Warm-up. If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors)

Size: px
Start display at page:

Download "Warm-up. If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors)"

Transcription

1 Warm-up If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors) 1

2 THE MOLE 2

3 Measuring Matter How do chemists determine amounts of chemicals that react? C + O 2 CO 2 How much oxygen will react with 200. g of C? 3

4 Measuring Matter C + O 2 CO 2 1 atom of C 1 molecule of O 2 Atoms and molecules react particle-by-particle, not by mass. THUS: need to count particles!! 4

5 Counting GEDANKEN: How would you count a pail of pennies or a beaker of beans? 5

6 Counting by Mass Recycling centers do it all the time! If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? 150 kg 1 x 1000 g kg 1can x = 7500 cans 20 g 6

7 The Mole Chemists count atoms & molecules using the mole. 1 mole = 6.02 x particles = Avogadro s number 7

8 Where did Avogadro stay when he was on vacation? A Mole-tel 8

9 9

10 The Mole 1 mole = 6.02 x particles mole = # grains of sand on all the earth s beaches! 10

11 The Mole: Chemists Dozen The mole is a number, just like dozen is a number 11

12 The Mole Why use such a huge number for counting atoms and molecules? What does a mole look like? Sulfur Lead Water 12

13 The Mole Abbreviation? mol 1 mole = 6.02 x particles particle atom ion molecule atom ion mlc formula unit 13 fu

14 Representative Particle Substance Particle atomic nitrogen atom N nitrogen (gas) molecule N 2 water molecule H 2 O sodium ion ion Na + calcium fluoride formula unit CaF 2 14

15 1 mole = 6.02 x particles The Mole I ll do 2 problems. 1. How many molecules in 1.14 mol SO 3? 2. How many moles in 1.86 x mlc SO 3? 15

16 Calculating Atoms Some problems have an extra step, requiring the number of atoms in one molecule. Example: In one molecule of H 2 O, there are three atoms, one O and 2H. 1 mlc H 2 O = 3 atoms = 1 atom O = 2 atom H 16

17 Calculating Atoms How many atoms are in 1.52 mol H 2 O? 1.52 mol 1 x 6.02x1023 mlc 1 mol x 3 atom 1 mlc = 2.75 x atom 17

18 Gram Atomic Mass (GAM) GAM = atomic mass expressed in grams rather than atomic mass units (u). Atomic mass of carbon is u so, GAM of carbon = g 18

19 Gram Atomic Mass How many atoms are there in one GAM of C? Recall: 1 u = 1.66 x g 12.0 g C 1 1 u x 1.66 x g x 1 atom C 12.0 u = 6.02 x atoms C Try it for a GAM of sulfur. 19

20 Gram Atomic Mass How many atoms are there in 1 GAM of any element? (count by mass) 20

21 The Mole Carbon: 1 mole = 12.0 g = 6.02 x atom Iron: 1 mole = 55.8 g = 6.02 x atom 21

22 Be Careful with Units The mass of one carbon atom is 12.0 u (atomic mass units) 1 atom =12.0 u 1 mole = 12.0 g The mass of one mole of carbon atoms is 12.0 g. 22

23 Compounds What is the mass of one mole of a compound? Just add up the GAM s of the atoms. Let s use H 2 O as an example. 23

24 GMM of Water: H 2 O H O + H + H = O 16.0 g g g = 18.0 g per mol gram molecular mass H 24

25 Gram Molecular Mass Thus for water 1 mole = 18.0 g = 6.02 x molecules 25

26 Gram Molecular Mass Calculate the GMM for: N 2 O 5 26

27 What about Ionic Compounds? Calculate the GFM for: (gram formula mass) (NH 4 ) 2 SO 4 27

28 Terms GAM GMM Molar Mass GFM (the mass of one mole) 28

29 Conversion Factors particle 6.02 x10 23 part. = 1 mol mole mass molar mass (g) = 1 mol look it up 29

30 Sample Problems 1. How many molecules are in 3.0 moles of CO 2? 2. How many moles is 81 g of H 2 O? 30

31 Molar Volume of a Gas Unlike solids and liquids, the volume of 1 mole of any gas at STP is 22.4 L. STP on Table A 1 mol = 22.4 L (gas at STP) (see box) 31

