Chapter 2 Measurements in Chemistry. Standard measuring device. Standard scale gram (g)


 Felicity Maxwell
 4 years ago
 Views:
Transcription
1 1 Chapter 2 Measurements in Chemistry Standard measuring device Standard scale gram (g)
2 2 Reliability of Measurements Accuracy closeness to true value Precision reproducibility Example: 98.6 o F 98.5 o F 98.7 o F average: precision: 0.1 o F o F o F
3 3 Ch. 2.1 Measurement Systems English & metric
4 4 Ch. 2.2 Metric System Units base unit =
5 5 base unit = mass vs weight
6 base unit = 6
7 7 10cm x 10cm x 10cm 1 L = 1000 ml
8 8 Table 2.1 Common Metric System Prefixes You must know all of these for exams and quizzes.
9 9 Ch. 2.3 Exact and Inexact Numbers Exact no uncertainty direct count defined equivalency Inexact any measurement has a degree of uncertainty
10 10 Ch. 2.4 Uncertainty in Measurement and Significant Figures # of significant figures = all certain digits + one estimated digit 2 sig. fig. 3 sig. fig.
11 Guidelines for Determining Significant Figures 1. All nonzero digits are significant. 2. Zeros may or may not be significant. a. Leading zeros not significant sig fig sig fig b. Confined zeros always significant sig fig sig fig c. Trailing zeros are significant if a decimal point is present in the number sig fig sig fig 11
12 12 Trailing zeros in numbers that do not contain a decimal point: g ambiguous To remove ambiguity, use prefixes or scientific notations (Ch 2.6) kg 5 sig fig 30.6 kg 3 sig fig Stoker text pg o F = 3 sig fig 30 o C = 2 sig fig
13 Ch. 2.5 Significant Figures and Mathematical Operations Rounding off Numbers These rules are listed on page 36 of your lab manual: 1. If the first nonsignificant figure is less than 5, drop it and all other nonsignificant figures. 2. If the first nonsignificant figure is more than 5 or is 5 followed by digits other than all zeros, drop all nonsignificant figures and increase the last significant figure by If the first nonsignificant figure is 5 alone or is 5 followed by only zeros, drop all nonsignificant figures and increase the last significant figure by 1 if it is odd but leave it alone if it is even. (Round Even Rule) 13
14 14 Examples of rounding off numbers round to 2 sig fig less than 5, round down = round to 2 sig fig a 5 followed by nonzeros, round up = round to 4 sig fig a 5 followed by zero, round even = round to 4 sig fig a 5 alone, round even =
15 15 Operational Rules 1. multiplication and division least number of sig fig in any of the measurements x 5.1 = (63.495) calculator answer sig fig sig fig correct answer = sig fig
16 16 2. addition and subtraction common number of digits to the right of the decimal point ( ) calculator answer correct answer to the common hundredth place
17 17 Mixed mode calculation Always watch the significant figures of intermediate answers ( ) x = calculator answer = correct answer sig fig for intermediate answer Round only the final answer!
