Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
|
|
|
- Winifred Brown
- 6 years ago
- Views:
Transcription
1 Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois
2 Chapter 9 Chemical Quantities
3 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers of reacting molecules and product molecules. 2 CO + O 2 2 CO 2 2 CO molecules react with 1 O 2 molecules to produce 2 CO 2 molecules Copyright Houghton Mifflin Company. All rights reserved. 9 3
4 Information Given by the Chemical Equation Since the information given is relative: 2 CO + O 2 2 CO CO molecules react with 100 O 2 molecules to produce 200 CO 2 molecules 2. 2 billion CO molecules react with 1 billion O 2 molecules to produce 20 billion CO 2 molecules 3. 2 moles CO molecules react with 1 mole O 2 molecules to produce 2 moles CO 2 molecules moles CO molecules react with 6 moles O 2 molecules to produce 12 moles CO 2 molecules Copyright Houghton Mifflin Company. All rights reserved. 9 4
5 Information Given by the Chemical Equation The coefficients in the balanced chemical equation show the molecules and the mole ratio of the reactants and products. Since moles can be converted to masses, we can determine the mass ratio of the reactants and products as well. Copyright Houghton Mifflin Company. All rights reserved. 9 5
6 Information Given by the Chemical Equation 2 CO + O 2 2 CO 2 2 moles CO = 1 mole O 2 = 2 moles CO 2 Since 1 mole of CO = g, 1 mole O 2 = g, and 1 mole CO 2 = g 2(28.01) g CO = 1(32.00) g O 2 = 2(44.01) g CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 6
7 Example #1 Determine the number of moles of carbon monoxide required to react with 3.2 moles oxygen, and determine the moles of carbon dioxide produced. Copyright Houghton Mifflin Company. All rights reserved. 9 7
8 Example #1 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 8
9 Example #1 (cont.) Use dimensional analysis: Copyright Houghton Mifflin Company. All rights reserved. 9 9
10 Example #2 Determine the number of moles of carbon monoxide required to react with 3.2 moles oxygen, and determine the moles of carbon dioxide produced. Copyright Houghton Mifflin Company. All rights reserved. 9 10
11 Example #2 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Determine the molar mass of each: 1 mol CO = g 1 mol O 2 = g 1 mol CO 2 = g Copyright Houghton Mifflin Company. All rights reserved. 9 11
12 Example #2 (cont.) Use the molar mass of the given quantity to convert it to moles. Use the mole relationship to convert the moles of the given quantity to the moles of the desired quantity: Copyright Houghton Mifflin Company. All rights reserved. 9 12
13 Example #2 (cont.) Use the molar mass of the desired quantity to convert the moles to mass: Copyright Houghton Mifflin Company. All rights reserved. 9 13
14 Limiting and Excess Reactants Limiting reactant: a reactant that is completely consumed when a reaction is run to completion Excess reactant: a reactant that is not completely consumed in a reaction Theoretical yield: the maximum amount of a product that can be made by the time the limiting reactant is completely consumed Copyright Houghton Mifflin Company. All rights reserved. 9 14
15 Example #3 Determine the number of moles of carbon dioxide produced when 3.2 moles oxygen reacts with 4.0 moles of carbon monoxide. Copyright Houghton Mifflin Company. All rights reserved. 9 15
16 Example #3 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 16
17 Example #3 (cont.) Use dimensional analysis to determine the number of moles of reactant A needed to react with reactant B: Copyright Houghton Mifflin Company. All rights reserved. 9 17
18 Example #3 (cont.) Compare the calculated number of moles of reactant A to the number of moles given of reactant A. If the calculated moles is greater, then A is the limiting reactant; if the calculated moles is less, then A is the excess reactant. The calculated moles of CO (6.4 moles) is greater than the given 4.0 moles; therefore CO is the limiting reactant. Copyright Houghton Mifflin Company. All rights reserved. 9 18
19 Example #3 (cont.) Use the limiting reactant to determine the moles of product: Copyright Houghton Mifflin Company. All rights reserved. 9 19
20 Example #4 Determine the mass of carbon dioxide produced when 48.0 g of oxygen reacts with 56.0 g of carbon monoxide. Copyright Houghton Mifflin Company. All rights reserved. 9 20
21 Example #4 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Determine the molar mass of each: 1 mol CO = g 1 mol O 2 = g 1 mol CO 2 = g Copyright Houghton Mifflin Company. All rights reserved. 9 21
22 Example #4 (cont.) Determine the moles of each reactant: Copyright Houghton Mifflin Company. All rights reserved. 9 22