32 Molar Volume of a Gas 1 mol = 22.4 L (gas at STP) How many moles are there in 6.2 L of NO 2 at STP? 32

33 Gas Density (Gas density measured in g/l) The density of an unknown gas is 2.87 g/l at STP. What is its molar mass? 2.87 g L x 22.4 L mol 64.3 = mol g 33

34 Gas Density Try it: What is the density of krypton gas at STP? 34

35 Mole Road Map particle 6.02 x10 23 part. = 1 mol mole volume 22.4 L = 1 mol (Gas at STP) mass molar mass (g) = 1 mol look it up 35

36 I ll do one, then it s your turn! 36

37 Chemical Formula Subscripts H 2 O 2 atoms 1 atom Ratio of 2 atoms H to 1 atom O = 20 atoms H to 10 atoms O = 2 mol H to 1 mol O Always a ratio of 2:1 Not a ratio of masses! 37

38 Empirical Formulas Lowest whole number ratio of atoms in a compound. Molec. Form. Empirical Form. H 2 O H 2 O N 2 H 4 NH 2 And all ionic compounds 38

39 Percent Composition (means % by mass of each element in a compound) What is the % (by mass) of each element in carbon dioxide (CO 2 )? First determine molar mass: C: 1 x 12.0 g = 12.0 g O: 2 x 16.0 g = 32.0 g total = 44.0 g per mol 39

40 Percent Composition CO 2 Then determine % composition: 12g %C = x 100% = 27% C 44g %O = x 100% = 73% O 32g 44g 40

41 Percent Composition 1. What is the % nitrogen in ammonium chloride? 2. What is the mass of nitrogen in 152 g of ammonium chloride? 41

42 Chemical Formulas Can be determined from the percent composition of each element in the compound. What is the formula of a compound with 25.9% N and 74.1% O? 42

43 Solve: 25.9% N and 74.1% O Assume 100 g of compound thus 25.9 g N and 74.1 g O The chemical formula is NOT: N 25.9 O 74.1 Percents or masses are not subscripts. 43

44 Chemical Formula Must find the ratio of moles 1 mol 25.9 g N x = 1.85 mol N 14.0 g 74.1 g O x 1 mol = 4.63 mol O 16.0 g 44

45 Chemical Formula N: 25.9 % O: 74.1 % 25.9 g 74.1 g 1.85 mol 4.63 mol N 1.85 O N 1 O 2.5 N 2 O 5 45

46 Chemical Formula You Try It! What is the formula of a compound that is 36% calcium and 64% chlorine? 46

47 Empirical Formula Actually, the formula you get using % composition is an empirical formula, not a molecular formula. Prove it to yourself: a. What is the percent composition of C 2 H 8 N 2? b. Given your answer in part a, calculate the chemical formula. 47

48 How to Get Molecular Formula Molecular formula was C 2 H 8 N 2 Empirical formula was CH 4 N What one more piece of information is needed to know the molecular formula is C 2 H 8 N 2? Molar mass of the compound! 48

49 Molecular Formula Can be determined from empirical formula and molar mass. What is molecular formula of a compound with empirical formula of CH 4 N and molar mass of 60 g? 49

50 Molecular Formula Empirical Mass of CH 4 N: C: 1 x 12.0 = 12.0g H: 4 x 1.0 = 4.0 g N: 1 x 14.0 = 14.0 g total = 30.0 g vs. molar mass of 60 g. Off by factor of 2. compare Thus molecular formula = C 2 H 8 N 2 50