18 18 Ch. 2.6 Scientific Notation A x 10 n Exponent Coefficient 1000 = 1 x 10 x 10 x 10 = 1 x = 1 = 1 = 1 x x ,000 = 7.5 x 10 4 decimal point is moved places = 5.6 x 106 decimal point is moved places
19 19 Significant Figures and Scientific Notation 37,000 = x sig fig x 10 4 sig fig 3.70 x 10 4 sig fig 3.7 x 10 4 sig fig 4 x 10 4 sig fig
20 Ch. 2.7 Conversion Factors Obtained from equalities and used in dimensional analysis (factor unit method) 12 in. = 1 ft 12 in. = 1 1 ft = 1 1 ft 12 in. example: Convert 2.5 ft into inches 2.5 ft x 12 in. = in. 1 ft information x conversion = information given factor sought 20
21 21 sample calculation: convert L to ml from table 2.1: which is equal to: 1 ml = 103 L 1000 ml = 1 L (preferred) conversion factors: 1000 ml 1L. 1 L 1000 ml L x 1000 ml = ml 1 L
22 Table 2.2 Equalities and Conversion Factors 22
23 23 ft to m not given in Table 2.2 but 1.00 m = 39.4 in. and we know 1 ft = 12 in. ft in. m 38 ft x 12 in. x 1 m = ( ) 1 ft 39.4 in. correct answer: m
24 24 Ch. 2.9 Density demo Pb vs styrofoam density = mass volume = m V usual units: g/cm 3 solids g/ml liquids g/l gases
25 25 Table 2.3 Densities of Selected Substances Density of water at 4 o C = need to memorize. g/ml This is the only density you
26 26 Fig. 2.9 A penny floats on liquid mercury (Hg)
27 27 Density is an Intensive Property Intensive Properties are independent of the sample size and represent qualities that identify the substance: density b.p. m.p. Extensive Properties depend on the amount of matter: mass volume length
28 28 demo: Determination of the density and identity of an unknown silver cube mass: volume: density: identity of metal: Densities of Selected Silver Metals Beryllium Be 1.85 g/cm 3 Aluminum Al 2.70 g/cm 3 Zinc Zn 7.13 g/cm 3 Silver Ag 10.5 g/cm 3 Lead Pb 11.3 g/cm 3
29 29 Density as a Conversion Factor Example: A patient s urine sample has a density of 1.02 g/ml. How many grams of urine are eliminated on a day in which 1250 ml is excreted? information x conversion = information given factor sought 1250 ml x 1.02 g = (1275) g calculator answer ml correct answer = g
30 30 Ch Temperature Scales Figure 2.10 Conversions Between Temperature Scales o F = 9 ( o C) + 32 o C = 5 ( o F 32) 5 9 K = o C o F 32 = o C
31 31 Sample calculation: Convert 3650 o C into o F o F 32 = o C o F 32 = o F = (3650 x 180/100) + 32 o F = sig fig
32 32 Ch Heat Energy and Specific Heat Temperature vs Heat Energy Intensive Property Extensive Property Common Unit of Heat Energy: calorie (cal) One cal is the amount of heat energy needed to raise the temperature of 1 g of water by 1 o C. Specific heat is the quantity of heat energy, in cal, necessary to raise the temperature of 1 g of a substance by 1 o C.
33 33 Table 2.4 Specific Heats of Selected Common Substances You must KNOW the specific heat of water = 1 cal/g o C (this is a defined quantity and has no uncertainty) demo: burn $ bill
34 34 Specific heat (c) = cal. g x o C cal = c x g x o C heat energy = specific heat x mass x temperature change heat energy (absorbed or released) = c x m x t
35 Sample calculation: 5.5 g of Au at 25 o C is heated by 10 cal of heat. What is the final temperature? c Au = cal/g o C heat energy (absorbed or released) = c x m x t 10 cal = cal/g o C x 5.5 g x t t = 59 o C t final = t initial + t = + 59 o C = 35
36 36 Exp 3 Determination of the specific heat of a metal hot metal + cold water t metal decreases t water increases t final is heat loss of metal = heat gain of water c 1 x m 1 x t 1 = c 2 x m 2 x t 2
37 37 Other common units for heat energy The joule (J) 1 cal = J The dietary Calorie (must know) 1 Cal = 1000 cal = 1 kcal Average basic metabolic rate: 2000 Cal/day 3500 Cal/lbs to gain or lose body weight Carbohydrates Fat Protein Hambuger Green beans Apples 4.1 Cal/g 9.3 Cal/g 4.1 Cal/g 3.6 Cal/g 0.38 Cal/g 0.59 Cal/g
38 Sample calculation: One ounce of cereal gives 112 Cal of energy on oxidation. How many kg of water can be heated from 20 o C to 30 o C by burning the cereal? (The specific heat of water, the equation, and the necessary conversion factors for this question will not be given on exams and quizzes.) 38 Heat energy released by cereal and absorbed by the water: 112 Cal = 112 kcal = cal heat energy = c x m x t m = heat energy c x t m = cal. 1 cal/(g o C) x (30 o C 20 o C) m = g = kg
UNIT (1) MEASUREMENTS IN CHEMISTRY
