Moles and Chemical Reactions. Moles and Chemical Reactions. Molar mass = 2 x x x = g/mol


 Violet Bishop
 1 years ago
 Views:
Transcription
1 We have used the mole concept to calculate mass relationships in chemical formulas Molar mass of ethanol (C 2 H 5 OH)? Molar mass = 2 x x x = g/mol Mass percentage of carbon in ethanol? % C = 2 x x 100 % = % We can also use the mole concept to calculate mass relationships in chemical reactions is the study of mass relationships It requires a balanced equation The coefficients in a balanced chemical equation represents how many moles of one reactant are needed to react with other reactants. It also shows how many moles of product will be formed. Chemical equation relates moles of reactants to moles of products The equation DOES NOT directly relate the masses of reactants and products Consider the reaction 3 H 2 + N 2 2 NH 3 Balanced? Coefficients in a balanced equation number of moles 3 H 2 + N 2 2 NH 3 The coefficients in a balanced chemical equation can be used to relate the number of moles of each substance involved in a reaction. Molar ratios 3 molecules 1 molecules 2 molecules 300 molecules 100 molecules 200 molecules 3(6.02x10 23 ) molecules 6.02x10 23 molecules 2(6.02x10 23 ) molecules 3 moles 1 mole 2 moles mol reactant mol reactant mol product mol reactant mol product mol product 1
2 For the reaction: N H 2 2 NH 3 If you have 1.0 mole of H 2, how many moles of NH 3 can you produce? 3 different s can be written (why 3?) N H 2 2 NH 3 Note: Make sure your equation is balanced! 1 mol N 2 1 mol N 2 3 mol H 2 3 mol H 2 2 mol NH 3 2 mole NH 3 MOLAR RATIOS = CONVERSION FACTORS Given: 1.0 mol H 2 Find: mol NH 3 Conversion factor: # mol NH 3 = 1.0 mol H 2 x 2 mol NH 3 3 mole H 2 If you have 1.0 mole of H 2, how many moles of N 2 will be required to completely react all of the H 2? N H 2 2 NH 3 = 0.67 mol NH 3 Given: 1 mol H 2 Find: mol N 2 Conversion factor: 2
3 # moles N 2 = 1.0 mol H 2 x 1 mol N 2 3 mol H 2 How many moles of N 2 are needed to produce 0.50 moles of NH 3? N H 2 2 NH 3 = 0.33 mol N 2 Given: 0.5 mol NH3 Find: mol N 2 Conversion factor: From a balanced chemical equation we get the number of moles of reactants and products BUT # mol N 2 = 0.50 mol NH 3 x 1 mol N 2 2 mol NH 3 = 0.25 mol N 2 We don t measure out moles in the lab! Chemists use a balance to measure the mass of a substance used or produced in a reaction. How can you determine the mass of reactants or products? 3
4 Use the molar mass to convert from moles to grams The number of grams of a substance per mole Mass (g) Compound A X Mass (g) Compound B Molar mass Molar mass Moles Compound A Molar ratio Moles Compound B For the following reaction: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) How many grams of NH 3 would form if 2.11 moles of N 2 reacted with excess H 2? Given: 2.11 mol N 2 Find: g NH 3 Conversion factors:, molar mass g NH 3 = 2.11 mol N 2 x 2 mol NH 3 x g NH 3 1 mol N 2 1 mol NH 3 = 71.9 g NH 3 How many grams of N 2 are required to react completely with 9.47 grams of H 2? N 2 (g) + 3 H 2 (g) 2 NH 3 (g) CH O 2 CO H 2 O Answer the following questions: How many moles of O 2 are required to react with 1.72 moles of CH 4? Given: 9.47g H 2 Find: g N 2 Conversion factors: molar mass, How many grams of H 2 O will form when 1.09 moles of CH 4 react with excess O 2? g N 2 = 9.47 g H 2 x 1 mol H 2 x 1 mol N 2 x 28.01g N g H 2 3 mol H 2 1 mol N 2 How many grams of O 2 must react with excess CH 4 to produce 8.42 grams of CO 2? = 43.9 g N 2 4
