# Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas

 To view this video please enable JavaScript, and consider upgrading to a web browser that supports HTML5 video
Save this PDF as:

Size: px
Start display at page:

Download "Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas"

## Transcription

1 Date In Class Homework 10/22 Thur Counting By Mass Lab 10/23 Fri (mole day!!!) THE MOLE! in room /26 Mon (LSM) More on the Mole Watch empirical and molecular formula video. 10/27 Tue % Composition & Calculating Empirical Formulas work on problems in the packet (1-7 on page 8) 10/28 Wed. Nomenclature Review Prelab for Hydrated Crystal Lab 10/29 Thurs Hydrated Crystal Lab 10/30 Fri NO SCHOOL! whoo hoo!!! 11/2 Mon Work on Unit Packet work on problems in the packet (8-20 on pages 9) Finish all problems in Unit Packet (21 28 on page 10-11) 11/3 Tues Review for Chapter 10 Test Study for Test 11/4 Wed Chapter 10 Test prelab for Types of Chemical Reactions 11/5 Thur Types of Chemical Reactions 1

2 Notes for chapter 10: 1. What is a mole? 2. What units can a mole be converted to/from: a. b. c. MOLE/PARTICLE (MOLECULES AND ATOMS) 3. How many molecules are in a mole? 4. When converting from molecules/atoms you 5. When converting from moles to molecules/atoms you Mole/Particle Practice: a. How many moles are in 5.3 x atoms of copper? b. How many molecules are there in 3.5 moles of sucrose? 2

3 MOLE/MASS (GRAMS) 6. Define atomic mass in terms of moles: a. What is the atomic mass of 1 mole of a hydrogen atom? b. What is the atomic mass of 1 mole of an aluminum atom? 7. Define molar mass. 8. Show how you calculate the molar mass of water (H 2 O) 9. When converting from grams to moles you 10. When converting from moles to grams you Mole/Gram Practice: a. How many grams of Iron are in 2.7 moles of Iron? b. How many moles of Zinc are in 15 grams of Zinc? c. How many grams are in 23 moles of CO 2? d. How many moles are in 562 grams of CO 2? e. Calculate the molar mass of ammonium carbonate f. How many grams are in3.5 moles of ammonium carbonate? 3

4 MOLE/VOLUME (LITERS) 11. What does STP stand for? 12. What is the temperature and pressure at STP? 13. At STP when converting from liters to moles you 14. At STP when converting from moles to liters you Mole/Liter Practice: a. How many liters are present in 10 moles of H 2 at STP? b. How many moles are in 17 L of water vapor? THE MOLE: A BRIGE BETWEEN PARTICLES, GRAMS, AND LITERS 15. List the steps used in calculating how many molecules of H 2 O are present in 10.8 grams? 16. How many liters are present in 6 grams of O 2 gas at STP 4

5 Video on Empirical and Molecular Formulas: Link: https://www.youtube.com/watch?v=wnrabwvhyky or search Tyler Dewitt Empirical and Molecular Formulas Video title is: Empirical Formula and Molecular Formula Introduction Guided Notes What is a molecular formula? Questions What is an empirical formula? Use ethene (which is really butene.) as an example of a molecular and empirical formula. Write the molecular formula and empirical formula for cyanuric triazide What do you divide by to get the empirical formula for C 5 H 10 O 5? What is the empirical formula for C 5 H 10 O 5? When is the molecular formula the same as the empirical formula? Why can many compounds have the same empirical formula? Show an example of several molecular formulas that come from the same empirical formula. Check your learning Practice. Write the empirical formulas for the following compounds: 1. H 2 O 2 2. H 2 O 3. C 2 H 10 O 4 4. C 5 H 10 O 2 Answers to above 1. HO 2. H 2 O 3. CH 5 O 2 4. C 5 H 10 O 2 5

6 Percent Composition and Calculating Empirical Formulas: 1. What is a percent composition? 2. Write the equation for calculating % composition? % composition = x Using the molar mass we calculated for ammonium carbonate from page 3 e, show how to calculate the percent of each element in the compound. a. N b. H c. C d. O 4. Calculate the percentage composition for all the elements in barium nitrate? 5. Write each step for how to calculate the empirical formula of a compound using mass or percent composition. a. Step 1. b. Step 2. c. Step 3. d. Step 4. 6