51 You Try One! What is the empirical formula of a compound that is 71.4% Br and 28.6% O? What is its molecular formula if this compound has a molar mass of 224g? 51

52 Summary of Calculations 1. Road Map (let units help!) (diagram in problem set) 1 mol = 6.02 x particles 1 mol = molar mass (g) 1 mol = 22.4 L (gas at STP) 52

53 Summary of Calculations 2. % Composition (by mass): start with formula molar mass calc. divide mass of each element by molar mass (x 100) 53

54 Summary of Calculations 3. Empirical Formula: start with % comp. change % sign to grams convert grams to moles moles as subscripts divide by smallest number 54

55 Summary of Calculations 4. Molecular Formula: divide molar mass by empirical formula molar mass multiply all subscripts by this result 55

56 Hocus pocus Abracadabra I command my homework to do itself. BE DONE! Flip aaflip aaaaaflip Rats 56

57 57

58 Warm-up What is Avogadro s number? What is it used for? 58

59 Warm-up What is Avogadro s number? How many moles is 6.78 x molecules of carbon dioxide? 59

60 Warm-up How many iron atoms are there in one GAM of iron? 60

61 Warm-up What did Avogadro put on tacos? How many oxygen atoms are in 3.5 mol sodium carbonate? What is GFM of sodium carbonate? How many formula units are in 0.51g of sodium carbonate? (use the map in the problem set) 61

62 Warm-up How many moles are 4.2E25 fu of sodium carbonate? How many oxygen atoms are in 3.5 mol sodium carbonate? 62

63 Warm-up How many moles of CO are x molecules of CO? 2 What is GMM of N O? 2 What did Avogadro put on tacos? 63

64 Warm-up What is GMM of N 2 O? What is GFM of aluminum sulfate? 64

65 Warm-up How many molecules are in L of carbon dioxide? What is the percent of oxygen in sulfuric acid? Honors: What is the density of Xenon gas at STP? 65

66 Warm-up How many molecules are in L of carbon dioxide? What is the volume of 27.8 g of carbon dioxide at STP? What is the percent of oxygen in sulfuric acid? 66

67 Warm-up You are at Burger King with a friend. She picks up a 0.51g salt packet for her fries and asks What is this stuff and how many thingies are in this packet? What is your answer? Of course you know thingies are formula units since NaCl is an ionic compound. 67

68 Warm-up You are at Burger King with a friend. She picks up a 0.51g salt packet for her fries and asks What is this stuff and how many thingies are in this packet? What is your answer? What is the volume (@STP) of 8.43 x molecules of SO 2? 68

69 Warm-up What is the volume of 18.5 g of SO 2 at STP? What is the percent of oxygen in barium hydroxide? What is the formula of a compound that is 27.3% carbon & 72.7% oxygen? 69

70 Warm-up How many grams is 9.3 x fu of calcium nitrate? What is the percent of copper in copper(i) oxide? A compound is 87.5% N and 12.5% H. What is its empirical formula? 70

71 Warm-up How many grams is 9.3 x fu of calcium nitrate? A compound is 87.5% N and 12.5% H. What is its empirical formula? If its molar mass is 64 g/mol, what is its molecular formula? 71

72 Warm-up In a lab experiment, it is found that 0.22 g S reacts with 0.33 g O. What is the mole ratio of oxygen to sulfur? What is the empirical formula of the compound that formed? 72

73 Lab 9 Empirical Formula Empty crucible g Crucible + Mg g Crucible + Mg + O g 1. mass Mg 3. mass O Conversion factors 2. mass Mg mol Mg 4. mass O mol O use 2 sig figs (0.022 mol) 5. Then ratio of mol Mg to mol O 73

74 Warm-up A compound is 87.5% N and 12.5% H. What is its empirical formula? If its molar mass is 32 g/mol, what is its molecular formula? What is the % composition of H 2 O? 74

How do you measure matter?