UNIT (1) MEASUREMENTS IN CHEMISTRY Measurements are part of our daily lives. We measure our weights, driving distances, and gallons of gasoline. As a health professional you might measure blood pressure,
More informationChapter 1: Chemistry: Measurements and Methods
Chapter 1: Chemistry: Measurements and Methods 1.1 The Discovery Process o Chemistry  The study of matter o Matter  Anything that has mass and occupies space, the stuff that things are made of. This
More informationSample Questions Chapter 2. Stoker
Sample Questions Chapter 2. Stoker 1. The mathematical meaning associated with the metric system prefixes centi, milli, and micro is, respectively, A) 2, 4, and 6. B) 2, 3, and 6. C) 3, 6, and 9. D) 3,
More informationChapter 2 Measurement and Problem Solving
Introductory Chemistry, 3 rd Edition Nivaldo Tro Measurement and Problem Solving Graph of global Temperature rise in 20 th Century. Cover page Opposite page 11. Roy Kennedy Massachusetts Bay Community
More information2.2 Scientific Notation: Writing Large and Small Numbers
2.2 Scientific Notation: Writing Large and Small Numbers A number written in scientific notation has two parts. A decimal part: a number that is between 1 and 10. An exponential part: 10 raised to an exponent,
More informationChapter 1 Lecture Notes: Science and Measurements
Educational Goals Chapter 1 Lecture Notes: Science and Measurements 1. Explain, compare, and contrast the terms scientific method, hypothesis, and experiment. 2. Compare and contrast scientific theory
More informationCHAPTER 2: MEASUREMENT AND PROBLEM SOLVING
CHAPTER 2: MEASUREMENT AND PROBLEM SOLVING Problems: 164, 6988, 91120, 123124 2.1 Measuring Global Temperatures measurement: a number with attached units When scientists collect data, it is important
More informationCHAPTER 4 DIMENSIONAL ANALYSIS
CHAPTER 4 DIMENSIONAL ANALYSIS 1. DIMENSIONAL ANALYSIS Dimensional analysis, which is also known as the factor label method or unit conversion method, is an extremely important tool in the field of chemistry.
More information10 g 5 g? 10 g 5 g. 10 g 5 g. scale
The International System of Units, or the SI Units Vs. Honors Chem 1 LENGTH In the SI, the base unit of length is the Meter. Prefixes identify additional units of length, based on the meter. Smaller than
More informationChapter Test B. Chapter: Measurements and Calculations
Assessment Chapter Test B Chapter: Measurements and Calculations PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.
More information1 Introduction The Scientific Method (1 of 20) 1 Introduction Observations and Measurements Qualitative, Quantitative, Inferences (2 of 20)
The Scientific Method (1 of 20) This is an attempt to state how scientists do science. It is necessarily artificial. Here are MY five steps: Make observations the leaves on my plant are turning yellow
More informationEXAMPLE EXERCISE 3.1 Metric Basic Units and Prefixes
EXAMPLE EXERCISE 3.1 Metric Basic Units and Prefixes Give the symbol for each of the following metric units and state the quantity measured by each unit: (a) gigameter (b) kilogram (c) centiliter (d) microsecond
More informationEXPERIMENT 4 THE DETERMINATION OF THE CALORIC CONTENT OF A CASHEW NUT
EXPERIMENT 4 THE DETERMINATION OF THE CALORIC CONTENT OF A CASHEW NUT Textbook reference: pp103105 Purpose: In this Activity, students determine how many calories are released per gram when cashews burn
More informationDETERMINING THE DENSITY OF LIQUIDS & SOLIDS
DETERMINING THE DENSITY OF LIQUIDS & SOLIDS 17 Density, like color, odor, melting point, and boiling point, is a physical property of matter. Therefore, density may be used in identifying matter. Density
More informationChapter 1 Chemistry: The Study of Change
Chapter 1 Chemistry: The Study of Change This introductory chapter tells the student why he/she should have interest in studying chemistry. Upon completion of this chapter, the student should be able to:
More information5 Answers and Solutions to Text Problems
Energy and States of Matter 5 Answers and Solutions to Text Problems 5.1 At the top of the hill, all of the energy of the car is in the form of potential energy. As it descends down the hill, potential
More informationAP Chemistry A. Allan Chapter 1 Notes  Chemical Foundations
AP Chemistry A. Allan Chapter 1 Notes  Chemical Foundations 1.1 Chemistry: An Overview A. Reaction of hydrogen and oxygen 1. Two molecules of hydrogen react with one molecule of oxygen to form two molecules
More informationWelcome to Physics 40!