7 6. Use the steps in 5. to calculate the empirical formula of a compound that contains 28.4 g copper and 71.6 g bromine? 7. Follow the steps in 5. to calculate the empirical formula of a compound that contains 36.4% Carbon and 63.6% Nitrogen 7

8 Homework Practice Problems answers on last pages 1. Find the molar mass (g/mole) of: a. Na e. MgI 2 b. C f. AgClO 2 c. O 2 g. Cu(NO 3 ) 2 d. KOH h. Mg 3 (PO 4 ) 2 2. Calculate the mass (grams) of: a mole of CaCl 2 b. 2.0 mol of Al c mol H 2 SO 4 d mole of Na 2 O 3. Calculate moles in: a g of O 2. b. 3.2 g of H 2 O c. 168 g of NaHCO 3 d. 6.25g Al 2 O 3 4. Calculate the number of molecules in: a. 3.0 moles OF ANYTHING b. 32 mol of CH 4 c. 1.4 mol of NH 3 d. 2.5 mol O 2 5. Calculate the number of moles in: a x molecules b. 3.5 x molecules of HCl c. 6.5 x molecules of H 2 SO 4 d. 3.5 x molecules of SO 3 6. Calculate the number of moles in: a. 45 L F 2 b. 3.5 L SO 2 c L CO 7. Calculate the volume in liters of: a mol NO 2 b. 8.5 mol CO 2 c. 105 mol CO 8

9 8. Determine mass in grams of 40.0 moles of sodium carbonate. 9. How many grams are in moles of Sn 10. How many liters are in 6.0 mol O Calculate moles in g of aluminum sulfate. 12. How many moles are in 40.0 g Na 2 CO How many moles are in 3.00 L of N 2 Moles are the Bridge between units: 14. Determine the mass in grams of 2.35 molecules of C 12 H 22 O How many liters are present in 100g of CO 2 (at STP)? 16. How many sulfur atoms are present in 25.0 grams of H 2 SO 4? 17. How many atoms are in 2.00 grams of carbon? (2 steps) 18. Determine the mass of 50L of CO. 19.(challenge) How many moles of carbon atoms are in 3.00 grams of C 2 H 5 OH? Percent Composition: 20. Determine the percentage composition of each element in the following compounds: a. magnesium iodide, MgI 2 %Mg = % I = b. calcium chlorate, Ca(ClO 3 ) 2 %Ca= %Cl = % O = 9

10 Empirical vs. Molecular formulas 21. Write the empirical formula for each of the following compounds. (Not all will need to be changed!) a. Na 2 O 2 d. Cu 2 C 2 O 4 b. Li 2 SO 4 e. CaC 4 H 4 O 6 c. Hg 2 F 2 f. C 6 H 6 Calculating Empirical Formulas 22. What is the empirical formula of a compound that contains 1.67 g of Ce and 4.54 g of I? 23. What is the empirical formula of benzoic acid (a food preservative) if it contains 68.8% carbon, 4.95% H, and 26.2% O by mass? 24. Calculate the empirical formula for a compound made up of 63.6% iron and 36.4% sulfur. 25. Calculate the empirical formula of a hydrate that is 48.8% magnesium sulfate and 51.2% water (from lab) 26. Calculate the formula for a hydrate that is 37.07% sodium carbonate and 62.93% water (from lab) 10

11 Nomenclature Practice: 27. Provide the name for each of the following: a. PbCl 2 g. H 2 CO 3 b. Hg(NO 3 ) 2 h. Sn 3 (PO 4 ) 2 c. AgF i. N 3 Br 7 d. Ca(OH) 2 j. H 2 SO 3 e. HF k. HNO 3 f. S 4 O 6 l. Cu(C 2 H 3 O 2 ) Provide the formula for each of the following: a. Iron (III) oxide g. acetic acid b. aluminum iodide h. carbon monosulfide c. Lead (II) sulfate i. phosphoric acid d. mercury (II) nitrate j. chlorous acid e. tin (IV) hydroxide k. hydroselenic acid f. ammonium sulfide l. disulfur noniodide 11