How do you measure matter? How do you measure matter? You may count how many you have. Determine a substances mass and weight. Determine a substances volume. But how can you relate these three types of measurements to one another?

More information

6.02 x 1023 CHAPTER 10. Mole. Avogadro s Number. Chemical Quantities The Mole: A Measurement of Matter Matter is measured in one of three ways:

6.02 x 1023 CHAPTER 10. Mole. Avogadro s Number. Chemical Quantities The Mole: A Measurement of Matter Matter is measured in one of three ways: Chapter 10 Notes CHAPTER 10 10.1 The Mole: A Measurement of Matter Matter is measured in one of three ways: Chemical Quantities Mole SI unit that measures the amount of a substance A mole of a substance

More information

What is a Representative Particle

What is a Representative Particle Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What

More information

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas In Chemistry, a Mole is: the unit that measures the amount of a substance - equals 6.022 x 10 23 particles of

More information

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole

More information

Chapter 10. How you measure how much? Moles. Representative particles. Conversion factors. Chemical Quantities or

Chapter 10. How you measure how much? Moles. Representative particles. Conversion factors. Chemical Quantities or Chapter 10 Chemical Quantities or 1 2 How you measure how much? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters. We count pieces in MOLES.

More information

HW 3 15 Hydrates Notes IC Hydrates HW 4 Water in a Hydrate IC/HW Unit 8 Test Review HW 5 X Unit 8 Test In class on 2/13 and 2/14

HW 3 15 Hydrates Notes IC Hydrates HW 4 Water in a Hydrate IC/HW Unit 8 Test Review HW 5 X Unit 8 Test In class on 2/13 and 2/14 Name: Unit 8- The Mole Day Page # Description IC/HW Due Date Completed All 2 Warm-up IC 1 3 4 Notes on the Mole IC 1 5 7 The Mole IC 1 8 9 Chemical Quantities HW 2 10 Percent Composition Notes IC X 2 Gum

More information

Notes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl -

Notes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl - Name I. Essential Terminology Notes: The Mole Period Chemistry Pre-AP The smallest particle of an element is the atom. Diatomic elements (like O 2 ) are the main exception to this. We say that diatomic

More information

Molar Mass. The total of the atomic masses of all the atoms in a molecule:

Molar Mass. The total of the atomic masses of all the atoms in a molecule: Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu

More information

The Mole. Chemical Quantities

The Mole. Chemical Quantities The Mole Chemical Quantities How Much vs What Is It? Quantitative Analysis -gives answers in a numerical form tells exactly how much Qualitative Analysisgives answers about a compounds without using numbers

More information

Honors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?

Honors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula

More information

Warm-Up. If I weigh 200 pounds, how many pounds of oxygen make up my body? How much hydrogen?

Warm-Up. If I weigh 200 pounds, how many pounds of oxygen make up my body? How much hydrogen? Warm-Up What are the percentage compositions (by mass) of the following elements in the human body? 1. Oxygen 2. Carbon 3. Hydrogen 4. Nitrogen 5. Calcium (65%) (18%) (10%) (3%) (1.5%) If I weigh 200 pounds,

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

Unit 6: Mole Assignment Packet Period:

Unit 6: Mole Assignment Packet Period: Unit 6: Mole Assignment Packet Name: Period: A1: Mole Conversions 1. Identify the representative particle in each of the following: (atom, molecule, formula unit) a. CuSO 4 b. H 2 O c. NaCl d. Zn e. Cu

More information

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction.

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction. Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting

More information

Unit III: Quantitative Composition of Compounds

Unit III: Quantitative Composition of Compounds Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using

More information

Stoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction.

Stoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction. Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting

More information

6.02 X Memorize this Number

6.02 X Memorize this Number Honors Chemistry - Unit 6 Chapters 3 & 7 The Mole Math with Chemical Formulas Voc. Assignment Due: Quiz Date(s): TBA Problem Set (UT Quest) Due: Test Date: Unit 6 Packet - Page 1 of 14 **VOCABULARY Assignment**

More information

7 Quantitative Composition of Compounds. Chapter Outline. The Mole. Slide 1. Slide 2. Slide 3

7 Quantitative Composition of Compounds. Chapter Outline. The Mole. Slide 1. Slide 2. Slide 3 1 7 Quantitative Composition of Compounds Black pearls are composed of calcium carbonate, CaCO 3. The pearls can be measured by either weighing or counting. Foundations of College Chemistry, 14 th Ed.

More information

Chem RG Chapter Packet 7 Mole & Chemical Composition. Assign Section # Name Ch 07 Test Review (turn in separately for graded points

Chem RG Chapter Packet 7 Mole & Chemical Composition. Assign Section # Name Ch 07 Test Review (turn in separately for graded points Name Period. Chem RG Chapter Packet 7 Mole & Chemical Composition Assign Section # Name 10 5 1. Assignment Sheet printed 2. Notes 7.1 3. Notes 7.2 4. Notes 7.3 5. 7.1 Chapter 7 WS #1 6. 7.2 Chapter 7 WS

More information

B. stoichiometry using balanced chemical equations to obtain info. C. mole-to-r.p. and r.p.-to-mole example problems:

B. stoichiometry using balanced chemical equations to obtain info. C. mole-to-r.p. and r.p.-to-mole example problems: Chem. Ch. 10 ~ THE MOLE NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 10.1 Notes I. Measuring Matter A. SI unit of chemical quantity = the mole (abbreviated

More information

Chapter 3. Stoichiometry

Chapter 3. Stoichiometry Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average

More information

What is a Mole? An Animal or What?

What is a Mole? An Animal or What? Unit 7: (Chapter 9) Chemical Quantities What is a Mole? An Animal or What? Section 9.1 The Mole: A Measurement of Matter Describe how Avogadro s number is related to a mole of any substance. Calculate

More information

PERCENTAGE COMPOSITION

PERCENTAGE COMPOSITION PERCENTAGE COMPOSITION Just like any percentage problems you are comparing the part to the whole. In chemistry, percentage composition is based on mass, not on numbers of atoms present. For Example, if

More information

1. Mole Definition & Background

1. Mole Definition & Background Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1 1. Mole Definition & Background The mole was developed

More information

CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units

CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units CHAPTER 11 The Mole 11.1 The Mole: Measurement of Matter Matter is measured in one of three ways: (How many?) Mole SI unit that measures the amount of a substance 6.02 x 10 particles of that substance.

More information

Stoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction.

Stoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction. Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting

More information

Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas

Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas Composition Stoichiometry Composition Stoichiometry NOTES 1 So far, we ve studied the products of a chemical reaction in terms of their identity. Stoichiometry is a branch of chemistry dealing with quantities.

More information

All Roads Lead to the Mole

All Roads Lead to the Mole CHEMICAL QUANTITIES Chemical Quantities Dozen: Baker as Mole: Chemist Measuring doughnuts: o 1 dozen = 1 doughnuts (count) o 1 dozen = 500 g doughnuts (mass) o 1 dozen = 1 box doughnuts (volume) All Roads

More information

CHAPTER 6 CHEMICAL COMPOSITION

CHAPTER 6 CHEMICAL COMPOSITION Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 6 CHEMICAL COMPOSITION Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.

7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation

More information

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular

More information

Please understand that you will NOT receive another copy of this packet! Name:

Please understand that you will NOT receive another copy of this packet! Name: Mole Unit Packet Please understand that you will NOT receive another copy of this packet! Name: Period: Introduction to The unit of the Mole is the HEART of all chemistry and most of its calculations.

More information

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate

More information

Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom.

Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom. Average Atomic Mass Since atoms are so small and the mass of individual atoms is also very small, it is not useful to use the units of grams or kilogram. A new unit called the atomic mass unit (amu) was

More information

Do Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet

Do Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet Do Now Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet All the math Molar Mass the mass of one mole of any substance, reported in grams (gram atomic mass)

More information

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction.

