measurements and their uncertainty
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Measurements and their uncertainty. Objectives. Convert measurements to scientific notation Distinguish among accuracy, precision and error of measurement Determine the number of significant figures in a measurement and in a calculated answer. Measurements. - PowerPoint PPT PresentationTRANSCRIPT
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Measurements and their uncertainty
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Objectives
Convert measurements to scientific notation
Distinguish among accuracy, precision and error of measurement
Determine the number of significant figures in a measurement and in a calculated answer
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Measurements
Definition – quantity that has both a number and a unit
Measurements are made every day:Buying productsSports activitiesCooking
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Measurement types
2 types of measurementsQualitative – measurements are words, not numbers – hot, heavy
Quantitative – measurements involve numbers and depends on: Reliability of measuring instrument
The care with which it is read
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Scientific Notation
Number is written as the product of two numbers:A coefficient10 raise to a power
Example:602,000,000,000,0000,0000,000,000
6.02 x 1023
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Accuracy, Precision, and Error
Accuracy – how close measurement is to true valueMeasured value must be compared to correct value
Precision – how close the measurements are to each otherCompare values of two or more repeated measurements (reproducible)
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Precision vs. Accuracy
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Determining Error
Accepted value – correct value based on reliable referencesExample: Density table pg 90
Experimental value – value measure in the lab
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Determining Error
Error – difference between experimental value and accepted valueError = exp. value – accepted value
Error can be either positive or negative
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Percent Error
Percent error – absolute value of error divided by the accepted value multiplied by 100
Percent error = |error| accepted value
x 100
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Sample Problem
For a boiling point measurement of water in the lab you read 99.1 oC. What is the percent error?
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Sample Problem
For a boiling point measurement of water in the lab you read 99.1 oC. What is the percent error?Answer: 0.9%
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Why Is There Uncertainty?
Measurements are performed with instrumentsNo instrument can be read to an infinite number of decimal places
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Why Is There Uncertainty?
Which of these has the greatest uncertainty?
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Significant Figures
Significant digits – in a measurement it includes all of the digits that are unknown plus a last digit that is estimated
Measurements are reported in correct sig figs b/c calculated answers depend on number of sig figs in the values used in the calculations
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Figure 3.5 Significant Figures - Page 67
Which measurement is the best?
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Sig Fig Rules
Non – zeros always count as significant figures:
3456
4 sig figs
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Sig Fig Rules
ZerosLeading zeros do not count as significant figures
0.0486
3 sig figs
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Sig Fig Rules
ZerosCaptive zeros always count as significant figures
16.07
4 sig figs
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Sig Fig Rules
ZerosTrailing zeros are significant only if the number contains a decimal point
9.300 9300
4 sig figs 2 sig figs
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Sig Fig Rules
Two special situations – have unlimited number of sig figsCounted items
23 people, 435 thumbtacksExactly defined quantities
60 minutes = 1 hour
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Sig Fig Practice
How many sig figs in the following?1.0070 m17.10 kg100890 L3.29 x 103 s0.0054 cm3,200,000 mL5 dogs
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Sig Figs in Calculations
A calculated answer cannot be more precise than the least precise measurement from which it was calculatedThe chain is only as strong as its weakest link
Calculated values need to be rounded
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Rounding
Decide how many sig figs are needed
Round to that many digits counting from the left!Is the next digit <5? Drop itIs the next digit >5? Increase by 1
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Problems
Round off each measurement to the number of sig figs shown in ( ). Write the answers in scientific notation.314.721 (four)0.001755 (two)8792 (two)
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Rounding – Addition and Subtraction
Answer should be rounded to same number of decimal places as the LEAST number of decimal places in problem
Problem:Calculate the sum:
12.52 m + 349.0 m + 8.24 m
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Rounding – Addition and Subtraction
Answer should be rounded to same number of decimal places as the LEAST number of decimal places in problem
Problem:Calculate the sum:
12.52 m + 349.0 m + 8.24 m369.8 m
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Rounding – Multiplication and Division
Round the answer to the same number of significant figures as the LEAST number of sig figs in the problem
How many sig figs for the following operations:7.55 x 0.34 meters2.10 x 0.70 meters2.4526/8.4
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Rounding – Multiplication and Division
Round the answer to the same number of significant figures as the LEAST number of sig figs in the problem
How many sig figs for the following operations:7.55 x 0.34 meters 2 sig figs2.10 x 0.70 meters 2 sig figs2.4526/8.40 3 sig figs
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Section Assessment
A technician experimentally determined the boiling point of octane to be 124.1 oC. The actual BP is 125.7 oC. Calculate the error and percent error.