12 Chemistry Chap. 10 HW- Answers 1. a g b g c g d g e g f g g g h g 2. a g b g c. 49 g d. 6.2 g 3. a..500 mol b..18 mol c mol d mol 4. a. 1.8 x molecules b. 1.9 x molecules c. 8.4 x molecules d. 1.5 x molecules 5. a mol b. 5.8 mol c. 1.1 x 10 6 mol d. 5.8 x mol 6. a. 2.0 mol b..17 mol c mol 7. a. 101 L b. 190 L c L moles Na2CO3 x 106g/1mol = 4240g g L g aluminum sulfate x 1molH2SO4/342g = 1.5 mol mol mol molecules C12H22O x 1023 molecules x 342g/mol = 1.34 x g g CO2 44g x 22.4L/mol = 50.9 L x atoms S grams C 12 gc x 6.02 x atoms/mol = 1.0 x atoms C L of CO 22.4L x 28g/mol = 62.5 g CO grams C2H5OH 46g x 2C/1 C2H5OH = 0.13 mol C atoms 20. a. %Mg= 24.3 / x 100 = 8.7% %I = 254/278.3 x 100 = 91.3% b. Cl = 71/207 x 100 = 34.3% O = 96 / 207 x 100 =46.4% 21. Write the empirical formula for each of the following compounds. (Not all will need to be changed!) a. Na2O2 _NaO d. Cu2C2O4 CuCO2 b. Li2SO4 _ Li2SO4 e. CaC4H4O6 CaC4H4O6 c. Hg2F2 HgF f. C6H6 CH 12

13 22. What is the empirical formula of a compound that contains 1.67 g of Ce and 4.54 g of I? 1.67g/140= 0.012mol 0.012/0.012 = g/127 = mol 0.036/0.012 = 3 CeF3 23. What is the empirical formula of benzoic acid (a food preservative) if it contains 68.8% carbon, 4.95% H, and 26.2% O by mass? 68.8g C/12 = 5.73 mol C 5.73/1.64 = 3.5 x g H/1 = 4.95 mol H 4.95/1.64 = 3 x g O / 16 = 1.64 mol O 1.64/1.64 = 1 x 2 2 C7H6O2 24. Calculate the empirical formula for a compound made up of 63.6% iron and 36.4% sulfur. 63.6/55.8 = 1.14 FeS 36.4g/32 = Calculate the empirical formula of a hydrate that is 48.8% magnesium sulfate and 51.2% water 48.8g/120 = mol MgSO /0.405 = g/18 = 2.84 mol H 2 O 2.84/0.045 = 7 MgSO4 7 H2O 26. Calculate the formula for a hydrate that is 37.07% sodium carbonate and 62.93% water 37.07g/106 = mole (Na) 2 CO / g / 18 = 3.49 mol H 2 O 3.49 / Na2CO3 * 10 H2O 27. Provide the name for each of the following: a. Lead (II) chloride b. mercury (II) oxide c. silver fluoride d. calcium hydroxide e. hydrofluoric acid f. tetrasulfur hexoxide g. carbonic acid h. tin(ii) phosphate i. trinitrogen heptabromide j. sulfurous acid k. nitric acid l. copper (II) acetate 28. Provide the formula for each of the following: a. Fe2O3 g. HC 2 H 3 O 2 b. Al I 3 h. CS c. PbSO4 i. H 3 PO 4 d. Hg(NO 3 ) 2 j. HClO 2 e. Sn(OH) 4 k. H 2 Se f. (NH 4 ) 2 S l. S 2 I 9 13

### Ch. 10 The Mole I. Molar Conversions

Ch. 10 The Mole I. Molar Conversions I II III IV A. What is the Mole? A counting number (like a dozen) Avogadro s number (N A ) 1 mole = 6.022 10 23 representative particles B. Mole/Particle Conversions

### Moles, Molecules, and Grams Worksheet Answer Key

Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3

### Study Guide For Chapter 7

Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance

### Mole Notes.notebook. October 29, 2014

1 2 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

### Name: Class: Date: 2 4 (aq)

Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

### SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

### Chemistry Post-Enrolment Worksheet

Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part

### Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

### MOLES AND MOLE CALCULATIONS

35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

### CHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT

CHAPTER 3 Calculations with Chemical Formulas and Equations MOLECULAR WEIGHT (M. W.) Sum of the Atomic Weights of all atoms in a MOLECULE of a substance. FORMULA WEIGHT (F. W.) Sum of the atomic Weights

### MOLECULAR MASS AND FORMULA MASS

1 MOLECULAR MASS AND FORMULA MASS Molecular mass = sum of the atomic weights of all atoms in the molecule. Formula mass = sum of the atomic weights of all atoms in the formula unit. 2 MOLECULAR MASS AND

### Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.

### PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

### How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique.

How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique. What units do we use to define the weight of an atom? amu units of atomic weight. (atomic

### Chemistry 65 Chapter 6 THE MOLE CONCEPT

THE MOLE CONCEPT Chemists find it more convenient to use mass relationships in the laboratory, while chemical reactions depend on the number of atoms present. In order to relate the mass and number of

### A dozen. Molar Mass. Mass of atoms

A dozen Molar Mass Science 10 is a number of objects. A dozen eggs, a dozen cars, and a dozen people are all 12 objects. But a dozen cars has a much greater mass than a dozen eggs because the mass of each

### W1 WORKSHOP ON STOICHIOMETRY

INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

### Chapter 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

### Calculating Molar Mass of a Compound

Instructions for Conversion Problems For every conversion problem Write the number in the problem down with unit and a multiplication sign Decide which conversion factor you should use, Avagadro s or molar

### The Mole. Chapter 2. Solutions for Practice Problems

Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of

### ATOMS. Multiple Choice Questions

Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

### Chapter 3 Stoichiometry

Chapter 3 Stoichiometry 3-1 Chapter 3 Stoichiometry In This Chapter As you have learned in previous chapters, much of chemistry involves using macroscopic measurements to deduce what happens between atoms

### Stoichiometry. Lecture Examples Answer Key

Stoichiometry Lecture Examples Answer Key Ex. 1 Balance the following chemical equations: 3 NaBr + 1 H 3 PO 4 3 HBr + 1 Na 3 PO 4 2 C 3 H 5 N 3 O 9 6 CO 2 + 3 N 2 + 5 H 2 O + 9 O 2 2 Ca(OH) 2 + 2 SO 2

Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500

### English already has many collective nouns for fixed, given numbers of objects. Some of the more common collective nouns are shown in Table 7.1.

96 Chapter 7: Calculations with Chemical Formulas and Chemical Reactions Chemical reactions are written showing a few individual atoms or molecules reacting to form a few atoms or molecules of products.

### Mole Calculations Multiple Choice Review PSI Chemistry

Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela

### Solution. 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

### 602X10 21 602,000,000,000, 000,000,000,000 6.02X10 23. Pre- AP Chemistry Chemical Quan44es: The Mole. Diatomic Elements

Pre- AP Chemistry Chemical Quan44es: The Mole Mole SI unit of measurement that measures the amount of substance. A substance exists as representa9ve par9cles. Representa9ve par9cles can be atoms, molecules,

### Lecture 5, The Mole. What is a mole?

Lecture 5, The Mole What is a mole? Moles Atomic mass unit and the mole amu definition: 12 C = 12 amu. The atomic mass unit is defined this way. 1 amu = 1.6605 x 10-24 g How many 12 C atoms weigh 12 g?

### Ch. 6 Chemical Composition and Stoichiometry

Ch. 6 Chemical Composition and Stoichiometry The Mole Concept [6.2, 6.3] Conversions between g mol atoms [6.3, 6.4, 6.5] Mass Percent [6.6, 6.7] Empirical and Molecular Formula [6.8, 6.9] Bring your calculators!

### Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.

Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of

### Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

### Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V

44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts

### Worksheet # 8 Graham/09 Due

CHE 100 Worksheet # 8 Graham/09 Name Key Due 1. According to the law of definite proportions, if a sample of a compound contains 7.00 grams of sulfur and 3.50 grams of oxygen, then another sample of the

### Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

### Formulas, Equations and Moles

Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule

### 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

### Calculating Atoms, Ions, or Molecules Using Moles

TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

### = 16.00 amu. = 39.10 amu

Using Chemical Formulas Objective 1: Calculate the formula mass or molar mass of any given compound. The Formula Mass of any molecule, formula unit, or ion is the sum of the average atomic masses of all

### Atomic Masses. Chapter 3. Stoichiometry. Chemical Stoichiometry. Mass and Moles of a Substance. Average Atomic Mass

Atomic Masses Chapter 3 Stoichiometry 1 atomic mass unit (amu) = 1/12 of the mass of a 12 C atom so one 12 C atom has a mass of 12 amu (exact number). From mass spectrometry: 13 C/ 12 C = 1.0836129 amu