23 Example #4 (cont.) Determine the number of moles of reactant A needed to react with reactant B: Copyright Houghton Mifflin Company. All rights reserved. 9 23
24 Example #4 (cont.) Compare the calculated number of moles of reactant A to the number of moles given of reactant A. If the calculated moles is greater, then A is the limiting reactant; if the calculated moles is less, then A is the excess reactant. The calculated moles of O 2 (1.00 moles) is less than the given 1.50 moles; therefore O 2 is the excess reactant. Copyright Houghton Mifflin Company. All rights reserved. 9 24
25 Example #4 (cont.) Use the limiting reactant to determine the moles of product, then the mass of product: Copyright Houghton Mifflin Company. All rights reserved. 9 25
26 Percent Yield Most reactions do not go to completion. Actual yield: the amount of product made in an experiment Percent yield: the percentage of the theoretical yield that is actually made Percent Yield = Actual Yield Theoretical Yield x 100% Copyright Houghton Mifflin Company. All rights reserved. 9 26
27 Example #4a If in the last problem 72.0 g of carbon dioxide is actually made, what is the percentage yield? Copyright Houghton Mifflin Company. All rights reserved. 9 27
28 Example #4a (cont.) Divide the actual yield by the theoretical yield, then multiply by 100% The actual yield of CO 2 is 72.0 g The theoretical yield of CO 2 is 88.0g Copyright Houghton Mifflin Company. All rights reserved. 9 28
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 8 Chemical Composition
3.9 Stoichiometric Calcs: Amounts of Reactants and Products
3.9 Stoichiometric Calcs: Amounts of Reactants and Products Law of Conservation of Mass The Law of Conservation of Mass indicates that in an ordinary chemical reaction, Matter cannot be created nor destroyed.
3.6 Determining the Formula of a Compound
3.6 Determining the Formula of a Compound Molecular compounds Copyright Houghton Mifflin Company. All rights reserved. 3 2 Formulas molecular formula = (empirical formula) n [n = integer] Ex. (CH 5 N)
Quantity Relationships in Chemical Reactions
Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 13 Gases Properties of
Chapter 3. Mass Relations in Chemistry; Stoichiometry
Chapter 3 Mass Relations in Chemistry; Stoichiometry Copyright 2001 by Harcourt, Inc. All rights reserved. Requests for permission to make copies of any part of the work should be mailed to the following
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY Work directly from Zumdahl (Chapter 3). Work through exercises as required, then summarise the essentials of the section when complete. A chemical equation is
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 5 Nomenclature Common Names
Calculations with Chemical Formulas and Equations
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 the chemist
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Stoichiometry. Please take out your notebooks
Stoichiometry Please take out your notebooks Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.
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
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
2.9 The Mole and Chemical Equations:
2.9 The Mole and Chemical Equations: Stoichiometry Whether you are making omelettes in a kitchen or soap in a factory, you need to know the quantities of ingredients required to produce a certain quantity
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 12 Chemical Bonding Structure
Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry
Stoichiometry The quantitative study of reactants and products in a chemical reaction 1 Stoichiometry Whether the units given for reactants or products are moles, grams, liters (for gases), or some other
Name Date Class STUDY GUIDE FOR CONTENT MASTERY
Stoichiometry Section 12.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1. The study of the quantitative relationships
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Chemistry I Chapter 9 Stoichiometry Objective Sheet. Equation 1. Objectives: 1. Define stoichiometry
Chemistry I Chapter 9 Stoichiometry Objective Sheet Equation 1 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O (g), at STP C 2 H 2 (acetylene) 26 g/mol O 2 32 g/mol CO 2 44 g/mol H 2 O 18 g/mol Objectives:
Chapter 9. Chemical Quantities
Chapter 9 Chemical Quantities Section 9.1 Information Given by Chemical Equations A balanced chemical equation gives relative numbers (or moles) of reactant and product molecules that participate in a
Chapter 12 Stoichiometry
12.2 Chemical Calculations > Chapter 12 Stoichiometry 12.1 The Arithmetic of Equations 12.22 Chemical Calculations 12.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates.