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Section Assessment
Determine the number of sig figs in the following:11 soccer players10,800 meters0.070020 meters5.00 cubic meters
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The International System of Units
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Objectives
List SI units of measurement and common SI prefixes
Distinguish between the mass and weight of an object
Convert between Celsius and Kelvin temperature scales
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International System of Units
SI – from French nameMeasurements depend on units that are used as reference standards
In chemistry we use metric system
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5 SI Base Units
SI units normally used in chemistry:Quantity SI base unit Symbol
Length Meter m
Mass Kilogram kg
Temperature Kelvin K
Time Seconds s
Amount of substance
Mole mol
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Nature of Measurements
Measurement – quantitative observation consisting of 2 parts:NumberUnit
Example: 20 grams or 20 g
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SI
Non-SI units are used in chemistry as well:Liter – volumeCelsius – temperatureCalorie - heat
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Common SI Prefixes
Prefix Abbreviation Meaning ExponentMega- M Million 106
Kilo- k thousand 103
Deci- d tenth 10-1
Centi- c hundredth 10-2
Milli- m thousandth 10-3
Micro- millionth 10-6
Nano- n billionth 10-9
Pico- P trillionth 10-12
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Units of Length
SI unit – meterMeasured using rulersMost common metric units of length are:Centimeter – cmMeter – mKilometer - km
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Volume
Space occupied by sample of matter
Calculated from a solid by multiplying length x width x heightThus, SI is cubic meter or cm3
We normally use liters for volume1 mL = 1 cm3
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Measuring Volume
Graduated cylinderPipetsBuretsVolumetric flaskSyringes
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Volume Changes
With an increase in temperature, the volume also increasesSeen most in gases
Instruments are calibrated for 20 oC which is room temperature
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Units of Mass
Mass – measure of the quantity of matter presentWeight – force that measures the pull by gravity – changes with location
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Measuring Mass
SI unit for mass is kg – we commonly use grams in the laboratory
Mass is measured using a triple beam balance (or electric balance)
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Temperature
Measure of how hot or cold something is
Heat moves from object of higher temperature to object of lower temp
2 units used:KelvinCelsius
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Temperature
Celsius scale defined by two readily determined temperatures:Freezing point of water = 0 oCBoiling point of water = 100 oC
Kelvin scale does not use the degree sign, but is just represented by K• absolute zero = 0 K (thus no negative values)
• formula to convert: K = oC + 273
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Sample Problem
Normal human body temperature is 37 oC. What is the temperature in Kelvin?
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Energy
Energy is the capacity to do work or produce heat
Energy can be measured using:Joule (J) – the SI unit for energyCalorie (cal) – the heat needed to raise 1 gram of water by 1 oC
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Energy
Conversions between Joules and Calories can be carried out by using the following relationship:
1 cal = 4.184 J
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Section Assessment
Name the quantity measured by each of the SI base units and give the SI symbol of the unit.
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Conversion Problems
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Objectives
Construct conversion factors from equivalent measurements
Apply the technique of dimensional analysis to a variety of conversion problems
Solve problems by breaking the solution into steps
Convert complex units, using DA
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Conversion Factors
A “ratio” of equivalent measurements
Start with 2 things that are the same:1 meter = 100 centimeters
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Practice
Write 2 conversion factors for the following:Between kilograms and gramsBetween feet and inchesUsing 1.096 qt = 1.00 L
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Why Use Conversion Factors?
We can multiply them to change the units
Question: 13 inches is how many yards?We know that 36 inches = 1 yard
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Dimensional Analysis
A way to analyze and solve problems by using units of measurement
Dimension = a unit Analyze = to solve
Using units so solve the problems
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Dimensional Analysis
DA provides alternative approach to problem solving, instead of with equation or algebra.
A ruler is 12.0 inches long. How long is it in cm? ( 1 inch = 2.54 cm)
How long is this in meters?A race is 10.0 km long. How far is this in miles, if: 1 mile = 1760 yards 1 meter = 1.094 yards
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Problem
How many minutes are there in a week?
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Problem
An experiment requires that each student use an 8.5-cm length of magnesium ribbon. How many students can do the experiment if there is a 570-cm length of magnesium ribbon available?
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Problem
Convert:0.044 km to m4.6 mg to g0.107 g to cg
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Complex Units
Complex units – units that are expressed as a ratio of two unitsSpeed – meters/hour
Sample problem: Change 15 m/hr to cm/s
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Density
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Objectives
Calculate the density of a material from experimental data
Describe how density varies with temperature
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Density
Density – relationship between mass and volume
Formula Density = mass
volumeCommon units: g/mL or g/cm3
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Density
If you recall, density is a physical property so it does not depend on sample size
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Density and Temperature
What happens to density as the temperature of an object increases?Mass remains the sameIncrease in volume as temperature increases
Density DECREASES as temperature increases
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Density and Water
Water is an exception to the density rule
Over certain temperatures, the volume of water increases as the temperature decreasesDoes ice float in liquid water?Why?
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Section Assessment
A 68 g bar of gold is cut into 3 equal pieces. How does the density of each piece compare to the density of the original gold bar?
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Section Assessment
What is the volume, in cubic centimeters, of a sample of cough syrup that has a mass of 50.0 g? The density of cough syrup is 0.950 g/cm3