Welcome to Physics 40! Physics for Scientists and Engineers Lab 1: Introduction to Measurement SI Quantities & Units In mechanics, three basic quantities are used Length, Mass, Time Will also use derived
More informationChapter 8 Unit Conversions
Chapter 8 Unit Conversions [M]athematics is the easiest of sciences, a fact which is obvious in that no one s brain rejects it. Roger Bacon (c. 1214c. 1294), English philosopher and scientist Stand firm
More information2. Room temperature: C. Kelvin. 2. Room temperature:
Temperature I. Temperature is the quantity that tells how hot or cold something is compared with a standard A. Temperature is directly proportional to the average kinetic energy of molecular translational
More information= 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C
Units and Dimensions Basic properties such as length, mass, time and temperature that can be measured are called dimensions. Any quantity that can be measured has a value and a unit associated with it.
More informationChapter 8 Unit Conversions
99 Chapter 8 Unit Conversions Review Skills 8.1 Unit Analysis An Overview of the General Procedure MetricMetric Unit Conversions EnglishMetric Unit Conversions 8.2 Rounding Off and Significant Figures
More informationThe volume of a penny will be calculated from its mass and density.
Measurement and Density In science a key concern is the quantities involved in chemical processes. These amounts can be directly measured or calculated from other measurements. A measurement consists of
More informationChemistry 11 Some Study Materials for the Final Exam
Chemistry 11 Some Study Materials for the Final Exam Prefix Abbreviation Exponent giga G 10 9 mega M 10 6 kilo k 10 3 hecto h 10 2 deca da 10 1 deci d 101 centi c 102 milli m 103 micro µ 106 nano n
More informationChapter 18 Temperature, Heat, and the First Law of Thermodynamics. Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57 Thermodynamics study and application of thermal energy temperature quantity
More informationFigure 1. A typical Laboratory Thermometer graduated in C.
SIGNIFICANT FIGURES, EXPONENTS, AND SCIENTIFIC NOTATION 2004, 1990 by David A. Katz. All rights reserved. Permission for classroom use as long as the original copyright is included. 1. SIGNIFICANT FIGURES
More informationChapter 3 Student Reading
Chapter 3 Student Reading If you hold a solid piece of lead or iron in your hand, it feels heavy for its size. If you hold the same size piece of balsa wood or plastic, it feels light for its size. The
More informationChapter 10: Temperature and Heat
Chapter 10: Temperature and Heat 1. The temperature of a substance is A. proportional to the average kinetic energy of the molecules in a substance. B. equal to the kinetic energy of the fastest moving
More informationWorksheet #17. 2. How much heat is released when 143 g of ice is cooled from 14 C to 75 C, if the specific heat capacity of ice is 2.087 J/(g C).
Worksheet #17 Calculating Heat 1. How much heat is needed to bring 12.0 g of water from 28.3 C to 43.87 C, if the specific heat capacity of water is 4.184 /(g? 2. How much heat is released when 143 g of
More informationSignificant Figures, Propagation of Error, Graphs and Graphing
Chapter Two Significant Figures, Propagation of Error, Graphs and Graphing Every measurement has an error associated with it. If you were to put an object on a balance and weight it several times you will
More informationThe Composition of Metals and Alloys
1 The Composition of Metals and Alloys Metals are shiny, malleable substances that conduct heat and electricity. They comprise the larest class of elements in the Periodic Table. All metals except mercury
More informationPhysics Notes Class 11 CHAPTER 2 UNITS AND MEASUREMENTS
1 P a g e Physics Notes Class 11 CHAPTER 2 UNITS AND MEASUREMENTS The comparison of any physical quantity with its standard unit is called measurement. Physical Quantities All the quantities in terms of
More informationCHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004. Name (print) SSN
CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004 Name (print) SSN Pledge: I have neither given nor received aid on this exam: Signature For ALL problems: SHOW ALL WORK TO GET FULL CREDIT
More informationName: Unit 2 Elements, Compounds and Mixtures and Physical/Chemical Properties and Changes. Elements, Compounds and Mixtures
Name: Unit 2 Elements, Compounds and Mixtures and Physical/Chemical Properties and Changes Day Page # Description IC/HW All 2 Warmup IC 1 3 5 Matter Notes IC 1 6 Nuts & Bolts IC 1 7 Elements, Compounds
More informationChapter 1 An Introduction to Chemistry
1 Chapter 1 An Introduction to Chemistry 1.1 What Is Chemistry, and What Can Chemistry Do for You? Special Topic 1.1: Green Chemistry 1.2 Suggestions for Studying Chemistry 1.3 The Scientific Method 1.4
More informationEXERCISE # 1.Metric Measurement & Scientific Notation
EXERCISE # 1.Metric Measurement & Scientific Notation Student Learning Outcomes At the completion of this exercise, students will be able to learn: 1. How to use scientific notation 2. Discuss the importance
More informationTest Bank  Chapter 3 Multiple Choice
Test Bank  Chapter 3 The questions in the test bank cover the concepts from the lessons in Chapter 3. Select questions from any of the categories that match the content you covered with students. The
More informationLAB #3: MEASURING SPECIFIC GRAVITY AND DENSITY. Setup and Materials for Experiment
Setup and Materials for Experiment 1 OVERVIEW The mass density of a substance is a measure of the mass that that substance contains in a given volume. Mathematically is written: ρ = m V ( Density = Volume
More informationWEEK 1. Engineering Calculations Processes Process Variables
WEEK 1 Engineering Calculations Processes Process Variables 2.1 Units and Dimensions Units and dimensions are important in science and engineering A measured quantity has a numerical value and a unit (ex:
More informationEnergy Conversions I. Unit of measure (most common one) Form Definition Example
Energy Conversions I Energy can take many forms, but any one form can usually be converted into another. And no matter what form we talk about, we can use conversion factors to calculate equivalent amounts
More informationREVIEW SHEETS INTRODUCTORY PHYSICAL SCIENCE MATH 52
REVIEW SHEETS INTRODUCTORY PHYSICAL SCIENCE MATH 52 A Summary of Concepts Needed to be Successful in Mathematics The following sheets list the key concepts which are taught in the specified math course.
More informationMEASUREMENT. Historical records indicate that the first units of length were based on people s hands, feet and arms. The measurements were:
MEASUREMENT Introduction: People created systems of measurement to address practical problems such as finding the distance between two places, finding the length, width or height of a building, finding
More informationModule 5: Combustion Technology. Lecture 34: Calculation of calorific value of fuels
1 P age Module 5: Combustion Technology Lecture 34: Calculation of calorific value of fuels 2 P age Keywords : Gross calorific value, Net calorific value, enthalpy change, bomb calorimeter 5.3 Calculation
More informationChapter 10 Temperature and Heat
Chapter 10 Temperature and Heat What are temperature and heat? Are they the same? What causes heat? What Is Temperature? How do we measure temperature? What are we actually measuring? Temperature and Its
More informationFollowing are Summaries from Two Chemistry Education Web Sites Concerning Significant Figure Rules
Following are Summaries from Two Chemistry Education Web Sites Concerning Significant Figure Rules From http://dbhs.wvusd.k12.ca.us/sigfigs/sigfigrules.html There are three rules on determining how many
More informationEXPERIMENT 9 Evaluation of the Universal Gas Constant, R
Outcomes EXPERIMENT 9 Evaluation of the Universal Gas Constant, R After completing this experiment, the student should be able to: 1. Determine universal gas constant using reaction of an acid with a metal.