5 Metallic iron reacts with oxygen to form iron(iii) oxide Balanced eqn: 4 Fe + 3 O 2 2 Fe 2 O 3 Calculate the grams of iron needed to produce 5.00 g of product. Given: 5.0 g Fe 2 O 3 Find: g Fe Conversion factors: molar masses Strategy: 4 Fe + 3 O 2 2 Fe 2 O 3 molar mass grams Fe 2 O 3 moles Fe 2 O 3 grams Fe moles Fe molar mass g Fe = 5.0 g Fe 2 O 3 x 1 mol Fe 2 O 3 x = 3.5 g Fe g Fe 2 O 3 x 4 mol Fe x g Fe 2 mol Fe 2 O 3 1 mol Fe Molar Mass of Fe 2 O 3 = 2 (55.85 g/mole) + 3 (16.0 g/mole) = g Fe 2 O 3 /mole 5
6 The steel industry relies on the reaction between iron(iii) oxide and carbon to produce iron and CO 2. 2Fe 2 O 3 3C 4Fe + 3CO 2 What mass of iron can be obtained from 454 g of iron(iii) oxide? Ethane (C 2 H 6 ) burns in oxygen to form CO 2 and water 2C 2 H 6 + 7O 2 4CO 2 + 6H 2 O What mass of ethane is required to produce 100. g of water? What mass of carbon is required to react with 454 g of iron(iii) oxide? What mass of CO 2 is formed along with the 100. g of water? Making Turkey Sandwiches Suppose you were going to make turkey sandwiches: slices bread + 1 slice cheese + 1 slice turkey 1 sandwich Making Turkey Sandwiches 2 slices bread + 1 slice cheese + 1 slice turkey 1 sandwich You have 8 slices of bread and 20 slices of turkey and 20 slices of cheese. How many sandwiches you can make using the above recipe? We can only make 4 sandwiches because we don t have enough bread! Bread = limiting reagent or limiting reactant You have 4 slices of cheese and 20 slices of turkey and 20 slices of bread. How many sandwiches you can make using the above recipe? Limiting reactant? 6
7 Similar situations occur in chemical reactions when one of the reactants is used up before the others. No further reaction can occur The excess reactant(s) are leftovers. 2 H 2 (g) + O 2 (g) 2 H 2 O (l) If we react 10 moles of H 2 with 7 moles of O 2, not all of the O 2 will react because we will run out of H 2 first! For 10 moles of H 2 we need only 5 moles of O 2! Limiting reactant: the reactant that is completely consumed in a reaction determines or limits the amount of product formed. To determine which reactant is the limiting reagent: Compare the number of moles of each reactant needed with the number of moles of each reactant available OR Calculate the number of grams of product that each reactant could form Reactant that forms the least amount of product will be the limiting reagent. 2 H 2 (g) + O 2 (g) 2 H 2 O (l) 7
8 If 10.0 grams of H 2 are mixed with 75.0 grams of O 2, which reactant is the limiting reagent? 2 H 2 (g) + O 2 (g) 2 H 2 O (l) Method 1 Step 1: Convert mass to moles Moles H 2 = 10.0 g H 2 x 1 mole = 4.95 mol H 2 available 2.02 g Moles O 2 = 75.0 g O 2 x 1 mole = 2.34 mol O 2 available 32.0 g Step 2 Step 3 Pick H 2 and find the moles O 2 needed to react with all of the H 2 moles O 2 needed = 4.95 mol H 2 x 1 mol O 2 2 mol H 2 = 2.48 moles O 2 Compare the # moles O 2 needed to # moles O 2 available. O 2 needed = 2.48 moles O 2 O 2 available = 2.34 moles O 2 Less O 2 is available than we need to react with all of the H 2. O 2 will run out first. Therefore, O 2 is the limiting reagent. 8
9 Method 2 Step 1: Calculate the amount of product each reactant could form. g H 2 O from H 2 = 10.0 g H 2 x 1 mol H 2 x 2 mol H 2 O 2.02 g H 2 2 mol H 2 x 18.0 g H 2 O = 89.1 g H 2 O 1 mol H 2 O g H 2 O from O 2 = 75.0 g O 2 x 1 mol O 2 x 2 mol H 2 O 32.0 g O 2 1 mol O 2 x 18.0 g H 2 O = 84.4 g H 2 O 1 mol H 2 O Limiting reagent is the one that produces the least product. O 2 is the 10.0 g H 2 could produce 89.1 g H 2 O limiting 75.0 g O 2 could produce 84.4 g H 2 O reagent The Limiting Reactant The Limiting Reactant Suppose we have a mixture of 20.0 g of CH 4 and grams of O 2. Which is the limiting reactant? CH O 2 CO H 2 O CH O 2 CO H 2 O Now suppose that the 20.0 grams of CH 4 reacts with the grams of O 2. What mass of the unused reactant is left over when all the CH 4 has been consumed? 9