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Lecture Outline 3.1 Chemical Equations The quantitative nature of chemical formulas and reactions is called stoichiometry. Lavoisier
Ideal Gas Law Stoichiometry
Assume you had the following, simple, chemical reaction: A B Volume of A (in Liters) Mass of A (in grams) Atoms, Molecules, or Particles of A Divide by Molar Mass Divide by 22.4L/mol Moles of A Divide
General Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
Reacting Masses and Volumes Thursday 09/24/15
Reacting Masses and Volumes Thursday 09/24/15 Agenda Start Topic 1.3 Reacting Masses and Volume Topic 1.3 Reacting masses and volumes Quiz next Wednesday on Topic 1.2: Stoichiometry Study guide and practice
STOICHIOMETRY HONORS CHEMISTRY
STOICHIOMETRY HONORS CHEMISTRY MOLE RATIO A mole ratio is the ratio of coefficients used to compare amounts of reactants and products. 1 ZnCl 2 (aq) + 2 NaOH (aq) 1 Zn(OH) 2 (aq) + 2 NaCl (aq) What is
Stoichiometry. Cartoon courtesy of NearingZero.net
Stoichiometry Cartoon courtesy of NearingZero.net Stoichiometry In solving a problem of this sort, the grand thing is to be able to reason backward. This is a very useful accomplishment, and a very easy
Chapter 9. Slide 1. Chemical Quantities. Slide 2. 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 3 Copyright Cengage Learning. All rights reserved 2 Section 9.1 Information Given by Chemical
Chapter 4. Chemical Quantities and Aqueous Reactions
Chapter 4 Chemical Quantities and Aqueous Reactions Stoichiometry The study of the numerical relationship between chemical quantities in a chemical reaction Making Pizza The number of pizzas you can make
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
11 Stoichiometry. Section 11.1 What is stoichiometry?
11 Stoichiometry Section 11.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1.. 3. 4. 5. The study of the quantitative
Module 5: Combustion Technology. Lecture 32: Fundamentals of thermochemistry
1 P age Module 5: Combustion Technology Lecture 32: Fundamentals of thermochemistry 2 P age Keywords : Heat of formation, enthalpy change, stoichiometric coefficients, exothermic reaction. Thermochemistry
When is chemical equilibrium? Let s look at a reaction. Why do we care? CO2 (aq) + H2O(l) H2CO3(aq) two examples. what is the product?
When is chemical equilibrium? Why do we care? two examples What is happening to the acidity of the ocean? How does ibuprofen work? Let s look at a reaction CO2 (aq) + H2O(l) H2CO3(aq) what is the product?!.!!
9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses
9/14/1 Chemistry Second Edition Julia Burdge Stoichiometry: Ratios of Combination Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Stoichiometry: Ratios
Formula Mass. not all compounds are molecular formula mass calculated exactly the same way as molecular mass. Solid structure of NaCl
Molecular Mass Molecular Mass synonymous with molar mass and molecular weight is the sum of the atomic masses of all the atoms in a molecule the mass in grams of one mole of a compound Formula Mass not
9.2 Chemical Calcualtions. Chapter 9 Stoichiometry. 9.1 The Arithmetic of Equations. 9.2 Chemical Calculations. 9.3 Limiting Reagent and Percent Yield
9.2 Chemical Calcualtions Chapter 9 Stoichiometry 9.1 The Arithmetic of Equations 9.2 Chemical Calculations 9.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates.
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
91 PERCENTAGE COMPOSITION
91 PERCENTAGE COMPOSITION - sometimes called "percent composition" or "percent composition by mass" - the percentage of each element in a compound, expressed in terms of mass Example: Find the percentage
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
STOICHIOMETRY. STOICHIOMETRY Chemists use balanced chemical equations to calculate how much reactant is needed or how much product is formed.