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction. Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting

More information

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction.

Stoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction. Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting

More information

Stoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)

Stoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules) Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number

More information

Percent Composition, Empirical Formula, Molecular Formula, Hydrates

Percent Composition, Empirical Formula, Molecular Formula, Hydrates Name: Percent Composition, Empirical Formula, Molecular Formula, Hydrates Essential Questions How can one explain the structure, properties, and interactions of matter? How do substances combine or react

More information

Unit III: Quantitative Composition of Compounds

Unit III: Quantitative Composition of Compounds Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using

More information

Unit 5. Chemical Composition

Unit 5. Chemical Composition Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles

More information

Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.

Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated

More information

1. Mole Definition & Background

1. Mole Definition & Background Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1 1. Mole Definition & Background The mole was developed

More information

Part 01 - Notes: The Mole and Its Calculations

Part 01 - Notes: The Mole and Its Calculations Part 01 - Notes: The Mole and Its Calculations Objectives: Identify, define, and explain: mole, Avogadro s number, representative particle, gram atomic mass, gram molecular mass, gram formula mass, molar

More information

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter OBJECTIVES: Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance.

More information

Notes on Mole 12.notebook. October 25, CaS. Ca + S. Oct 14 6:22 PM. Oct 14 6:23 PM. Oct 14 6:24 PM. Oct 14 6:23 PM MOLE.

Notes on Mole 12.notebook. October 25, CaS. Ca + S. Oct 14 6:22 PM. Oct 14 6:23 PM. Oct 14 6:24 PM. Oct 14 6:23 PM MOLE. How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the mole,

More information

Atoms, Molecules, and the Mole

Atoms, Molecules, and the Mole The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting

More information

7 Quan'ta've Composi'on of Compounds. Chapter Outline. The Mole. The Mole. The Mole. The Mole. Advanced Chemistry

7 Quan'ta've Composi'on of Compounds. Chapter Outline. The Mole. The Mole. The Mole. The Mole. Advanced Chemistry 7 Quan'ta've Composi'on of Compounds Chapter Outline 7.1 The Mole 7.2 7.3 Percent Composition of Compounds 7.4 Calculating Empirical Formulas 7.5 Calculating the Molecular Formula from Black pearls are

More information

1. Mole Definition & Background

1. Mole Definition & Background Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1. Mole Definition & Background The mole was developed

More information

Molar Calculations - Lecture Notes for Chapter 6. Lecture Notes Chapter Introduction

Molar Calculations - Lecture Notes for Chapter 6. Lecture Notes Chapter Introduction Page 1 of 9 Page 2 of 9 Lecture Notes Chapter 6 1. Introduction a. The above equation describes the synthesis of water from hydrogen and oxygen. b. It is not balanced, however. c. Notice how the number

More information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs

More information

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities Chapter 10 Chemical Quantities 101 The Mole: A Measurement 102 Mole-Mass and Mole-Volume Relationships 103 Percent Composition and Chemical Formulas 1 CHEMISTRY & YOU How can you quantify the amount of

More information

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages )

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages ) Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches

More information

THE MOLE (a counting unit)

THE MOLE (a counting unit) MOLE AND MATH THE MOLE (a counting unit) A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mole eggs = 6.022 x 10 23 eggs 1 dozen

More information

Lecture Notes Chapter 6

Lecture Notes Chapter 6 Lecture Notes Chapter 6 1. Introduction a. The above equation describes the synthesis of water from hydrogen and oxygen. b. It is not balanced, however. à c. Notice how the number of oxygen atoms on left

More information

Finding Formulas. using mass information about a compound to find its formula

Finding Formulas. using mass information about a compound to find its formula Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula

More information

6/28/11. Avogadro s Number and the Mole. The Mole. The Mole. The Mole (mol)

