Administratium morons peons isodopes Critical Mass

Transcription

1 Subject: new element A major research institution has recently announced the discovery of the heaviest element yet known to science. This new element has been tentatively named "Administratium". Administratium has I neutron, 12 assistant neutrons, 75 deputy neutrons, and III assistant deputy neutrons, giving it an atomic mass of 312. These 312 particles are held together by a force called "morons", which are surrounded by vast quantities of lepton-like particles called "peons". Since Administratium has no electrons, it is inert. However, it can easily be detected as it impedes every reaction with which it comes into contact. A minute amount of Administratium causes one reaction to take over 4 days to complete when it would normally take less than an hour. Administratium has a normal half-life of 3 years; it does not decay but instead undergoes a reorganization, in which a portion of the assistant neutrons and deputy neutrons and assistant deputy neutrons exchange places. In fact, Administratium's mass will actually increase over time, since each reorganization causes some morons to become neutrons forming "isodopes." This characteristic of moron-promotion leads some scientists to speculate that Administratium is formed whenever morons reach a certain quantity in concentration. This hypothetical quantity is referred to as "Critical Mass". You will know it when you see it. OFB Chapter 1 1

2 Chem 1310 Spring 2003 William J. Baron, Ph.D. GaTech School of Chemistry and Biochemistry Director of the Freshman Chemistry Program 1310, 1311, 1312, 1313 Office Boggs 1-59A (temporary) inside Main Chemistry office Boggs Office Chem Annex Room 47 preferred Phone Mailbox in Chemistry Office Lucent Technologies, Bell Laboratories (retired) Director, Optical Products Technology Norcross Fiber Optics, R&D, product design and development Director, Advanced Materials Development New Jersey Semiconductor crystals and devices Circuit board fabrication and assembly Ph.D. Princeton, Postdoctoral work at Ruhr Universität Bochum and Columbia Specialties: Physical Organic Chemistry, reaction mechanism, reactive intermediates, photochemistry, polymers OFB Chapter 1 2

3 Chem 1310 Spring 2003 Sections AB Course Objectives Semester Schedule (later slide) Problems, Exercises Exams Friday, January 24 Wednesday, February 12 Wednesday, March 19 Monday, April 14 Friday,,May 2 2:50 PM to 5:40 PM Room CoC 16) Grading Hour Exams 45% (5%. 10%, 15%, 15%) Final Exam 25% Homework 10% Laboratory 20% OFB Chapter 1 3

4 Chem 1310 Spring 2003 Sections AB Lectures MWF, 10:05-10:55 Will use ppt, suggest downloading lecture notes, print 1, 4, 6 per slide Recitations and Labs Recitations: (50 minutes) Wednesdays, either 1:05, 2:05, or 3:05 PM Labs: (2 hours 50 minutes) Tuesdays, either 12:05 or 3:05 Office Hours MWF following lecture in Chem Annex 47 office Or by appointment Study ask questions, memorization not the whole answer, study everyday, stay limber, can t cram OFB Chapter 1 4

5 Instructor Teaching Assistants Required Course materials Course Description Grading Policies Syllabus Homework Lecture Notes Exams Exam 1 old exams answer key Exam 2 Exam 3 Exam 4 Final Exam OFB Chapter 1 5

6 CHEM 1310 SECTION AB SPRING 2003 GENERAL CHEMISTRY Class Meetings Classes begin on Monday, January 6 and end on Friday April, 25. Holidays are Monday, January 20 (MLK Day), and Monday through Friday, March 3 to 7 (Mid- Semester Break). Lectures: Monday, Wednesday, and Friday, 10:05 10:55 Recitations: Wednesday, either 1:05 to 1:55, or 2:05 to 2:55, or 3:05 to 3:55 or 4:05 to 4:55. First meeting is January 8. Labs: Tuesday, either 12:05 to 2:55, or 3:05 to 5:55. First Lab meeting is Tuesday January 14. Instructor Dr. William J. Baron Office: 1-59A Boggs Bldg. (will be moving in early semester to Boggs 1-108) Phone: bill.baron@chemistry.gatech.edu Office Hours: Monday, Wednesday, and Friday, 11:00 12:00 in Chem Annex 47 or by appointment Teaching Assistants SECTION NAME LOCATION OFFICE HOURS A1 Tumpa Sarkar gtg532f@prism.gatech.edu A2 Berhane Temelso gte403f@prism.gatech.edu A3 Victoria Mariani gt7398b@prism.gatech.edu B1 Frankie Onyemauwa gtg512d@prism.gatech.edu B2 Kristin Shepperd gtg944j@prism.gatech.edu B3 Asmerom Hagos gt7130a@prism.gatech.edu Required Course Materials Lecture Text: Chemistry: Science of Change, 4 th Ed., by Oxtoby, Freeman, & Block. Lab Text: Laboratory Experiments for General Chemistry, 4 th Ed., by Hunt, Block, & McElvey