### Stoichiometry. Unit Outline

3 Stoichiometry Unit Outline 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis

### 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

### Answers and Solutions to Text Problems

Chapter 7 Answers and Solutions 7 Answers and Solutions to Text Problems 7.1 A mole is the amount of a substance that contains 6.02 x 10 23 items. For example, one mole of water contains 6.02 10 23 molecules

### UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12

### Part One: Mass and Moles of Substance. Molecular Mass = sum of the Atomic Masses in a molecule

CHAPTER THREE: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS Part One: Mass and Moles of Substance A. Molecular Mass and Formula Mass. (Section 3.1) 1. Just as we can talk about mass of one atom of

### EXPERIMENT 12: Empirical Formula of a Compound

EXPERIMENT 12: Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound

### Calculation of Molar Masses. Molar Mass. Solutions. Solutions

Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements

### Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

### STOICHIOMETRY UNIT 1 LEARNING OUTCOMES. At the end of this unit students will be expected to:

STOICHIOMETRY LEARNING OUTCOMES At the end of this unit students will be expected to: UNIT 1 THE MOLE AND MOLAR MASS define molar mass and perform mole-mass inter-conversions for pure substances explain

### Sample Exercise 3.1 Interpreting and Balancing Chemical Equations

Sample Exercise 3.1 Interpreting and Balancing Chemical Equations The following diagram represents a chemical reaction in which the red spheres are oxygen atoms and the blue spheres are nitrogen atoms.

### Tuesday, November 27, 2012 Expectations:

Tuesday, November 27, 2012 Expectations: Sit in assigned seat Get out Folder, Notebook, Periodic Table Have out: Spiral (notes), Learning Target Log (new) No Backpacks on tables Listen/Pay Attention Learning

### Chem 31 Fall 2002. Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Writing and Balancing Chemical Equations

Chem 31 Fall 2002 Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations Writing and Balancing Chemical Equations 1. Write Equation in Words -you cannot write an equation unless you

### Chapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole

Chapter 4 Chemical Composition Chapter 4 Topics 1. Mole Quantities 2. Moles, Masses, and Particles 3. Determining Empirical Formulas 4. Chemical Composition of Solutions Copyright The McGraw-Hill Companies,

### Lecture Topics Atomic weight, Mole, Molecular Mass, Derivation of Formulas, Percent Composition

Mole Calculations Chemical Equations and Stoichiometry Lecture Topics Atomic weight, Mole, Molecular Mass, Derivation of Formulas, Percent Composition Chemical Equations and Problems Based on Miscellaneous

### The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015

The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical

### Atomic mass is the mass of an atom in atomic mass units (amu)

Micro World atoms & molecules Laboratory scale measurements Atomic mass is the mass of an atom in atomic mass units (amu) By definition: 1 atom 12 C weighs 12 amu On this scale 1 H = 1.008 amu 16 O = 16.00

### Chemical formulae are used as shorthand to indicate how many atoms of one element combine with another element to form a compound.

29 Chemical Formulae Chemical formulae are used as shorthand to indicate how many atoms of one element combine with another element to form a compound. C 2 H 6, 2 atoms of carbon combine with 6 atoms of

### Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

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

### We know from the information given that we have an equal mass of each compound, but no real numbers to plug in and find moles. So what can we do?

How do we figure this out? We know that: 1) the number of oxygen atoms can be found by using Avogadro s number, if we know the moles of oxygen atoms; 2) the number of moles of oxygen atoms can be found

### THE MOLE / COUNTING IN CHEMISTRY

1 THE MOLE / COUNTING IN CHEMISTRY ***A mole is 6.0 x 10 items.*** 1 mole = 6.0 x 10 items 1 mole = 60, 00, 000, 000, 000, 000, 000, 000 items Analogy #1 1 dozen = 1 items 18 eggs = 1.5 dz. - to convert

### Stoichiometry. Web Resources Chem Team Chem Team Stoichiometry. Section 1: Definitions Define the following terms. Average Atomic mass - Molecule -

Web Resources Chem Team Chem Team Section 1: Definitions Define the following terms Average Atomic mass - Molecule - Molecular mass - Moles - Avagadro's Number - Conservation of matter - Percent composition

### Chapter 6 Chemical Calculations

Chapter 6 Chemical Calculations 1 Submicroscopic Macroscopic 2 Chapter Outline 1. Formula Masses (Ch 6.1) 2. Percent Composition (supplemental material) 3. The Mole & Avogadro s Number (Ch 6.2) 4. Molar

Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching

Page 1 of 14 Amount of Substance Key terms in this chapter are: Element Compound Mixture Atom Molecule Ion Relative Atomic Mass Avogadro constant Mole Isotope Relative Isotopic Mass Relative Molecular

### 3.3 Moles, 3.4 Molar Mass, and 3.5 Percent Composition

3.3 Moles, 3.4 Molar Mass, and 3.5 Percent Composition Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans Copyright

### GCE. Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry (9080) Edexcel Advanced GCE in Chemistry (Nuffield) (9086) Issue 3 October 2004

GCE Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry (Nuffield) (9086) Issue 3 October 2004 Workbook for GCE students GCE Moles, Formulae and Equations Edexcel Advanced GCE in Chemistry

### Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE

T-6 Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE FORMULAS: A chemical formula shows the elemental composition of a substance: the chemical symbols show what elements are present and the numerical

### Chemistry Final Study Guide

Name: Class: Date: Chemistry Final Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The electrons involved in the formation of a covalent bond

### Woods Chem-1 Lec-02 10-1 Atoms, Ions, Mole (std) Page 1 ATOMIC THEORY, MOLECULES, & IONS

Woods Chem-1 Lec-02 10-1 Atoms, Ions, Mole (std) Page 1 ATOMIC THEORY, MOLECULES, & IONS Proton: A positively charged particle in the nucleus Atomic Number: We differentiate all elements by their number

### Lecture 3: (Lec3A) Atomic Theory

Lecture 3: (Lec3A) Atomic Theory Mass of Atoms Sections (Zumdahl 6 th Edition) 3.1-3.4 The Concept of the Mole Outline: The mass of a mole of atoms and the mass of a mole of molecules The composition of

### EDEXCEL INTERNATIONAL GCSE CHEMISTRY EDEXCEL CERTIFICATE IN CHEMISTRY ANSWERS SECTION E

EDEXCEL INTERNATIONAL GCSE CHEMISTRY EDEXCEL CERTIFICATE IN CHEMISTRY ANSWERS SECTION E (To save endless repetition, wherever they are included, comments are intended for homeschooling parents who may

### Calculations and Chemical Equations. Example: Hydrogen atomic weight = 1.008 amu Carbon atomic weight = 12.001 amu

Calculations and Chemical Equations Atomic mass: Mass of an atom of an element, expressed in atomic mass units Atomic mass unit (amu): 1.661 x 10-24 g Atomic weight: Average mass of all isotopes of a given

### Moles Lab mole. 1 mole = 6.02 x 1023. This is also known as Avagadro's number Demo amu amu amu

Moles I. Lab: Rice Counting II. Counting atoms and molecules I. When doing reactions chemists need to count atoms and molecules. The problem of actually counting individual atoms and molecules comes from

### Test Review Periodic Trends and The Mole

Test Review Periodic Trends and The Mole The Mole SHOW ALL WORK ON YOUR OWN PAPER FOR CREDIT!! 1 2 (NH42SO2 %N 24.1 %H 6.9 %S 27.6 %O 41.3 % Al %C 35.3 %H 4.4 %O 47.1 Al(C2H3O23 13.2 3 How many moles are

### INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e

CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum

### Molecules, Atoms, Grams and Mole Calculation Practice

Molecules, Atoms, Grams and Mole Calculation Practice Helpful HINTS: In these problems look for two things: 1) From what unit to what unit? 2) Does the object stay the same, or does the object change?

### Chapter 5 Chemical Quantities and Reactions. Collection Terms. 5.1 The Mole. A Mole of a Compound. A Mole of Atoms.

Chapter 5 Chemical Quantities and Reactions 5.1 The Mole Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans 1

### Matter. Atomic weight, Molecular weight and Mole

Matter Atomic weight, Molecular weight and Mole Atomic Mass Unit Chemists of the nineteenth century realized that, in order to measure the mass of an atomic particle, it was useless to use the standard

### 10 Cl atoms. 10 H2O molecules. 8.3 mol HCN = 8.3 mol N atoms 1 mol HCN. 2 mol H atoms 2.63 mol CH2O = 5.26 mol H atoms 1 mol CH O