10 The Limiting Reactant Reaction Yield H 2 + C CH 4 Suppose that 20.0 g of H 2 reacts with 40.0 g of carbon Which reactant is limiting? What mass of CH 4 could form when combining these reactants? How much of the unused reactant is left over? We have been calculating how much product would form for various chemical reactions The amount we calculate is usually higher than what we would obtain in lab This is not a violation of the law of conservation of matter Why are the two values different? Reaction Yield Reaction Yield Often, the actual yield is less than the theoretical yield: reactants may not react completely i.e. the reaction does not go to completion byproducts may form unwanted side reactions (competing reactions) difficulty isolating and purifying the desired product The mass of product obtained in the reaction is the actual yield The maximum amount possible, calculated from the limiting reagent principle, is the theoretical yield The percentage yield is defined as: Actual yield Theoretical yield x 100 = percentage yield 10
11 Reaction Yield Reaction Yield A chemist isolates g of product from a reaction that has a calculated theoretical yield of g. What is the percentage yield? Lime (CaO) is produced by heating CaCO 3 according to the following equation: CaCO 3 (s) CaO(s) + CO 2 (g) Suppose we heat 510 grams of CaCO 3 and isolate 235 grams of CaO. What is the percentage yield? 11
PERIODIC TABLE OF ELEMENTS. 4/23/14 Chapter 7: Chemical Reactions 1
PERIODIC TABLE OF ELEMENTS 4/23/14 Chapter 7: Chemical Reactions 1 CHAPTER 7: CHEMICAL REACTIONS 7.1 Describing Reactions 7.2 Types of Reactions 7.3 Energy Changes in Reactions 7.4 Reaction Rates 7.5 Equilibrium
More informationPart 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
More informationChapter 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
More informationChapter 4 Chemical Equations & Stoichiometry
Chapter 4 Chemical Equations & Stoichiometry Chemical reactions are best described using equations which tells us what compounds we started with (reactants), what we did to them (reaction conditions) and
More informationChemical Equations and Calculations
Chemical Equations and Calculations A chemical equation is a shorthand way of indicating what is going on in a chemical reaction. We could do it the long way Two molecules of Hydrogen gas react with one
More informationCalculating 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
More informationMoles. 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)
More informationChapter 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.
More informationMass and Moles of a Substance
Chapter Three Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows
More informationThe mass of the formula unit is called the formula mass Formula masses are calculated the same way as molecular masses
Chapter 4: The Mole Atomic mass provides a means to count atoms by measuring the mass of a sample The periodic table on the inside cover of the text gives atomic masses of the elements The mass of an atom
More information7.1 Stoichiometry and Percent Yield
score /10 pts. Name Class Date 7.1 Stoichiometry and Percent Yield Mole Ratios An example: The combustion of propane is used to heat many rural homes in winter. Balance the equation below for the combustion
More informationAtomic 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
More informationName Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)
Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.