More informationExperiment 6 ~ Joule Heating of a Resistor
Experiment 6 ~ Joule Heating of a Resistor Introduction: The power P absorbed in an electrical resistor of resistance R, current I, and voltage V is given by P = I 2 R = V 2 /R = VI. Despite the fact that
More informationEnergy and Matter CHAPTER OUTLINE CHAPTER GOALS
4 When sweat evaporates, it cools the skin by absorbing heat from the body. Energy and Matter CAPTER OUTLINE 4.1 Energy 4.2 The Three States of Matter 4.3 Intermolecular Forces 4.4 Boiling Point and Melting
More informationGuide To Preparation of Stock Standard Solutions
chemias ft Guide To Preparation of Stock Standard Solutions First Edition May 2011 Na+ 1000 ppm Guide To Preparation Of Stock Standard Solutions By: CHEMIASOFT May 2011 Page 2 of 61 Page 3 of 61 Table
More informationMath Concepts for Science
1 Math Concepts for Science Math for Science webpages originally created by Stephanie S. Baiyasi, D.V.M., Instructor, Science Division, Delta College Karen Constan, B.A., Staff Tutor, Teaching/Learning
More informationUnit A: Studying Materials Scientifically
ITEM BANKS Unit A: Studying Materials Scientifically Multiple choice: Circle the best answer. 1. What safety rules should you always follow while doing a science laboratory? a. Wear safety goggles at all
More informationName: Class: Date: 10. Some substances, when exposed to visible light, absorb more energy as heat than other substances absorb.
Name: Class: Date: ID: A PS Chapter 13 Review Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 1. In all cooling
More informationExperiment 1: Measurement and Density
Experiment 1: Measurement and Density Chemistry 140 Learning Objectives Become familiar with laboratory equipment and glassware Begin to see the link between measurement and chemical knowledge Begin to
More informationChapter 10 Temperature and Heat
Chapter 10 Temperature and Heat GOALS When you have mastered the contents of this chapter, you will be able to achieve the following goals: Definitions Define each of the following terms, and use it an
More informationType: Single Date: Homework: READ 12.8, Do CONCEPT Q. # (14) Do PROBLEMS (40, 52, 81) Ch. 12
Type: Single Date: Objective: Latent Heat Homework: READ 12.8, Do CONCEPT Q. # (14) Do PROBLEMS (40, 52, 81) Ch. 12 AP Physics B Date: Mr. Mirro Heat and Phase Change When bodies are heated or cooled their
More informationExperiment 6 Coffeecup Calorimetry
61 Experiment 6 Coffeecup Calorimetry Introduction: Chemical reactions involve the release or consumption of energy, usually in the form of heat. Heat is measured in the energy units, Joules (J), defined
More informationAP Physics 1 and 2 Lab Investigations
AP Physics 1 and 2 Lab Investigations Student Guide to Data Analysis New York, NY. College Board, Advanced Placement, Advanced Placement Program, AP, AP Central, and the acorn logo are registered trademarks
More informationThe Great Peanut Problem
elearning 2009 Introduction The Great Peanut Problem Calorimetry Publication No. 91259 All human activity requires burning food for energy. How much energy is released when food burns in the body? How
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More informationOPEN LESSON SAMPLE LESSONS FOR THE CLASSROOM FROM LAYING THE FOUNDATION
OPEN LESSON SAMPLE LESSONS FOR THE CLASSROOM FROM LAYING THE FOUNDATION Middle Grades Science Running the Stairs Measuring Work, Energy, and Power About this Lesson This activity can be used to introduce
More informationMeasurement and Calibration
Adapted from: H. A. Neidig and J. N. Spencer Modular Laboratory Program in Chemistry Thompson Learning;, University of Pittsburgh Chemistry 0110 Laboratory Manual, 1998. Purpose To gain an understanding
More informationConverting Units of Measure Measurement
Converting Units of Measure Measurement Outcome (lesson objective) Given a unit of measurement, students will be able to convert it to other units of measurement and will be able to use it to solve contextual
More informationChemistry 110 Lecture Unit 5 Chapter 11GASES
Chemistry 110 Lecture Unit 5 Chapter 11GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all
More informationCHEM 36 General Chemistry EXAM #1 February 13, 2002
CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show
More informationChapter 4: Transfer of Thermal Energy
Chapter 4: Transfer of Thermal Energy Goals of Period 4 Section 4.1: To define temperature and thermal energy Section 4.2: To discuss three methods of thermal energy transfer. Section 4.3: To describe
More informationMOLECULAR WEIGHT CALCULATIONS
MOLECULAR WEIGHT CALCULATIONS Calculating Formula Weight; Significant Figures Page 2 Percentage Composition of a Compound 18 Exponential Notation; Avogadro s Number; Moles 28 Calculating Empirical Formulas
More informationMeasurement of Length, Mass, Volume and Density
Measurement of Length, Mass, Volume and Density Experimental Objective The objective of this experiment is to acquaint you with basic scientific conventions for measuring physical quantities. You will
More informationChapter 4 Practice Quiz
Chapter 4 Practice Quiz 1. Label each box with the appropriate state of matter. A) I: Gas II: Liquid III: Solid B) I: Liquid II: Solid III: Gas C) I: Solid II: Liquid III: Gas D) I: Gas II: Solid III:
More informationREASONING AND SOLUTION
39. REASONING AND SOLUTION The heat released by the blood is given by Q cm T, in which the specific heat capacity c of the blood (water) is given in Table 12.2. Then Therefore, T Q cm 2000 J 0.8 C [4186
More informationTeenage Detectives. Aaron Jacobson Chemistry Teacher South High School Bakersfield 1101 Planz Road Bakersfield, CA 93304.