6/28/11. Avogadro s Number and the Mole. The Mole. The Mole. The Mole (mol) Avogadro s Number and the Mole Molecular weight: The sum of atomic weights of all atoms in a molecule. Formula weight: The sum of atomic weights of all atoms in one formula unit of any compound. Mole:

More information

Note Taking Guide: Episode 701. Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.) Avogadro s Number - the = the number

Note Taking Guide: Episode 701. Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.) Avogadro s Number - the = the number Note Taking Guide: Episode 701 Name Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.)? grains of rice = 1.94 g Avogadro s Number - the = the number Molar Mass the of one of

More information

1.2: Mole, Conversion Factors, Empirical & Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL

1.2: Mole, Conversion Factors, Empirical & Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL 1.2: Mole, Conversion Factors, Empirical & Molecular Formulas Ms. Kiely Coral Gables Senior High IB Chemistry SL TURN IN the Signed Syllabus and Topic 1 Exercises Bell-Ringer #2 What amount in grams is

More information

Introductory Chemistry Fourth Edition Nivaldo J. Tro

Introductory Chemistry Fourth Edition Nivaldo J. Tro Introductory Chemistry Fourth Edition Nivaldo J. Tro Chapter 6 Chemical Composition Dr. Sylvia Esjornson Southwestern Oklahoma State University Weatherford, OK 6.1 How Much Sodium? Sodium is an important

More information

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance.

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. I. Measuring Matter Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. As you know, atoms and molecules are extremely

More information

Composion Stoichiometry

Composion Stoichiometry Composition Stoichiometry blank 3.3.13.notebook Due: Ch 10 RG Hummmm... How do you "measure" bananas? > How many? Count 1 dozen naners or 12 naners Composion Stoichiometry 3 new conversion factors > Avogadro's

More information

WKS 9.1 Calculating Molar Mass (1 page)

WKS 9.1 Calculating Molar Mass (1 page) WKS 9.1 Calculating Molar Mass (1 page) Find the molar mass (AKA the molecular or formula mass) for each of the following substances. Name of compound Formula of compound Work Molar Mass (g/mol) dichlorine

More information

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities 101 The Mole: A Measurement Chapter 10 Chemical Quantities 101 The Mole: A Measurement 102 Mole-Mass and Mole-Volume Relationships 103 Percent Composition and Chemical Formulas 1 Copyright Pearson Education,

More information

Naming and Counting Atoms and Molecules. Chemistry--Unit 2

Naming and Counting Atoms and Molecules. Chemistry--Unit 2 Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have

More information

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For

More information

Chemistry 101 Chapter 8 Chemical Composition

Chemistry 101 Chapter 8 Chemical Composition Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given

More information

Lesson 13: Ionic Equations & Intro to the Mole with Conversions

Lesson 13: Ionic Equations & Intro to the Mole with Conversions NOTES Name: Date: Class: Lesson 13: Ionic Equations & Intro to the Mole with Conversions Box 1: Balance: 1. Mg + O2 MgO 2. KClO3 KCl + O2 3. C2H6 + O2 CO2 + H2O Write and balance the equation that represents

More information

Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry

Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are

More information

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022 CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)

More information

The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume.

The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume. The Mole Concept The mole is a convenient unit A mole is the number of atoms present in exactly 12 g of the isotope carbon-12. In 12 g of carbon-12 there are 6.022 x 10 23 carbon atoms It is easily converted

More information

Chapter 3. Mass Relationships in Chemical Reactions

Chapter 3. Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and

More information

(DO NOT WRITE ON THIS TEST)

(DO NOT WRITE ON THIS TEST) Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation

More information

Unit 6: Chemical Quantities. Understanding The Mole

Unit 6: Chemical Quantities. Understanding The Mole Unit 6: Chemical Quantities Understanding The Mole 1 How do We Typically Measure Matter? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters.