More informationLIMITING REAGENT PROBLEMS
LIMITING REAGENT PROBLEMS The first step in solving a limiting reagent problem is being able to recognize that you have a limiting reagent problem. Suppose you were given the following problem: A 50.6
More informationChapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGrawHill 2009 1
Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGrawHill 2009 1 3.1 Molecular and Formula Masses Molecular mass  (molecular weight) The mass in amu
More informationStoichiometry Dr. M. E. Bridge
Preliminary Chemistry Course Stoichiometry Dr. M. E. Bridge What is stoichiometry? The meaning of the word: The word stoichiometry comes from two Greek words: (meaning element ) and (meaning measure )
More informationPractice questions for Ch. 3
Name: Class: Date: ID: A Practice questions for Ch. 3 1. A hypothetical element consists of two isotopes of masses 69.95 amu and 71.95 amu with abundances of 25.7% and 74.3%, respectively. What is the
More informationChapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
More informationStoichiometry: Calculations with Chemical Equations
Stoichiometry: Calculations with Chemical Equations Objectives Use chemical equations to predict amount of product from given reactants Determine percentage yield Determine limiting reactant Working with
More informationCalculations with Chemical Reactions
Calculations with Chemical Reactions Calculations with chemical reactions require some background knowledge in basic chemistry concepts. Please, see the definitions from chemistry listed below: Atomic
More informationMolecular Formula: Example
Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More informationFormulas, 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
More informationLimiting Reactants and Percentage Yield
Section 3 Main Ideas One reactant limits the product of a reaction. Comparing the actual and theoretical yields helps chemists determine the reaction s efficiency. Limiting Reactants and Percentage Yield
More information3. How many moles of KCl and O 2 are formed from the decomposition of 6 moles of KClO 3?
What coefficients mean: 2 Na + Cl 2 2NaCl 2 Na 1 Cl 2 2NaCl 4 Na 2 Na + Cl 2 4Cl 2 6 moles Na 2NaCl 10 atoms Na ONLY WORKS FOR MOLES, MOLECULES, ATOMS 1. How many moles of H 2 and O 2 must react to form
More informationSection 9.1. Using Chemical Equations
1984, Union Carbide Plant 10000+ killed in Bhopal, India by Methyl Isocyanate 1988 Pepcon, Henderson Rocket Fuel Explosion Objectives 1. To understand more of the information given in a balanced equation
More informationDaily Practice Review 2/2829/08
Daily Practice Review 2/2829/08 1. Why is it not correct to balance an equation by changing the subscripts in one or more of the formulas? If you change the subscripts in a formula you change the chemical
More informationSTOICHIOMETRY.  the study of the quantitative aspects of chemical
STOICHIOMETRY  the study of the quantitative aspects of chemical GENERAL PLAN FOR STOICHIOMETRY Mass reactant Mass product Moles reactant Stoichiometric factor Moles product STOICHIOMETRY It rests on
More informationOutline. 6.1 The Mole and Avogadro s Number. 6.2 Gram Mole Conversions. 6.3 Mole Relationships and Chemical Equations
Outline 6.1 The Mole and Avogadro s Number 6.2 Gram Mole Conversions 6.3 Mole Relationships and Chemical Equations 6.4 Mass Relationships and Chemical Equations 6.5 Limiting Reagent and Percent Yield Goals
More informationStoichiometry Chapter 9 Assignment & Problem Set
Stoichiometry Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Stoichiometry 2 Study Guide: Things You Must Know Vocabulary (know the definition
More informationChapter 7: Stoichiometry  Mass Relations in Chemical Reactions
Chapter 7: Stoichiometry  Mass Relations in Chemical Reactions How do we balance chemical equations? How can we used balanced chemical equations to relate the quantities of substances consumed and produced
More informationChapter 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
More informationChemical calculations
Chemical calculations Stoichiometry refers to the quantities of material which react according to a balanced chemical equation. Compounds are formed when atoms combine in fixed proportions. E.g. 2Mg +
More informationIf you remember, we left off this part of the story with defining the mass of one 12
Chapter 11 Chemical Calculations For the past several weeks we have been working on our qualitative understanding of first atoms, then molecules, and finally chemical reactions. In this chapter we enter
More informationLimiting Reactant and Percent Yield Practice
Limiting Reactant and Percent Yield Practice Name 1) Consider the following reaction: NH 4 NO 3 + Na 3 PO 4 (NH 4 ) 3 PO 4 + NaNO 3 Which reactant is limiting, assuming we started with 30.0 grams of ammonium
More informationAT Chapter 3 Notes 15.notebook. September 29, Measuring Atomic Masses
Measuring Atomic Masses Mass Spectrometer used to isolate isotopes of an element and determine their mass. 1 An element sample is heated to vaporize it and the gaseous atoms are zapped with an electron