Teenage Detectives Bring the world of forensic investigation into your chemistry curriculum with the use of investigative labs and real world cases. What really happens in a crime lab? How do they obtain
More informationStoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
More informationThe Empirical Formula of a Compound
The Empirical Formula of a Compound Lab #5 Introduction A look at the mass relationships in chemistry reveals little order or sense. The ratio of the masses of the elements in a compound, while constant,
More informationThe Mole Notes. There are many ways to or measure things. In Chemistry we also have special ways to count and measure things, one of which is the.
The Mole Notes I. Introduction There are many ways to or measure things. In Chemistry we also have special ways to count and measure things, one of which is the. A. The Mole (mol) Recall that atoms of
More informationDensity Determinations and Various Methods to Measure
Density Determinations and Various Methods to Measure Volume GOAL AND OVERVIEW This lab provides an introduction to the concept and applications of density measurements. The densities of brass and aluminum
More informationINTERIM UNITS OF MEASURE As suggested by Federal Standard 376B January 27, 1993. hectare (ha) Hundred for traffic buttons.
SI  The Metrics International System of Units The International System of Units (SI) is a modernized version of the metric system established by international agreement. The metric system of measurement
More informationFlorida Math 0018. Correlation of the ALEKS course Florida Math 0018 to the Florida Mathematics Competencies  Lower
Florida Math 0018 Correlation of the ALEKS course Florida Math 0018 to the Florida Mathematics Competencies  Lower Whole Numbers MDECL1: Perform operations on whole numbers (with applications, including
More informationSection 1 Tools and Measurement
Section 1 Tools and Measurement Key Concept Scientists must select the appropriate tools to make measurements and collect data, to perform tests, and to analyze data. What You Will Learn Scientists use
More informationExp 13 Volumetric Analysis: AcidBase titration
Exp 13 Volumetric Analysis: AcidBase titration Exp. 13 video (time: 47:17 minutes) Titration  is the measurement of the volume of a standard solution required to completely react with a measured volume
More informationMOLES, MOLECULES, FORMULAS. Part I: What Is a Mole And Why Are Chemists Interested in It?
NAME PARTNERS SECTION DATE_ MOLES, MOLECULES, FORMULAS This activity is designed to introduce a convenient unit used by chemists and to illustrate uses of the unit. Part I: What Is a Mole And Why Are Chemists
More informationForms of Energy. Freshman Seminar
Forms of Energy Freshman Seminar Energy Energy The ability & capacity to do work Energy can take many different forms Energy can be quantified Law of Conservation of energy In any change from one form
More informationKey. Name: OBJECTIVES
Name: Key OBJECTIVES Correctly define: observation, inference, classification, percent deviation, density, rate of change, cyclic change, dynamic equilibrium, interface, mass, volume GRAPHICAL RELATIONSHIPS
More information4.5.1 The Metric System
4.5.1 The Metric System Learning Objective(s) 1 Describe the general relationship between the U.S. customary units and metric units of length, weight/mass, and volume. 2 Define the metric prefixes and
More information1. Metric system developed in Europe (France) in 1700's, offered as an alternative to the British or English system of measurement.