7 Other Materials (GT bookstore) Calculator (+, -, *, /, ln, and log) Key-controlled combination lock. Locks can be purchased at the bookstore (must be "chemistry locks"). Used locks may be purchased (at a discount price) from the stockroom in the Chem Annex. Safety glasses or goggles Lab Apron (recommended) NOTE: You should maintain a balance of at least $30 on your BuzzCard so that you can pay for any fees you might incur in lab (breaking glassware, renting safety goggles, etc). Payment will be made at the Annex stockroom. You will not be permitted to work in lab unless you are wearing safety glasses or goggles and closed shoes. Course Description The course covers fundamental observations, laws, and theories of chemistry at the introductory level. Topics include atoms/molecules, stoichiometry, acids/bases, solutions, equilibria, gases, solids, liquids, thermodynamics, electrochemistry, kinetics, quantum theory, the periodic table, and chemical bonding. Grading Policies Attendance: Recitation: Exams: Final Exam: Attendance is expected in lecture, required in laboratory and highly beneficial in recitation. Material on exams may be taken from assigned reading, homework, lecture material, or problems similar to those at the end of each chapter in the course text. The weekly recitation section is meant to give students a chance to ask questions and see sample problems worked. Each recitation section will be directed by a teaching assistant (TA) who is usually a chemistry graduate student. Four closed-book exams will be given during the semester. The exam dates are Friday, January 24, Wednesday February 23, Wednesday March 19, and Monday April 14, A three-hour final exam will be given at the time and place determined for this course by standard Georgia Tech procedures. The final exam for this course is tentatively scheduled for Friday, May 2 at 2:50 PM in Room 16 CHEM Annex. Homework: Homework problems will be assigned weekly and will be graded on a 0, 1, 2 basis. Many exam questions will be analogous to assigned homework problems, so working homework problems is an essential part of exam

8 preparation. Assigned homework problems are taken from the textbook. It is OK for students to collaborate on homework, but each student should turn in their own homework in their own writing. Homework will be collected each week during. Laboratory Grade: You must pass Laboratory to pass the overall course. Teaching Assistants will have the responsibility for establishing laboratory grades. Students are graded on pre-lab quizzes, formal lab reports, summary reports, report accuracy, lab technique and attitude, Lab Midterm exam, and Lab Final exam. A grade of 70% or better in the lab is considered passing. Grades between 60% and 65% will be considered, if documentation is provided for any extenuating circumstances. Grade Changes: Make-up Exams: Honor Code: Re-grades of hour exams must be requested within one week of the date that the graded exams are returned to students. Only re-grades that could add four or more points to the score will be considered. There will be no make-up exams. If a student has a valid excuse for missing an exam, his/her grade for that exam will be calculated from his/her performance on that part of the final exam that covers topics from the missed exam.. Students are expected to adhere to the Georgia Tech honor code during all aspects of this course (see for details). The basis for course grades will be as follows: Hour Exam 1 5% Hour Exam 2 10% Hour Exam 3 15% Hour Exam 4 15% Final Exam 25% Homework 10% Laboratory 20% Course Webpage Information of interest to students will be posted on the course webpage:

9 Students should consult the webpage at frequent intervals throughout the semester.

10 Dr. William J. Baron Department of Chemistry and Biochemistry Chem 1310 General Chemistry Sections A1-3, B1-3 MWF 10:05 to 10:55 Monday, Wednesday and Friday Course Schedule Recitation on Wednesdays College of Computing Room 16 Homework Assignments, due at Recitation Date Topic Reading Problems for Homework Monday, January 06, 2003 Course Introduction & OFB Chapter 1 Chapter 1 Wednesday, January 08, 2003 Lab Introduction (Dr. George McKelvy) Appendices A-C Meet TAs, discuss Labs, recitations, etc. Friday, January 10, 2003 The Atomic Nature of Matter Monday, January 13, 2003 Stoichiometry Chapter 2 Wednesday, January 15, 2003 OFB 1: # 9, 10, 11, 17, 19, 20, 29, 37, 38, 55, 68 Friday, January 17, 2003 Chemical Periodicity & Formation of Simple Compounds Chapter 3 Monday, January 20, 2003 Holiday Wednesday, January 22, 2003 OFB 2: # 2, 5, 33, 42, 43, 44, 81 Friday, January 24, 2003 Exam 1 (Chapters 1-3) Monday, January 27, 2003 Review & Types of Chemical Reactions Chapter 4 Wednesday, January 29, 2003 OFB 3:# 8, 9, 18, 34, 45, 57, 59, 60, 69, 70 Friday, January 31, 2003 Monday, February 03, 2003 The Gaseous State Chapter 5 Wednesday, February 05, 2003 OFB 4: # 1, 6, 12, 50, 54, 55, 59, 71 Friday, February 07, 2003 Condensed Phases and Phase Transitions Chapter 6 Monday, February 10, 2003 Wednesday, February 12, 2003 Exam 2 (Chapters 4-6) OFB 5: # 34, 38, 48, 62, 70, 81 Friday, February 14, 2003 Review & Chemical Equilibrium (Last Day to Drop) Chapter 7 Monday, February 17, 2003 Wednesday, February 19, 2003 OFB 6: # 4, 20, 26, 38, 44, 62 Friday, February 21, 2003 OFB Acid-Base Equilibria Chapter 8 Monday, February 24, 2003 Wednesday, February 26, 2003 OFB 7: # 1, 2, 7, 9, 12, 15, 18, 24, 31, 42, 45 Friday, February 28, 2003 Dissolution and Precipitations Equilibria (mid-term Grades Due) chapter 9 Monday, March 03, 2003 Break Wednesday, March 05, 2003 Break OFB 8: # 5, 9, 11, 12, 26, 31, 42, 43, 44, 46 Friday, March 07, 2003 Break Monday, March 10, 2003 Wednesday, March 12, 2003 Thermochemistry Chapter 10 OFB 9: # 16, 19, 23, 30, 39, 41, 42, 51, 52, 54 Friday, March 14, 2003 Monday, March 17, 2003 Wednesday, March 19, 2003 Exam 3 (Chapters 7-10) OFB 10: # 11,13,19, 23,33,37,40, 43,49,53,59,63 Friday, March 21, 2003 Review & Spontaneous Change and Equilibrium Chapter 11 Monday, March 24, 2003 Wednesday, March 26, 2003 OFB 11: # 13, 15, 23, 29, 31, 37, 39, 43, 49, 53, 57, 63, 69 Friday, March 28, 2003 Redox reactions and Electrochemistry Chapter 12 Monday, March 31, 2003 Wednesday, April 02, 2003 Electrochemistry and Cell Voltage Chapter 13 OFB 12: # 1, 3, 7,9, 11, 13, 29, 31, 33 Friday, April 04, 2003 Monday, April 07, 2003 Chemical Kinetics Chapter 14 Wednesday, April 09, 2003 OFB 13: # 3, 5, 9, 11, 15, 19, 29, 31, 35, 37, 41, 45 Friday, April 11, 2003 Monday, April 14, 2003 Exam 4 (Chapters 11-14) Wednesday, April 16, 2003 Review & Quantum Mechanics & The Hydrogen Atom Chapter 16 (note skip OFB 15) OFB 14: # 7, 9, 11, 15, 19, 21, 23, 25, 37, 41, 43, 45, 51, 53 Friday, April 18, 2003 Monday, April 21, 2003 Wednesday, April 23, 2003 Many-Electron Atoms and chemical Bonding Chapter 17 OFB 16: # 14, 16, 22, 28, 34, 41 Friday, April 25, 2003 Friday, May 02, 2003 Tentative Final 2:50 PM to 5:40 PM OFB 17 don t turn in: # 1, 3, 5, 7 Monday, May 05, 2003 All grades due to Registrar's Office by 12 noon Phone: bill.baron@chemistry.gatech.edu Office Boggs Mailbox in Chemistry Department Main Office