More informationLaw of Conservation of Mass
Chapter Chemical Reactions Quantities Law of Conservation of Mass.7 Mole Relationships in Chemical Equations Conservation of Mass The Law of Conservation of Mass indicates that in an ordinary chemical
More informationUnit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C12 and C13. Of Carbon s two isotopes, there is 98.9% C12 and 11.1% C13. Find
More informationChemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
More informationChapter 8: Quantities in Chemical Reactions
Ch 8 Page 1 Chapter 8: Quantities in Chemical Reactions Stoichiometry: the numerical relationship between chemical quantities in a balanced chemical equation. Ex. 4NH 3 + 5O 2 4NO + 6H 2 O The reaction
More informationChapter 9. Slide 1. Slide 2. Slide 3. Chemical Quantities. Table of Contents
1 Chapter 9 Chemical Quantities 2 Chapter 9 Table of Contents 9.1 Information Given by Chemical Equations 9.2 9.3 Copyright Cengage Learning. All rights reserved 2 3 Section 9.1 Information Given by Chemical
More informationMOLAR MASS AND MOLECULAR WEIGHT Themolar mass of a molecule is the sum of the atomic weights of all atoms in the molecule. Molar Mass.
Counting Atoms Mg burns in air (O 2 ) to produce white magnesium oxide, MgO. How can we figure out how much oxide is produced from a given mass of Mg? PROBLEM: If If 0.200 g of Mg is is burned, how much
More informationChemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
More information2 NO + O 2 2 NO 2 3/18/2014. iclicker Participation Question: A B C
Today: Stoichiometric Analysis: Gram to Gram Conversions: Use MOLAR MASS to get to moles Limiting Reagents: Method 1 Method 2 Actual Yield & Percent Yield Combustion Analysis Titrations Next Meeting Reading
More informationSample Problem: STOICHIOMETRY and percent yield calculations. How much H 2 O will be formed if 454 g of. decomposes? NH 4 NO 3 N 2 O + 2 H 2 O
STOICHIOMETRY and percent yield calculations 1 Steps for solving Stoichiometric Problems 2 Step 1 Write the balanced equation for the reaction. Step 2 Identify your known and unknown quantities. Step 3
More informationChapter 3 Chemical Reactions and Reaction Stoichiometry. 許富銀 ( Hsu FuYin)
Chapter 3 Chemical Reactions and Reaction Stoichiometry 許富銀 ( Hsu FuYin) 1 Stoichiometry The study of the numerical relationship between chemical quantities in a chemical reaction is called stoichiometry.
More informationSubscripts and Coefficients Give Different Information
Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Chemical equations (Balancing REVIEW) 2. Some simple patterns of reactivity 3. Formula weights (REVIEW) 4. Avogadro's
More information10 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
More informationChapter 4: Chemical and Solution Stoichiometry
Chapter 4: Chemical and Solution Stoichiometry (Sections 4.14.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances
More informationBalance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O
Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1
More informationCalculations 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 1024 g Atomic weight: Average mass of all isotopes of a given
More information1. How many hydrogen atoms are in 1.00 g of hydrogen?
MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 1024 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?
More informationChemical Reactions, Counting Atoms, and Balancing Chemical Equations.
Chemical Reactions, Counting Atoms, and Balancing Chemical Equations. A Chemical Reaction is A process where one or more elements or compounds are changed into one or more different substances A process
More information2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant.
UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in
More information4. Magnesium has three natural isotopes with the following masses and natural abundances:
Exercise #1 Atomic Masses 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. In a sample that contains 90.0% new and 10.0% old pennies,
More informationChem 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
More informationTuesday, October 23rd. Review Quiz Finish Chapter 6, Begin Chapter 7 Group Assignment
Tuesday, October 23rd Review Quiz Finish Chapter 6, Begin Chapter 7 Group Assignment 1 Review 2 Naming Ionic Compounds  When a metal is bonded to a nonmetal: 1. Name the metal. 2. Name the anion, use
More information1. P 2 O 5 2. P 5 O 2 3. P 10 O 4 4. P 4 O 10
Teacher: Mr. gerraputa Print Close Name: 1. A chemical formula is an expression used to represent 1. mixtures, only 3. compounds, only 2. elements, only 4. compounds and elements 2. What is the total number
More informationChapter 7: Chemical Reactions: An Introduction. Chemical Reactions, Equations and Balancing
Chapter 7: Chemical Reactions: An Introduction Chemical Reactions, Equations and Balancing Learning Target Chapter 7 Vocabulary 4 words 1. Chemical reaction 2. Reactant 3. Product 4. Coefficients balanced
More informationLecture 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 1024 g How many 12 C atoms weigh 12 g?