GS104 Basics Review of Math I. MATHEMATICS REVIEW A. Decimal Fractions, basics and definitions 1. Decimal Fractions  a fraction whose deonominator is 10 or some multiple of 10 such as 100, 1000, 10000,
More informationSession 29 Scientific Notation and Laws of Exponents. If you have ever taken a Chemistry class, you may have encountered the following numbers:
Session 9 Scientific Notation and Laws of Exponents If you have ever taken a Chemistry class, you may have encountered the following numbers: There are approximately 60,4,79,00,000,000,000,000 molecules
More information2014 Spring CHEM101 Ch12 Review Worksheet Modified by Dr. ChengYu Lai,
Ch1 1) Which of the following underlined items is not an intensive property? A) A chemical reaction requires 3.00 g of oxygen. B) The density of helium at 25 C is 1.64 104 g/cm3. C) The melting point
More informationChapter 5 Principles of Chemical Reactivity: Energy and Chemical Reactions
PRACTICING SKILLS Energy Chapter 5 Principles of Chemical Reactivity: 1. To move the lever, one uses mechanical energy. The energy resulting is manifest in electrical energy (which produces light); thermal
More informationExponents, Radicals, and Scientific Notation
General Exponent Rules: Exponents, Radicals, and Scientific Notation x m x n = x m+n Example 1: x 5 x = x 5+ = x 7 (x m ) n = x mn Example : (x 5 ) = x 5 = x 10 (x m y n ) p = x mp y np Example : (x) =
More informationWhat s in a Mole? Molar Mass
LESSON 10 What s in a Mole? Molar Mass OVERVIEW Key Ideas Lesson Type Lab: Groups of 4 Chemists compare moles of substances rather than masses because moles are a way of counting atoms. When considering
More informationMixing Warm and Cold Water
Mixing Warm and Cold Water A Continuing Investigation of Thermal Pollution By Kevin White 1 Context: This lesson is intended for students conducting an ongoing study of thermal pollution. Perhaps, students
More informationChemistry 112 Laboratory Experiment 6: The Reaction of Aluminum and Zinc with Hydrochloric Acid
Chemistry 112 Laboratory Experiment 6: The Reaction of Aluminum and Zinc with Hydrochloric Acid Introduction Many metals react with acids to form hydrogen gas. In this experiment, you will use the reactions
More informationNegative Integral Exponents. If x is nonzero, the reciprocal of x is written as 1 x. For example, the reciprocal of 23 is written as 2
4 (4) Chapter 4 Polynomials and Eponents P( r) 0 ( r) dollars. Which law of eponents can be used to simplify the last epression? Simplify it. P( r) 7. CD rollover. Ronnie invested P dollars in a year
More informationCHEMISTRY II FINAL EXAM REVIEW
Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationPhys222 W11 Quiz 1: Chapters 1921 Keys. Name:
Name:. In order for two objects to have the same temperature, they must a. be in thermal equilibrium.
More informationMeasurements 1. BIRKBECK MATHS SUPPORT www.mathsupport.wordpress.com. In this section we will look at. Helping you practice. Online Quizzes and Videos
BIRKBECK MATHS SUPPORT www.mathsupport.wordpress.com Measurements 1 In this section we will look at  Examples of everyday measurement  Some units we use to take measurements  Symbols for units and converting
More informationPS Chapter 1 Review. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A PS Chapter 1 Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The two main branches of science are a. physics and chemistry.
More informationMetric Mania Conversion Practice. Basic Unit. Overhead Copy. Kilo  1000 units. Hecto  100 units. Deka  10 units. Deci  0.
Metric Mania Conversion Practice Overhead Copy Kilo  1000 Hecto  100 Deka  10 To convert to a larger unit, move decimal point to the left or divide. Basic Unit Deci  0.1 To convert to a smaller unit,
More information$566.30. What is the monthly interest rate on the account? (Round to the nearest hundredth of a percent.) 4 = x 12. 7)
Exam Name SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 1)What percent of 6 is 27? 1) 2)64.288 is 28.7% of what number? 2) 3)112% of what number is
More informationA.2. Exponents and Radicals. Integer Exponents. What you should learn. Exponential Notation. Why you should learn it. Properties of Exponents
Appendix A. Exponents and Radicals A11 A. Exponents and Radicals What you should learn Use properties of exponents. Use scientific notation to represent real numbers. Use properties of radicals. Simplify
More information