11 CHEM 1310 SECTION AB Spring 2003 GENERAL CHEMISTRY Homework Problems (to be turned in at Recitation) December 17, 2002 update Chapter Problems Due Date 1 9, 10, 11, 17, 19, 20, 29, 37, 38, 55, 68 Jan , 5, 33, 42, 43, 44, 81 Jan , 9, 18, 34, 45, 57, 59, 60, 69, 70 Jan , 6, 12, 50, 54, 55, 59, 71 Feb , 38, 48, 62, 70, 81 Feb , 20, 26, 38, 44, 62 Feb , 2, 7, 9, 12, 15, 18, 24, 31, 42, 45 Feb , 9, 11, 12, 26, 31, 42, 43, 44, 46 Mar , 19, 23, 30, 39, 41, 42, 51, 52, 54 Mar ,13,19, 23,33,37,40, 43,49,53,59,63 Mar , 15, 23, 29, 31, 37, 39, 43, 49, 53, 57, 63, 69 Mar , 3, 7,9, 11, 13, 29, 31, 33 Apr , 5, 9, 11, 15, 19, 29, 31, 35, 37, 41, 45 Apr , 9, 11, 15, 19, 21, 23, 25, 37, 41, 43, 45, 51, 53 Apr , 16, 22, 28, 34, 41 Apr , 3, 5, 7 don t turn in

12 Spring 2003 Tutorial Room Place: Chem Annex Room 50 Days: Tuesday, Wednesday, Thursday Hours: 12 Noon to 2:00 PM

13 Reading OFB Chapter 1 Appendices A, B, and C Read, Read, Read Work Problems, Work Problems, Work Problems OFB Chapter 1 6

14 Chapter 1 The Atomic Nature of Matter 1-1 Chemistry: Science of Change 1-2 The Composition of Matter 1-3 The Atomic Theory of Matter 1-4 Chemical Formulas and Relative Atomic Masses 1-5 The Building Blocks of the Atom 1-6 Finding Atomic Masses the Modern Way 1-7 The Mole Concept: Counting and Weighing Atoms and Molecules 1-8 Finding Empirical and Molecular Formulas the Modern Way 1-9 Volume and Density OFB Chapter 1 7

15 Definitions Analysis (Take things apart) Synthesis (Put things together) Physical Properties (Color, odor, taste, boiling point, etc.) Chemical properties (with respect to other materials, e.g., uniformity) Substance (refer to elements and compounds, never mixtures) Elements (cannot be decomposed into simpler substances) Compounds (contain two or more elements bonded together, e.g., NaCl) Molecule (a few atoms connected together, e.g., CO 2 ) Mixtures (can be separated into two or more substances) Homogenous (uniform throughout, solutions) Heterogeneous (properties vary from region to region) Phase (liquid, gas, solid) OFB Chapter 1 8

16 Examples Table Salt Heterogeneous (mixture of NaCl and small amounts of other substances) Wood Heterogeneous (mixture of tree cells, and thousands of other substances) Mercury A substance and an element Air Homogenous mixture of gases Also a Heterogeneous mixture of gases and dust Water A substance that is a compound with molecular formula H 2 O What is an example of a homogenous sample that would gradually become heterogeneous if left to itself? E.g., A solution of sugar in water 1 st Homogeneous 2 nd allow evaporation to start, becomes heterogeneous 3 rd, complete evaporation, becomes homogeneous OFB Chapter 1 9

17 Atomic Theory of Matter Law of conservation of mass: Mass is neither created nor destroyed in a chemical reaction Dalton s Atomic Theory of Matter (1808): 1. All matter consists of solid and indivisible atoms 2. All atoms of a given chemical element are identical in mass and in all other properties 3. Different elements have different kinds of atoms; these atoms differ in mass from element to element 4. Atoms are indestructible and retain their identity in all chemical reactions 5. The formation of a compound from its elements occurs through the combination of atoms of unlike elements in small whole-number ratio. OFB Chapter 1 10