STOICHIOMETRY Stoikheion = element; metron = to measure STOICHIOMETRY Chemists use balanced chemical equations to calculate how much reactant is needed or how much product is formed. provides the same
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
CHEMICAL CALCULATIONS - RELATING MASS AND ATOMS
CHEMICAL CALCULATIONS - RELATING MASS AND ATOMS Chemical equations are written and balanced in terms of ATOMS and MOLECULES - While chemical equations are written in terms of ATOMS and MOLECULES, that's
Chapter 4: Chemical and Solution Stoichiometry
Chapter 4: Chemical and Solution Stoichiometry (Sections 4.1-4.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances
Lesson 22: Theoretical Yield Actual Yield Percent Yield
Lesson 22: Theoretical Yield Actual Yield Percent Yield Do Now (5pts) 3.20.8 Copy down info from CJ board. Answer questions in Box of Lesson 22 note packet. You have a test in one week it ll be multiple
Chapter 9. Calculations from Chemical Equations. to patients Introduction to General, Organic, and Biochemistry 10e throughout the
Chapter 9 Calculations from Chemical Equations Accurate measurement and calculation of the correct dosage are important in dispensing the correct medicine to patients Introduction to General, Organic,
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
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
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,
Chapter 9 Stoichiometry
Chapter 9 Stoichiometry Section 9.1 Intro to Stoichiometry 9.1 Objectives Define stoichiometry. Describe the importance of the mole ratio in stoichiometric calculations. Write a mole ratio relating two
Chapter 3 Calculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Contents and Concepts Mass and Moles of Substances Here we will establish a critical relationship between the mass of a chemical substance and
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
UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY
UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance
Equilibrium. Chapter How Reactions Occur How Reactions Occur
Copyright 2004 by Houghton Mifflin Company. Equilibrium Chapter 16 ll rights reserved. 1 16.1 How Reactions Occur Kinetics: the study of the factors that effect speed of a rxn mechanism by which a rxn
Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages )
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.
9.1 The Arithmetic of Equations > Chapter 9 Stoichiometry. 9.1 The Arithmetic of Equations. 9.2 Chemical Calculations
Chapter 9 Stoichiometry 9.1 The Arithmetic of Equations 9.2 Chemical Calculations 9.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. CHEMISTRY
Chapter 5. Question. Question. Answer. Answer. Question (continued) The Gaseous State
Chapter 5 CRS s The Gaseous State Equal volumes of propane, C 3 H 8, and carbon monoxide at the same temperature and pressure have the same a. density. b.. c. number of atoms. 1) a only 2) b only 3) c
Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product?
Unit 6: Stoichiometry How do manufacturers know how to make enough of their desired product? Chocolate Chip Cookies Using the following recipe, complete the questions. Cookie Recipe 1.5 c sugar 1 c. butter
Chemistry I Notes Unit 7: Stoichiometry Notes
Chemistry I Notes Unit 7: Stoichiometry Notes Stoichiometry Relating Mass to Numbers of Atoms The Mole The mole is the SI unit for amount of substance. A mole (abbreviated mol) is the amount of a substance
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
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,
AP Chemistry: Chapter 3 Notes Outline
AP Chemistry: Chapter 3 Notes Outline Objectives: Balance chemical equations Use dimensional analysis to solve stoichiometric problems Use dimensional analysis to do limiting reactant problems Use dimensional
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
Stoichiometry. Chapter 3
Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry: The study of quantities of materials consumed and produced in chemical reactions. In macroworld, we can count objects by weighing assuming
AP CHEMISTRY SCORING GUIDELINES
Mean 5.64 out of 9 pts AP CHEMISTRY Question 1 CO(g) + 1 2 O 2 (g) CO 2 (g) 1. The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change,
CHAPTER 9: STOICHIOMETRY
9.1 Interpreting a chemical Equation CHAPTER 9: STOICHIOMETRY H 2 (g) + Cl 2 (g) 2 HCl (g) 1 molecule 1 molecule 2 molecules N 2 + 3 H 2 (g) 2 NH 3 (g) molecule(s) molecule(s) molecule(s) It follows that
CHEMISTRY 102B Practice Hour Exam I. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts)
CHEMISTRY 102B Practice Hour Exam I Spring 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 17 questions on 5 numbered pages. Check now to make sure you have a complete exam. You have one hour
Chemical Reactions. Chapter 17
Chemical Reactions Chapter 17 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Some equations
Chapter 9. Chemical Calculations and Chemical Formulas
Chapter 9 Chemical Calculations and Chemical Formulas Chapter Map Making Phosphoric Acid Furnace Process for making H 3 PO 4 to be used to make fertilizers, detergents, and pharmaceuticals. React phosphate
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
Chemistry. Chapter 17
Chemistry Chapter 17 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Balancing Chemical
Reading Balanced Chemical Equations (see MHR Text p )
Reading Balanced Chemical Equations (see MHR Text p. 114 118) 2 H 2(g) + O 2(g) 2 H 2 O (l) Read: 2 molecules of hydrogen gas reacts with 1 molecule of oxygen gas to produce 2 molecules of water or 2 moles
Quantitative Relationships in Chemical Reactions Chapter 7
Quantitative Relationships in Chemical Reactions Chapter 7 The burning of charcoal releases heat (thermal energy) that grills our food. But the combustion of charcoal and fossil fuels also releases CO
The change in enthalpy accompanying many reactions can be experimentally measured using calorimetry.