More informationThe Mole Concept. The Mole. Masses of molecules
The Mole Concept Ron Robertson r2 c:\files\courses\111020\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
More informationChemical 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
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change CHAPTER 11 Table Of Contents Chapter 11: Stoichiometry Section 1 Section 1 Section 1 Section 1 Describe the types of relationships indicated by a balanced chemical equation.
More informationChapter 1 The Atomic Nature of Matter: Selected Answersc for Practice Exam.
Chapter 1 The Atomic Nature of Matter: Selected Answersc for Practice Exam. MULTIPLE CHOICE 50. 5.80 g of dioxane (C 4 H 8 O 2 ) is how many moles of dioxane? 0.0658 mol 0.0707 mol 0.0725 mol d. 0.0804
More informationChapter 3! Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry
Chapter 3! : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2
More informationWe 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
More information1. Given the following chemical equation, answer the questions that follow.
Problems to practice on Chapter 6 1. Given the following chemical equation, answer the questions that follow. A. Balance the equation. CH 3 OH (l) + O 2(g) CO 2(g) + H 2 O (g) Balancing Organic formulas
More informationLimiting Reagent Worksheet #1
Limiting Reagent Worksheet #1 1. Given the following reaction: (Balance the equation first!) C 3 H 8 + O 2 > CO 2 + H 2 O a) If you start with 14.8 g of C 3 H 8 and 3.44 g of O 2, determine the
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationStoichiometry. 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
More informationLecture Notes Chemistry E1. Chapter 3
Lecture Notes Chemistry E1 Chapter 3 http://inserbia.info/news/wpcontent/uploads/2013/05/tamiflu.jpg http://nutsforhealthcare.files.wordpress.com/2013/01/tamiflumoa.jpg The Mole A mole is a certain
More informationChemical Reactions. Chemistry 100. Bettelheim, Brown, Campbell & Farrell. Introduction to General, Organic and Biochemistry Chapter 4
Chemistry 100 Bettelheim, Brown, Campbell & Farrell Ninth Edition Introduction to General, Organic and Biochemistry Chapter 4 Chemical Reactions Chemical Reactions In a chemical reaction, one set of chemical
More informationChapter Three: STOICHIOMETRY
p70 Chapter Three: STOICHIOMETRY Contents p76 Stoichiometry  The study of quantities of materials consumed and produced in chemical reactions. p70 31 Counting by Weighing 32 Atomic Masses p78 Mass Mass
More informationMoles. 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
More informationMetals Topic Test. Part 1: Multiple Choice Choose the best alternative and indicate your response on the answer sheet
Metals Topic Test Part 1: Multiple Choice Choose the best alternative and indicate your response on the answer sheet 1. The chemical equation for the reaction between aluminium and oxygen is: 4Al (s) +
More informationAP Chemistry. Unit #3. Chapter 3 Zumdahl
AP Chemistry Unit #3 Chapter 3 Zumdahl Stoichiometry C6H12O6 + 6 O2 6 CO2 + 6 H2O Students should be able to: Calculate the atomic weight (average atomic mass) of an element from the relative abundances
More informationLecture 5 Outline. Derived from the Greek stoicheion ( element ) and metron ( measure )
Lecture 5 Outline 5.1 Stoichiometry,, the mole etc. 5.2 Chemical Equations 5.3 Molarity 5.4 Limiting reagents and yields 5.5 Reaction enthalpies and Gibbs free energy 5.6 Catalyst Lecture 5 Stoichiometry
More informationFormulas, Equations, and Moles. + "reacts with" "to produce" Equations must be balanced. Equal amounts of each element on each side of the equation.