18 Chemical Formulas and Relative Atomic Masses Chemical Formulas display symbols for the elements and the relative number of atoms E.g., NH 3, CO 2, CH 3 CO 2 H or C 2 H 4 O 2 Molecules are groupings of two or more atoms bound closely together by strong forces that maintain them in a persistent combination OFB Chapter 1 11

19 Exercise 1-1 Problem: Every g of the compound SiH 4 contains g of Si and g of H. Find the ratio of the atomic mass of S to the atomic mass of H. Strategy: 1. Take the ratio of S/H 2. Account for the 1:4 ratio of S:H OFB Chapter 1 12

20 Exercise 1-1 Problem: Every g of the compound SiH 4 contains g of Si and g of H. Find the ratio of the atomic mass of S to the atomic mass of H Solution: OFB Chapter 1 13

21 Building Blocks of the Atom Electrons, Protons and Neutrons Electrons discovered in 1897 by Thomson Rutherford proposed that the atomic nucleus was composed of neutral particles called Neutrons and positively charged particles called protons Neutron number = N Atomic number = Z = number of Protons Atomic mass number = A A = Z + N OFB Chapter 1 14

22 OFB Chapter 1 15

23 C Carbon N Nitrogen Si Silicon P Phosphorus OFB Chapter 1 16

24 Atomic Mass C Carbon Atomic Number A = Z + N Atomic Mass = # Protons + # Neutrons For Carbon, 12 = 6 + Neutrons Neutrons = 6 Every Carbon atom has 6 electrons, 6 protons and 6 neutrons OFB Chapter 1 17

25 Mass Spectrometry and Isotopes Mass Spectrometer accelerates ions (or molecular ions) in an electric field and then separates those ions by relative mass in a magnetic field Cl Chlorine Mass Spectrometer Separation of Chlorine Relative Amount Relative Mass OFB Chapter 1 18

26 Atoms Avogadro s Number is the number of 12 C atoms in exactly 12 grams of carbon N 0 = X The mass, in grams, of Avogadro's number of atoms of an element is numerically equal to the relative atomic mass of that element OFB Chapter 1 19

27 Molecules Relative Molecular Mass of a molecule equals the sum of the relative atomic masses of all of the atoms making up the molecule OFB Chapter 1 20

28 Moles A mole measures the chemical amount of a substance Mole is an abbreviation of gram molecular weight One mole of a substance equals the amount that contains Avogadro's number of atoms, molecules. One mole = Molar mass (M) of that element or molecule OFB Chapter 1 21

29 Exercise 1-6 Molecules of isoamyl acetate have the formula C 7 H 14 O 2. Calculate (a) how many moles and (b) how many molecules are present in 0.250g of isoamyl acetate. Strategy: 1. Calculate molar mass of C 7 H 14 O 2 2. Calculate the number of moles in grams 3. Using Avogadro s number to calculate the number of molecules in X moles of C 7 H 14 O 2 OFB Chapter 1 22

30 Exercise 1-6 Molecules of isoamyl acetate have the formula C 7 H 14 O 2. Calculate (a) how many moles and (b) how many molecules are present in 0.250g of isoamyl acetate. Solution: 1. Calculate molar mass of C 7 H 14 O 2 2. Calculate the number of moles in grams 3. Using Avogadro s number calculate the number of molecules in X moles of C 7 H 14 O 2 OFB Chapter 1 23

31 Percentage Composition from Empirical or Molecular Formula Exercise 1-8 Tetrodotoxin, a potent poison found in the ovaries and liver of the globefish, has the empirical formula C 11 H 17 N 3 O 8. Calculate the mass percentages of the four element in this compound. Strategy: 1. Calculate molar mass of C 11 H 17 N 3 O, by finding the mass contributed by each element 2. Divide the mass for each element by the total mass of the compound. OFB Chapter 1 24

32 Exercise 1-8 Tetrodotoxin has the empirical formula C 11 H 17 N 3 O 8. Calculate the mass percentages of the four element in this compound. Solution: 1. Calculate molar mass of C 11 H 17 N 3 O, by finding the mass contributed by each element 2. Divide the mass for each element by the total mass of the compound. OFB Chapter 1 25

