObservations to Theory
ObservationsObservations Theory Theory
Chem 106, Prof. J.T. Spencer 2323
Matter; MeasurementMatter; Measurement
AA BB
Which is True?Which is True?A = BA = BA > BA > BA < BA < B
Chem 106, Prof. J.T. Spencer 2424
Matter; MeasurementMatter; Measurement
AA BB
Which is True?Which is True?A = BA = BA > BA > BA < BA < B
Chem 106, Prof. J.T. Spencer 2525
Matter; MeasurementMatter; Measurement
AA BB
Which is True?Which is True?A = BA = BA > BA > BA < BA < B
Chem 106, Prof. J.T. Spencer 2626
Matter; MeasurementMatter; Measurement
Chapt. 1.4
SystemsSystems
– Metric - base 10
– SI- international scientific system
– mass Kilogram
– length Meter
– time Second
– electric current Ampere
– temperature Kelvin
– light Candela
– Amount Mole Factor label method for conversionsFactor label method for conversions
Chem 106, Prof. J.T. Spencer 2727
Matter; MeasurementMatter; Measurement
Chapt. 1.4
PrefixesPrefixes
Mega M 106
Kilo k 103
Deci d 10-1
Centi c 10-2
Milli m 10-3
Micro 10-6
Nano n 10-9
Chem 106, Prof. J.T. Spencer 2828
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: What fraction of a second is a picosecond, ps?
Chem 106, Prof. J.T. Spencer 2929
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: What fraction of a second is a picosecond, ps?
10-12 second
Chem 106, Prof. J.T. Spencer 3030
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Common Units:Length and Mass
Length - unit of distance measured in meters
Mass - measures the amount of matter in an object in grams
TemperatureKelvinCelsius °C = 5/9 (°F -32)
K = °C + 273.15
Chem 106, Prof. J.T. Spencer 3131
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F
Chem 106, Prof. J.T. Spencer 3232
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °FK = °C + 273.15
= -11.5 + 273.15
Chem 106, Prof. J.T. Spencer 3333
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °FK = °C + 273.15
= -11.5 + 273.15
= 261.65 K
Chem 106, Prof. J.T. Spencer 3434
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °FK = °C + 273.15
= -11.5 + 273.15
= 261.65 K
= 261.7 K
Chem 106, Prof. J.T. Spencer 3535
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F -32)
Chem 106, Prof. J.T. Spencer 3636
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
Chem 106, Prof. J.T. Spencer 3737
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
9(-11.5) + 32 = x
5
Chem 106, Prof. J.T. Spencer 3838
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
9(-11.5) + 32 = x
5
11.3°F = x
Chem 106, Prof. J.T. Spencer 3939
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Derived Units:Volume
Length x length x lengthmeasured in cm3, which is equal to mL
Chem 106, Prof. J.T. Spencer 4040
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Derived Units:Density
amount of mass per unit volumemeasured in g/cm3, or g/mL
Chem 106, Prof. J.T. Spencer 4141
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed?
Chem 106, Prof. J.T. Spencer 4242
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
Chem 106, Prof. J.T. Spencer 4343
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
= 15.0 g 0.789 g/mL
Chem 106, Prof. J.T. Spencer 4444
Matter; MeasurementMatter; Measurement
Chapt. 1.4
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
= 15.0 g 0.789 g/mL
= 19.0 mL
Chem 106, Prof. J.T. Spencer 4545
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Precision and AccuracyPrecision and Accuracy– Precision - how closely individual measurements
agree– Accuracy- how closely the measurements agree with
the true value
Significant FiguresSignificant Figures– All measurements are inaccurate intrinsically
– measured quantities are reported such that the last figure is uncertain
Chem 106, Prof. J.T. Spencer 4646
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Good PrecisionPoor Accuracy
Good PrecisionGood Accuracy
Poor PrecisionPoor Accuracy
Chem 106, Prof. J.T. Spencer 4747
Determining Significant FiguresDetermining Significant Figures
–all non zero digits are significantall non zero digits are significant
– zeros between nonzero digits are significantzeros between nonzero digits are significant
– zeros to the left of first nonzero digit are not zeros to the left of first nonzero digit are not significantsignificant
– zeros at the end of a number and to the right zeros at the end of a number and to the right of a decimal point are significantof a decimal point are significant
–when a number ends in a zero but with no when a number ends in a zero but with no decimal point, the zero may or may not be decimal point, the zero may or may not be signigicant (use scientific notation)signigicant (use scientific notation)
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Chem 106, Prof. J.T. Spencer 4848
Determining Significant FiguresDetermining Significant Figures
3.573 has 4 significant figures3.573 has 4 significant figures
0.073 has 2 significant figures0.073 has 2 significant figures
3.070 has 4 significant figures3.070 has 4 significant figures
0.003 has 1 significant figures0.003 has 1 significant figures
- - multiplication and divisionmultiplication and division; result can have no ; result can have no more than the figure with the fewest significant more than the figure with the fewest significant figuresfigures
- - addition and subtractionaddition and subtraction; result can have the ; result can have the same number of decimal places as the term with same number of decimal places as the term with the least number of decimal placesthe least number of decimal places
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Chem 106, Prof. J.T. Spencer 4949
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: A balance has a precision of 0.001 g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
Chem 106, Prof. J.T. Spencer 5050
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: A balance has a precision of 0.001 g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
25.XXX
Chem 106, Prof. J.T. Spencer 5151
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: A balance has a precision of 0.001 g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
25.XXX
5 sig figs
Chem 106, Prof. J.T. Spencer 5252
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g
B) 2.3 x 104 cm
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 5353
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 5454
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 5555
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) 0.00134 m3 3 sig figs
Chem 106, Prof. J.T. Spencer 5656
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
Chem 106, Prof. J.T. Spencer 5757
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
Chem 106, Prof. J.T. Spencer 5858
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
x = 2172.6144 m
Chem 106, Prof. J.T. Spencer 5959
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs 1 is infinitely significant
Chem 106, Prof. J.T. Spencer 6060
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.5
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs x = 2170 m 1 is infinitely significant
Chem 106, Prof. J.T. Spencer 6161
Use Units throughout the calculation (helps “guide” calculation.
Should always yield the proper units Uses conversion factors Example; How fast is 50 mph in in/sec.?
Dimensional AnalysisDimensional Analysis
50 mi.50 mi. 1 hour1 hour 5280 ft5280 ft 12 in.12 in. = = inin1 hour1 hour 3600 sec.3600 sec. 1 mi.1 mi. 1 ft1 ft sec.sec.
Chem 106, Prof. J.T. Spencer 6262
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
Chem 106, Prof. J.T. Spencer 6363
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi
Chem 106, Prof. J.T. Spencer 6464
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km
0.62137 mi
Chem 106, Prof. J.T. Spencer 6565
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km = 804.674 km
0.62137 mi
Chem 106, Prof. J.T. Spencer 6666
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km = 804.674 km
0.62137 mi
* answer can only have 4 sig figs; 804.7 km
Chem 106, Prof. J.T. Spencer 6767
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
Chem 106, Prof. J.T. Spencer 6868
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm
Chem 106, Prof. J.T. Spencer 6969
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm 1 m 103 mm
1012 pm 1 m
Chem 106, Prof. J.T. Spencer 7070
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm 1 m 103 mm = 1.54 x 10-7 mm
1012 pm 1 m
Chem 106, Prof. J.T. Spencer 7171
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
Chem 106, Prof. J.T. Spencer 7272
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi
gal
Chem 106, Prof. J.T. Spencer 7373
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi 1 km
gal 0.62137 mi
Chem 106, Prof. J.T. Spencer 7474
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi 1 km 1 gal
gal 0.62137 mi 3.7854 L
Chem 106, Prof. J.T. Spencer 7575
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi 1 km 1 gal = 11.9041 km
gal 0.62137 mi 3.7854 L L
Chem 106, Prof. J.T. Spencer 7676
Dimensional AnalysisDimensional Analysis
Chapt. 1.6
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi 1 km 1 gal = 11.9041 km
gal 0.62137 mi 3.7854 L L
* 2 sig figs = 12 km L
Chem 106, Prof. J.T. Spencer 7777
Matter: Chemical and Physical ChangesMatter: Chemical and Physical Changes Elements and CompoundsElements and Compounds Units of MeasurementUnits of Measurement Uncertainty and Significant FiguresUncertainty and Significant Figures Precision and AccuracyPrecision and Accuracy ““Factor Label” Method (Dimensional Factor Label” Method (Dimensional
Analysis)Analysis)
Chapter One; ReviewChapter One; Review