Chapter 3 Formulas, Equations, and Moles Chemical Equations 2 2 + 2 2 2 reactants products + "reacts with" "to produce" coefficients  indicate amount of substance Equations must be balanced. Equal amounts
More informationUnit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationPercent Yield = Actual yield of product x 100% Theoretical yield of product
Yields of Chemical Reactions In the stoichiometry examples so far we have made the unstated assumption that the reaction goes to completion, that all reactants are converted to products. In actual fact,
More informationChapter 7: Stoichiometry  Mass Relations in Chemical Reactions
Chapter 7: Stoichiometry  Mass Relations in Chemical Reactions How do we balance chemical equations? How can we used balanced chemical equations to relate the quantities of substances consumed and produced
More informationMOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]
MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH
More informationSample 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.
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationChapter 3 Calculation with Chemical Formulas and Equations
Chapter 3 Calculation with Chemical Formulas and Equations Practical Applications of Chemistry Determining chemical formula of a substance Predicting the amount of substances consumed during a reaction
More informationIB Chemistry 1 Mole. One atom of C12 has a mass of 12 amu. One mole of C12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon12 that were needed to make 12 g of carbon. 1 mole
More informationChapter 6 Quantities in Chemical Reactions
Chapter 6 Quantities in Chemical Reactions The Meaning of a Balanced Chemical Equation MoleMole Conversions MassMass Conversions Limiting Reactants Percent Yield Energy Changes Copyright The McGrawHill
More informationStoichiometry. What is the atomic mass for carbon? For zinc?
Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon12
More informationSTOICHIOMETRY ANALOGY
STOICHIOMETRY ANALOGY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant
More informationdealing with relationships between the amounts of reactants and products
I. Stoichiometry I. Stoichiometry = a quantitative study dealing with relationships between the amounts of reactants and products in a chemical reaction. I. Stoichiometry Comes from the Greek words stoicheion,
More informationThe Mole, Avogadro s Number, and Molar Mass
The Mole, Avogadro s Number, and Molar Mass Example: How many atoms are present in 2.0 kg of silver? (1 amu = 1.6605402x1024 g) Example: How many molecules are present in 10. mg of smelling salts, (NH
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter Molar mass and the mole one mole is defined as the number of carbon atoms in exactly 1.000000 grams of pure 1C. From the sugar example, a mole of C 1 H
More informationIs it still balanced? Has anything changed? What does it mean? Is it still balanced? Has anything changed? What does it mean?
Chemistry 11 Unit VII Stoichiometry Introduction: Let s look at the following equation 2 H 2 + O 2 2 H 2 O The numbers in front of the H 2 and H 2 O are called coefficients. What do they tell us? They
More informationChemistry Stoichiometry. 45 points. Do not turn page until told to do so.
Chemistry 2010 Stoichiometry 45 points Do not turn page until told to do so. Stoichiometry Multiple Choice (Each worth 2 points) Identify the letter of the choice that best completes the statement or
More informationChemical Composition. Introductory Chemistry: A Foundation FOURTH EDITION. Atomic Masses. Atomic Masses. Atomic Masses. Chapter 8
Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Chemical Composition Chapter 8 1 2 Atomic Masses Balanced equation tells us the relative numbers of molecules
More informationStudent Exploration: Chemical Equations
Name: Date: Student Exploration: Chemical Equations Vocabulary: Avogadro s number, chemical equation, chemical formula, chemical reaction, coefficient, combination, combustion, conservation of matter,
More informationThe Mole and Molar Mass
The Mole and Molar Mass 1 Molar mass is the mass of one mole of a substance. Molar mass is numerically equal to atomic mass, molecular mass, or formula mass. However the units of molar mass are g/mol.
More information2 Stoichiometry: Chemical Arithmetic Formula Conventions (1 of 24) 2 Stoichiometry: Chemical Arithmetic Stoichiometry Terms (2 of 24)
Formula Conventions (1 of 24) Superscripts used to show the charges on ions Mg 2+ the 2 means a 2+ charge (lost 2 electrons) Subscripts used to show numbers of atoms in a formula unit H 2 SO 4 two H s,
More information