33 Finding an Empirical Formula Exercise 1-9 Heating a 150.0mg dose of a compound used to treat rheumatism decomposes it to its constituent elements, which are separated. There are mg of gold, mg of sodium, mg of oxygen, and mg of sulfur. Determine the empirical formula of this compound. Strategy: 1. Calculate the chemical amount (in moles) of each element in the sample using the table of atomic masses. 2. Find the ratios of the moles for each element by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 26

34 Exercise 1-9 Heating a 150.0mg dose of a compound used to treat rheumatism decomposes it to its constituent elements, which are separated. There are mg of gold, mg of sodium, mg of oxygen, and mg of sulfur. Determine the empirical formula of this compound. Solution: 1. Calculate the chemical amount (in moles) of each element in the sample using the table of atomic masses. 2. Find the ratios of the moles for each element by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 27

35 Exercise 1-9 Determine the empirical formula of this compound. Solution: 1. Calculate the chemical amount (in moles) of each element in the sample using the table of atomic masses. 2. Find the ratios of the moles for each element by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 28

36 Exercise 1-10 Moderate Heating of mg of a compound containing nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves mg of metallic nickel behind. Determine the empirical formula of the compound. Strategy: 1. Write the reaction 2. Use the conservation of mass to find the amount of CO 3. Find the number of moles of CO and Nickel 4. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. OFB Chapter 1 29

37 Exercise 1-10 Moderate Heating of mg of a compound containing nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves mg of metallic nickel behind. Determine the empirical formula of the compound. Solution: 1. Write the reaction 2. Use the law of conservation of mass to find the amount of CO 3. Find the number of moles of CO and Nickel 4. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. OFB Chapter 1 30

38 Exercise 1-10 Moderate Heating of mg of a compound containing nickel, carbon and oxygen and no other elements drives off all of the carbon and oxygen in the form of carbon monoxide (CO) and leaves mg of metallic nickel behind. Determine the empirical formula of the compound. Solution: 1. Write the reaction 2. Use the law of conservation of mass to find the amount of CO 3. Find the number of moles of CO and Nickel 4. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. OFB Chapter 1 31

39 Combustion Analysis Exercise 1-11 A sample of a liquid hydrocarbon weighing mg is burned in a combustion train to give mg of carbon dioxide, mg of water and no other products. What is the empirical formula of this hydrocarbon? Strategy: 1. Calculate the chemical amount (in moles) of carbon dioxide and water using the table of atomic masses. 2. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 32

40 Exercise 1-11 A sample of a liquid hydrocarbon weighing mg is burned in a combustion train to give mg of carbon dioxide, mg of water and no other products. What is the empirical formula of this hydrocarbon? Solution: 1. Calculate the chemical amount (in moles) of carbon dioxide and water using the table of atomic masses. 2. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 33

41 Exercise 1-11 Solution: 1. Calculate the chemical amount (in moles) of carbon dioxide and water using the table of atomic masses. 2. Find the ratios of the moles for each substance by dividing each by the smallest one, i.e., normalize to the smallest. 3. If necessary, multiply smallest factor that clears any fractions that they contain. OFB Chapter 1 34

42 Volume and Density Exercise 1-13 The density of liquid mercury at 20 deg C is g cm -3. A chemical reaction requires mol of mercury. What volume (in cubic centimeters) of mercury should be measured out at 20 C? Strategy: 1. Use density and mass to find volume. Rearrange m m d = V = V d 2. Density is given, can find mass from the number of moles of mercury which is given 3. Solve for volume. OFB Chapter 1 35

43 Exercise 1-13 The density of liquid mercury at 20 deg C is g cm -3. A chemical reaction requires mol of mercury. What volume (in cubic centimeters) of mercury should be measured out at 20 C? Solution: 1. Use density and mass to find volume. m V = d 2. Density is given, can find mass from the number of moles of mercury which is given 3. Solve for volume. OFB Chapter 1 36

44 Chapter 1 The Atomic Nature of Matter Examples / Exercises All (1-1 thru 1-13) Problems 9, 10, 11, 17, 19, 20, 29, 37, 38, 55, 68 OFB Chapter 1 37