More information

Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 11.1 notes 1 MOLE = 6.02 x 10 23 representative particles representative particles

More information

Chemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9

Chemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9 Chapter 9 Chemical Calculations: The Mole concept and Chemical Formula This material is not included in Midterm 1 1 Law of Definite Proportions (John Dalton) Chapter 9 A given compound always contains

More information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages )

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages ) 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate

More information

Chemical Quantities: Stoichiometry and the Mole

Chemical Quantities: Stoichiometry and the Mole Chemical Quantities: Stoichiometry and the Mole This is trying to summarize what we have learned up to this point: formulas, names, conversions, moles, quantities, reaction types, balancing equations,

More information

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance.

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. I. Measuring Matter Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. As you know, atoms and molecules are extremely

More information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for

More information

Chapter 8. The Mole Concept

Chapter 8. The Mole Concept Chapter 8 The Mole Concept Chapter 9 2 Avogadro s Number Avogadro s number (symbol N) is the number of atoms in 12.01 grams of carbon. Its numerical value is 6.02 10 23. Therefore, a 12.01 g sample of

More information

23 carbon atoms The number is known as Avogadro s d Number.

23 carbon atoms The number is known as Avogadro s d Number. THE MOLE (a counting unit).again! i A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon

More information

Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles representative particles = ATOMS, IONS,

More information

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq)

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq) 1) Write the reaction for Calcium and nitrogen reacting 3) What element on the periodic table is the largest? 3)Name these a) H2S (aq) b) HNO 3 (aq) Stoichiometry: mathematical relationships in formulas

More information

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,

More information

UNIT 9. Stoichiometry

UNIT 9. Stoichiometry UNIT 9 Stoichiometry FORMULA MASS Atomic Mass Unit (u): unit of mass for measuring atoms. (1 u = 1/12 th the mass of a carbon 12 atom) FORMULA MASS FORMULA MASS Example 2: Find the mass of one molecule

More information

A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH

A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH Chapter Outline Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly.

More information

Unit Two Worksheet WS DC U2

Unit Two Worksheet WS DC U2 Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed

More information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

Moles Homework Unit 6

Moles Homework Unit 6 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining

More information

Summer Preparatory Tasks for A Level Chemistry 2017.

Summer Preparatory Tasks for A Level Chemistry 2017. Summer Preparatory Tasks for A Level Chemistry 2017. Task One: Why have you chosen to complete an A Level in Chemistry? Research your future career and what subjects and grades are required to achieve

More information

CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY

CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY 1 One drop of water is about 0.05g or 0.05 ml One drop of water contains about 1.67 x 10 21 H 2 O molecules 167,000,000,000,000,000,000 H 2 O molecules

More information

The Mole. Relative Atomic Mass Ar

The Mole. Relative Atomic Mass Ar STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers

More information

If you're given a mass percent, you can use it as a conversion factor between the element and the compound

If you're given a mass percent, you can use it as a conversion factor between the element and the compound Announcements Wednesday, September 23, 2009 MasteringChemistry due dates (all at 11:59 pm): Ch 3: Fri, Sep 25 Exam 1: next Mon, Sep 28. 20-25 multiple choice questions Short answer (naming, chemical equations)

More information

CHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet

CHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is

More information

Chapter 9: Stoichiometry The Arithmetic ti Of Equations

Chapter 9: Stoichiometry The Arithmetic ti Of Equations Chapter 9: Stoichiometry The Arithmetic of Equations Chemical Calculations Limiting Reagent and Percent Yield The Arithmetic ti Of Equations -- The Arithmetic of Equations -- Using Everyday Equations Stoichiometry

More information

CHAPTER 9 AVOGADRO S NUMBER

CHAPTER 9 AVOGADRO S NUMBER CHAPTER 9 AVOGADRO S NUMBER Just like we count in dozens, gross or ream, we count atoms in groups because of their minute sizes. Like in finding the number of atoms in12.01g of C, Experiments have shown

More information