Chem 100 Mole conversions and stoichiometry worksheet 1. How many Ag atoms are in.4 mol Ag atoms? 6.0 10 Ag atoms 4.4 mol Ag atoms = 1.46 10 Ag atoms 1 mol Ag atoms. How many Br molecules are in 18. mol

### 4.4 Calculations Involving the Mole Concept

44 Section 43 Questions 1 Define Avogadro s constant, and explain its significance in quantitative analysis 2 Distinguish between the terms atomic mass and molar mass 3 Calculate the mass of a molecule

### CHEM 120 Online: Chapter 6 Sample problems Date: 2. Which of the following compounds has the largest formula mass? A) H2O B) NH3 C) CO D) BeH2

CHEM 120 Online: Chapter 6 Sample problems Date: 1. To determine the formula mass of a compound you should A) add up the atomic masses of all the atoms present. B) add up the atomic masses of all the atoms

### Calculate the molar mass of each of the following: (a) SnO 2. Calculate the molar mass of each of the following: (a) N 2 O 4

Calculate the molar mass of each of the following: (a SnO (b BaF (c Al (SO 3 (d MnCl Calculate the molar mass of each of the following: (a N O (b C 8 H 10 (c MgSO. 7 H O (d Ca(C H 3 O (a Mass in grams

### AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

### F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

### A 1.008 g sample of H contains 6.0221415 x 10 23 H atoms.

7 Chemical Composition 7. Avogadro s umber n 8, the talian scientist, Amadeo Avogadro proposed that: Equal volumes of gas at equal temperatures and pressures have the same number of particles. This law,

### CH3 Stoichiometry. The violent chemical reaction of bromine and phosphorus. P.76

CH3 Stoichiometry The violent chemical reaction of bromine and phosphorus. P.76 Contents 3.1 Counting by Weighing 3.2 Atomic Masses 3.3 The Mole 3.4 Molar Mass 3.5 Percent Composition of Compounds 3.6

### The Mole Concept. The Mole. Masses of molecules

The Mole Concept Ron Robertson r2 c:\files\courses\1110-20\2010 final slides for web\mole concept.docx The Mole The mole is a unit of measurement equal to 6.022 x 10 23 things (to 4 sf) just like there

### MASS RELATIONSHIPS IN CHEMICAL REACTIONS

MASS RELATIONSHIPS IN CHEMICAL REACTIONS 1. The mole, Avogadro s number and molar mass of an element. Molecular mass (molecular weight) 3. Percent composition of compounds 4. Empirical and Molecular formulas

### Stoichiometry of Formulas and Equations

sil07204_ch03_69-107 8/22/05 15:16 Page 69 CHAPTER THREE Stoichiometry of Formulas and Equations Key Principles The mole (mol) is the standard unit for amount of substance and consists of Avogadro s number

### EXAMPLE EXERCISE 4.1 Change of Physical State

EXAMPLE EXERCISE 4.1 Change of Physical State State the term that applies to each of the following changes of physical state: (a) Snow changes from a solid to a liquid. (b) Gasoline changes from a liquid

### Solutions to Supplementary Check for Understanding Problems

Chapter 5 s to Supplementary Check for Understanding Problems Moles and Molar Mass 1. Indicate the appropriate quantity for each of the following. a) A mole of N atoms contains atoms. b) A mole of N molecules

### Type: Single Date: Kinetic Theory of Gases. Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14

Type: Single Date: Objective: Kinetic Theory of Gases Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14 AP Physics Mr. Mirro Kinetic Theory of Gases Date Unlike the condensed phases

### CHEMICAL FORMULAE AND STOICHIOMETRY

LOCUS 1 Section - CHEMICAL FORMULAE AND STOICHIOMETRY The language that chemists use to describe the forms of matter and the changes in its composition appears throughout the scientific world. Chemical

Contents Getting the most from this book...4 About this book....5 Content Guidance Topic 1 Atomic structure and the periodic table...8 Topic 2 Bonding and structure...14 Topic 2A Bonding....14 Topic 2B

### Summer Holidays Questions

Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the

### 7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

### AP Chemistry 2006 Free-Response Questions

AP Chemistry 006 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college

### Solubility of Salts - Ksp. Ksp Solubility

Solubility of Salts - Ksp We now focus on another aqueous equilibrium system, slightly soluble salts. These salts have a Solubility Product Constant, K sp. (We saw this in 1B with the sodium tetraborate