1. Hess s Law Students: investigate Hess s Law in quantifying the enthalpy change for a stepped reaction using standard enthalpy change data and bond energy data, for example: - carbon reacting with oxygen
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
Solutions to the Extra Problems for Chapter 8
Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.
Stoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
Chemical Equilibrium
Chemical Equilibrium Chemical Equilibrium When compounds react, they eventually form a mixture of products and unreacted reactants, in a dynamic equilibrium. A dynamic equilibrium consists of a forward
Stoichiometry Part I
Stoichiometry Part I Name Section DCI10.2. The equation for the reaction is 2S(g) + 3O 2 (g) ---> 2SO 3 (g) Consider a mixture of sulfur atoms and dioxygen molecules in a closed container below: Which
4.3.1 Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
4.3 Quantitative chemistry Chemists use quantitative analysis to determine the formulae of compounds and the equations for reactions. Given this information, analysts can then use quantitative methods
Stoichiometry World of Chemistry: Chapter 9
Stoichiometry World of Chemistry: Chapter 9 Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups all-purpose flour 1 teaspoon
Mass Relationships in Chemical Reactions
Reading Assignments: Chapter 3 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Mass Relationships in Chemical Reactions Or Related topics in other textbooks. Consultation outside lecture room: Office
**continued on next page**
Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants
CHEMISTRY Matter and Change
CHEMISTRY Matter and Change CHAPTER 11 Table Of Contents Section 11.1 Defining Chapter 11: Section 11.2 Section 11.3 Section 11.4 Percent Yield SECTION11.1 Defining Defining Particle and Mole Relationships
Lecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
Ch 1-6 Working With Numbers; Scientific Notation pp Ch 1-5 to 1-6 Significant Figures pp 22-37
Ch 1-5 to 1-6 Significant Figures pp 22-37 Know how significant digits are found and used in calculations. Ch 1-6 Working With Numbers; Scientific Notation pp 30-32 Know how to use the calculator exponent
Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations
Stoichiometry Table of Contents Section 1 Introduction to Stoichiometry Section 2 Ideal Stoichiometric Calculations Section 3 Limiting Reactants and Percentage Yield Section 1 Introduction to Stoichiometry
What does this equation tell you? 1. 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to produce 2 molecules of ammonia gas.
Chapter 7 Quantities in Chemical Reactions Stoichiometry For example, the Haber Process (used to make ammonia gas) is based on the following balanced equation: N 2(g) + 3H 2(g) 2NH 3(g) Stoichiometry is
CH. 12 STOICHIOMETRY
CH. 12 STOICHIOMETRY Balanced Chemical Equations Used to calculate: How much of each reactant is needed How much product will form If you know one quantity you can calculate the rest. Quantity may be in
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)
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
Notes: Stoichiometry (text Ch. 9)
Name Per. Notes: Stoichiometry (text Ch. 9) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to get missing information
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 10 Chemical Equation Calculations by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 10 1 What
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units )
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units ) N A 6.0 10 mol -1 1 mol substance contains N A Molar mass (g/mol)
4.3 Quantitative chemistry
4.3 Quantitative chemistry Chemists use quantitative analysis to determine the formulae of compounds and the equations for reactions. Given this information, analysts can then use quantitative methods
Percent yield Combustion analysis. General Chemistry I Dr. Stone Chapter 3 clicker 5
Percent yield Combustion analysis General Chemistry I Dr. Stone Chapter 3 clicker 5 % Yield = Actual x 100% Theoretical Actual= what is made Theoretical = the amount that could be made from the limiting
Chapter 3. Stoichiometry. Copyright 2018 Cengage Learning. All Rights Reserved.
Chapter 3 Stoichiometry Chapter 3 Table of Contents (3.1) (3.2) (3.3) (3.4) (3.5) (3.6) Counting by weighing Atomic masses The mole Molar mass Learning to solve problems (can read on own, not responsible
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
LIMITING REAGENT. Taking Stoichiometric conversions one step further
LIMITING REAGENT Taking Stoichiometric conversions one step further Limiting Reagent The reactant that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant