3.9 Stoichiometric Calcs: Amounts of Reactants and Products
|
|
|
- Ursula Ross
- 6 years ago
- Views:
Transcription
1 3.9 Stoichiometric Calcs: Amounts of Reactants and Products
2 Law of Conservation of Mass The Law of Conservation of Mass indicates that in an ordinary chemical reaction, Matter cannot be created nor destroyed. No change in total mass occurs in a reaction. Mass of products is equal to mass of reactants. Copyright Houghton Mifflin Company. All rights reserved. 3 2
3 Conservation of Mass 2 moles Ag + 1 moles S = 1 mole Ag 2 S 2 (107.9 g) + 1(32.1 g) = 1 (247.9 g) g reactants = g product Copyright Houghton Mifflin Company. All rights reserved. 3 3
4 Reading Equations In Moles Consider the following equation: 4 Fe(s) + 3 O 2 (g) 2 Fe 2 O 3 (s) This equation can be read in moles by placing the word moles between each coefficient and formula. 4 moles Fe + 3 moles O 2 2 moles Fe 2 O 3 Copyright Houghton Mifflin Company. All rights reserved. 3 4
5 Writing Mole-Mole Factors A mole-mole factor is a ratio of the moles for any two substances in an equation. 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) Fe and O 2 4 moles Fe and 3 moles O 2 3 moles O 2 4 moles Fe Fe and Fe 2 O 3 4 moles Fe and 2 moles Fe 2 O 3 2 moles Fe 2 O 3 4 moles Fe O 2 and Fe 2 O 3 3 moles O 2 and 2 moles Fe 2 O 3 2 moles Fe 2 O 3 3 moles O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 5
6 Learning Check Consider the following equation: 3 H 2 (g) + N 2 (g) 2 NH 3 (g) A. A mole-mole factor for H 2 and N 2 is 1) 3 moles N 2 2) 1 mole N 2 3) 1 mole N 2 1 mole H 2 3 moles H 2 2 moles H 2 B. A mole-mole factor for NH 3 and H 2 is 1) 1 mole H 2 2) 2 moles NH 3 3) 3 moles N 2 2 moles NH 3 3 moles H 2 2 moles NH 3 Copyright Houghton Mifflin Company. All rights reserved. 3 6
7 Solution 3H 2 (g) + N 2 (g) 2NH 3 (g) A. A mole-mole factor for H 2 and N 2 is 2) 1 mole N 2 3 moles H 2 B. A mole-mole factor for NH 3 and H 2 is 2) 2 moles NH 3 3 moles H 2 Copyright Houghton Mifflin Company. All rights reserved. 3 7
8 Calculations with Mole Factors How many moles of Fe 2 O 3 can form from 6.0 mole O 2? 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) Relationship: 3 mole O 2 = 2 mole Fe 2 O 3 Write a mole-mole factor to determine the moles of Fe 2 O mole O 2 x 2 mole Fe 2 O 3 = 4.0 mole Fe 2 O 3 3 mole O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 8
9 Guide to Using Mole Factors Copyright Houghton Mifflin Company. All rights reserved. 3 9
10 Learning Check How many moles of Fe are needed for the reaction of 12.0 moles O 2? 4 Fe(s) + 3 O 2 (g) 2 Fe 2 O 3 (s) 1) 3.00 moles Fe 2) 9.00 moles Fe 3) 16.0 moles Fe Copyright Houghton Mifflin Company. All rights reserved. 3 10
11 Solution 3) 16.0 moles Fe 12.0 moles O 2 x 4 moles Fe = 16.0 moles Fe 3 moles O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 11
12 Steps in Finding the Moles and Masses in a Chemical Reaction Copyright Houghton Mifflin Company. All rights reserved. 3 12
13 Moles to Grams Suppose we want to determine the mass (g) of NH 3 that can form from 2.50 moles N 2. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) The plan needed would be moles N 2 moles NH 3 grams NH 3 The factors needed would be: mole factor NH 3 /N 2 and the molar mass NH 3 Copyright Houghton Mifflin Company. All rights reserved. 3 13
14 Moles to Grams The setup for the solution would be: 2.50 mole N 2 x 2 moles NH 3 x 17.0 g NH 3 1 mole N 2 1 mole NH 3 given mole-mole factor molar mass = 85.0 g NH 3 Copyright Houghton Mifflin Company. All rights reserved. 3 14
15 Learning Check How many grams of O 2 are needed to produce mole Fe 2 O 3 in the following reaction? 4 Fe(s) + 3 O 2 (g) 2 Fe 2 O 3 (s) 1) 38.4 g O 2 2) 19.2 g O 2 3) 1.90 g O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 15
16 Solution 2) 19.2 g O mole Fe 2 O 3 x 3 mole O 2 x 32.0 g O 2 = 19.2 g O 2 2 mole Fe 2 O 3 1 mole O 2 mole factor molar mass Copyright Houghton Mifflin Company. All rights reserved. 3 16
17 Calculating the Mass of a Reactant The reaction between H 2 and O 2 produces 13.1 g water. How many grams of O 2 reacted? 2 H 2 (g) + O 2 (g) 2 H 2 O(g) The plan and factors would be? g 13.1 g g H 2 O mole H 2 O mole O 2 g O 2 molar mole-mole molar mass H 2 O factor mass O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 17
18 Calculating the Mass of a Reactant The setup would be: 13.1 g H 2 O x 1 mole H 2 O x 1 mole O 2 x 32.0 g O g H 2 O 2 moles H 2 O 1 mole O 2 molar mole-mole molar mass H 2 O factor mass O 2 = 11.6 g O 2 Copyright Houghton Mifflin Company. All rights reserved. 3 18
19 Learning Check Acetylene gas C 2 H 2 burns in the oxyacetylene torch for welding. How many grams of C 2 H 2 are burned if the reaction produces 75.0 g CO 2? 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(g) 1) 88.6 g C 2 H 2 2) 44.3 g C 2 H 2 3) 22.2 g C 2 H 2 Copyright Houghton Mifflin Company. All rights reserved. 3 19
20 Solution 3) 22.2 g C 2 H 2 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(g) 75.0 g CO 2 x 1 mole CO 2 x 2 moles C 2 H 2 x 26.0 g C 2 H g CO 4 moles CO mole C 2 H 2 molar mole-mole molar mass CO 2 factor mass C 2 H 2 = 22.2 g C 2 H 2 Copyright Houghton Mifflin Company. All rights reserved. 3 20
21 Calculating the Mass of Product When 18.6 g ethane gas C 2 H 6 burns in oxygen, how many grams of CO 2 are produced? 2 C 2 H 6 (g) + 7 O 2 (g) 4 CO 2 (g) + 6 H 2 O(g) 18.6 g? g The plan and factors would be g C 2 H 6 mole C 2 H 6 mole CO 2 g CO 2 molar mole-mole molar mass C 2 H 6 factor mass CO 2 Copyright Houghton Mifflin Company. All rights reserved. 3 21
22 Calculating the Mass of Product 2 C 2 H 6 (g) + 7 O 2 (g) 4 CO 2 (g) + 6 H 2 O(g) The setup would be 18.6 g C 2 H 6 x 1 mole C 2 H 6 x 4 moles CO 2 x 44.0 g CO g C 2 H 6 2 moles C 2 H 1 mole CO 6 2 molar mole-mole molar mass C 2 H 6 factor mass CO 2 = 54.4 g CO 2 Copyright Houghton Mifflin Company. All rights reserved. 3 22
23 Learning Check How many grams H 2 O are produced when 35.8 g C 3 H 8 react by the following equation? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g) 1) 14.6 g H 2 O 2) 58.4 g H 2 O 3) 117 g H 2 O Copyright Houghton Mifflin Company. All rights reserved. 3 23
24 Solution 2) 58.4 g H 2 O C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g) 35.8 g C 3 H 8 x 1 mole C 3 H 8 x 4 mole H 2 O x 18.0 g H 2 O = 58.4 g H 2 O 44.1 g C 3 H 8 1 mole C 3 H 8 1 mole H 2 O molar mole-mole molar mass C 3 H 8 factor mass H 2 O Copyright Houghton Mifflin Company. All rights reserved. 3 24
Chapter 5 Chemical Reactions Law of Conservation of Mass and Quantities 5.7 Mole Relationships in Chemical Equations
Chapter 5 Chemical Reactions and Quantities Law of Conservation of Mass 5.7 Mole Relationships in Chemical Equations The Law of Conservation of Mass indicates that in an ordinary chemical reaction, Matter
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 9 Chemical Quantities Information
STOICHIOMETRY is. Math-tastic! Let s make some Cookies! 2/21/2015
Math-tastic! Unit 9: Math of Chemistry Part II - Stoichiometry Lesson # 9.4: The Arithmetic of Equations Mr. Mole 87 STOICHIOMETRY is Greek for measuring elements Pronounced stoy-kee-ahm-uhtree Defined
3.7 Chem. Eqs & 3.8 Balancing Chem. Eqs
3.7 Chem. Eqs & 3.8 Balancing Chem. Eqs Chemical Equations A chemical equation gives the chemical formulas of the reactants on the left of the arrow and the products on the right. Reactants Product C(s)
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
Pearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world
Pearson Education Limited Edinburgh Gate Harlow Essex CM0 JE England and Associated Companies throughout the world Visit us on the World Wide Web at: www.pearsoned.co.uk Pearson Education Limited 014 All
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
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
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:
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
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.
Measuring and Expressing Enthalpy Changes. Copyright Pearson Prentice Hall. Measuring and Expressing Enthalpy Changes. Calorimetry
Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will learn to measure heat flow in
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
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)
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
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.
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
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 11. Unit 7 - Stoichiometry
1 Chemistry 11 Unit 7 - Stoichiometry 2 1. Coefficients of chemical equations In chapter 6, we have learned how to balance a chemical reaction by considering the laws of conservation of atoms and charges.
Chemistry Slide 1 of 33
Chemistry 17.2 1 of 33 17.2 Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will
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
Chemical Reactions and Stoichiometry. Ms. Grobsky
Chemical Reactions and Stoichiometry Ms. Grobsky Wrapping Up the Types of Chemical Reactions We just got done investigating the different types of chemical reactions We can now answer the two questions
Notes 2: Stoichiometry
Notes 2: Stoichiometry 1.1 Defining Stoichiometry Particle and Mole Relationships Chemical reactions stop when one of the reactants is used up. Stoichiometry is the study of quantitative relationships
9.1 Information Given by Chemical Equations 9.2 Mole Mole Relationships 9.3 Mass Calculations 9.4 The Concept of Limiting Reactants 9.
9.1 Information Given by Chemical Equations 9.2 Mole Mole Relationships 9.3 Mass Calculations 9.4 The Concept of Limiting Reactants 9.5 Calculations Involving a Limiting Reactant 9.6 Percent Yield mole-to-mole
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
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
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
CHEM 120: Introduction to Inorganic Chemistry. Chapters Covered and Test dates. The mole concept and atoms. Avogadro s number
CHEM 120: Introduction to Inorganic Chemistry Instructor: Upali Siriwardane (Ph.D., Ohio State University) CTH 311, Tele: 257-4941, e-mail: upali@chem.latech.edu Office hours: 10:00 to 12:00 Tu & Th ;
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
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
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.
7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.
Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation
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 Problems
Stoichiometry Problems 1. Consider the container label initial condition as the reactants before any reaction has occurred, and the container labeled final condition as the same container after the reaction
Name Date Class. Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line.
12 STOICHIOMETRY Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. 1. 2. 3. 4. 5. Column A the substance
Burning a Hydrocarbon II
Burning a Hydrocarbon II Name Lab Section Problem Statement: How are the masses of products limited by the amounts of reactants? I. Data Collection: A. Go to http://cheminfo.chem.ou.edu/~mra/home.html
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
Skill Building UNDERSTANDING AND BALANCING EQUATIONS
Skill Building UNDERSTANDING AND BALANCING EQUATIONS Equations are the language of chemistry, and they are important in helping us understand how atoms and molecules form new substances. It has been said
PowerPoint to accompany. Chapter 2. Stoichiometry: Calculations with Chemical Formulae and Equations. Dr V Paideya
PowerPoint to accompany Chapter 2 Stoichiometry: Calculations with Chemical Formulae and Equations Dr V Paideya Chemical Equations CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Figure 2.4 Chemical Equations
Stoichiometry. Before You Read. Chapter 10. Chapter 11. Review Vocabulary. Define the following terms. mole. molar mass.
Stoichiometry Before You Read Review Vocabulary Define the following terms. mole molar mass conversion factor dimensional analysis law of conservation of mass Chapter 10 Balance the following equation.
HOMEWORK 11-1 (pp )
CHAPTER 11 HOMEWORK 11-1 (pp. 333 335) VOCABULARY Define. 1. Gay-Lussac s law of combining volumes of gases 2. Avogadro s law Answer each question. 3. Write and explain the equation that expresses the
Session 6: LECTURE OUTLINE (SECTION M2 pp F88 - F90)
Session 6: LECTURE OUTLINE (SECTION M2 pp F88 - F90) I. The Limiting Reagent a. Stoichiometric amounts b. Non-Stoichiometric amounts c. Limiting reagent (L.R) II. III. How Do We Determine Which Is The
Chemical Equations. Chemical Equations
Page III-4a-1 / Chapter Four Part I Lecture Notes Chemical Reactions Chapter 4 Part 1 Chemistry as Cooking! - the Chemical Reaction "Recipe" and technique leads to successful creations Must know amounts
Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass,
Stoichiometry Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, volume, and heat of reaction. Stoichiometry
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
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
Usual Atomic Charges of Main Group Elements
Usual Atomic Charges of Main Group Elements +1 +2 +3 +4 +5 +6 +7-5 -4-3 -2-1 Examples SO 3 sulfur trioxide CO 2 carbon dioxide Al 2 O 3 aluminum trioxide IF 7 iodine heptafluoride Fig. 2-6, p.63 Chemical
Chapter 3 Stoichiometry. Ratios of combination
Chapter 3 Stoichiometry Ratios of combination Topics Molecular and formula masses Percent composition of compounds Chemical equations Mole and molar mass Combustion analysis (Determining the formula of
Chemical Reactions BIOB111 CHEMISTRY & BIOCHEMISTRY. Session 3
Chemical Reactions BIOB111 CHEMISTRY & BIOCHEMISTRY Session 3 Session Plan Physical & Chemical changes Chemical equations Balancing chemical equations Classification of chemical reactions Redox reactions
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 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
1. Making the invisible, visible. 2. Enabling the students to witness experiments that they cannot conduct themselves.
Lesson Plan Lesson: Gas Calculations Aim: To investigate the molar and reacting volumes of gases. Learning Outcomes : At the end of the lesson, students will be able to : 1. state the molar volumes of
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
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
Chemical Equations. Law of Conservation of Mass. Anatomy of a Chemical Equation CH4(g) + 2O2(g) Chapter 3
Chemical Equations Chemical equations are concise representations of chemical reactions. Chapter 3 : Calculations with Chemical Formulas and Equations Law of Conservation of Mass Anatomy of a Chemical
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
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
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
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
The Question (Learning Goals)
The Question (Learning Goals) What is the Law of Conservation of Mass (or atoms)? What is a balanced Chemical Reaction? How do we balance a chemical reaction?? (A Level) Review: Chemical Reactions Chemical
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Lecture Presentation
Lecture Presentation Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College Cottleville, MO Law of Conservation of Mass We may lay it down as an
Practice 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
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?!.!!
6/28/11. Avogadro s Number and the Mole. The Mole. The Mole. The Mole (mol)
Avogadro s Number and the Mole Molecular weight: The sum of atomic weights of all atoms in a molecule. Formula weight: The sum of atomic weights of all atoms in one formula unit of any compound. Mole:
Chapter 5. Stoichiometry
Chapter 5 Stoichiometry Chapter 5 Table of Contents (5-1) Counting by weighing (5-2) Atomic masses (5-3) Learning to solve problems (5-4) The mole (5-5) Molar mass (5-6) Percent composition of compounds
Chapter 8 Thermochemistry: Chemical Energy
Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be
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
Balancing Chemical Reactions. CHAPTER 3: Quantitative Relationships in Chemical Reactions. Zn + HCl ZnCl 2 + H 2. reactant atoms product atoms
CHAPTER 3: Quantitative Relationships in Chemical Reactions Stoichiometry: Greek for measure elements Stoichiometry involves calculations based on chemical formulas and chemical equations (reactions) quantitative.
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
Chemical Equations 10/30/13. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions
Chemical Equations A chemical equation just like a mathematical equation is a way to express, in symbolic form, the reactions occurring in a chemical system. n Balancing chemical equations n Reaction stoichiometry
, what volume of chlorine, measured at STP, reacts completely with 8 moles of gallium? A)
7- In the reaction,, what volume of chlorine, measured at STP, reacts completely with 8 moles of gallium? A) B) C) D) E) Explanation of the answer: In this mole-volume stoichiometry problem # 7 above we
CHAPTER 11 Stoichiometry Defining Stoichiometry
CHAPTER 11 Stoichiometry 11.1 Defining Stoichiometry Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry
Practice Problems Stoich!
Practice Problems Stoich! Name: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS
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
Reacting Masses 1 of 24 Boardworks Ltd 2016
Reacting Masses 1 of 24 Boardworks Ltd 2016 Reacting Masses 2 of 24 Boardworks Ltd 2016 What is a mole? 3 of 24 Boardworks Ltd 2016 A mole is an SI unit that is used to denote the number of atoms or molecules
Name: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2
Name: Class: _ Date: _ Chpt 12 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is conserved in the reaction shown below? H 2 + Cl 2 2HCl a.
Name Date Class THE ARITHMETIC OF EQUATIONS
Name Date Class 12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in
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
Thermochemistry Chapter 4
Thermochemistry Chapter 4 Thermochemistry is the study of energy changes that occur during chemical reactions Focus is on heat and matter transfer between the system and the surroundings Energy The ability
Section 1 Introduction to Stoichiometry. Describe the importance of the mole ratio in stoichiometric calculations.
Section 1 Introduction to Stoichiometry Objective Define stoichiometry. Describe the importance of the mole ratio in stoichiometric calculations. Write a mole ratio relating two substances in a chemical
Enthalpy Chapter 5.3-4,7
Enthalpy Chapter 5.3-4,7 heat transfer in (endothermic), +q heat transfer out (exothermic), -q SYSTEM E = q + w w transfer in (+w) w transfer out (-w) Internal Energy at Constant Volume E = E K + E P ΔE
A chemical reaction shows the process in which a substance (or substances) is changed into one or more new substances
A chemical reaction shows the process in which a substance (or substances) is changed into one or more new substances Chang, R. 2002. Chemistry 7 th ed. Singapore: McGraw-Hill. A chemical equation uses
Chapter 3 Molecules, Compounds, and Chemical Equations
Chapter 3 Molecules, Compounds, and Chemical Equations 3.7 Formula Mass versus Molar mass Formula mass The average mass of a molecule or formula unit in amu also known as molecular mass or molecular weight
Finding Formulas. using mass information about a compound to find its formula
Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula
Stoichiometry. A. The Meaning of Coefficients in a Reaction Equation 1. Consider the following reaction: 200 H O H 2 O or
Stoichiometry A. The Meaning of Coefficients in a Reaction Equation 1. Consider the following reaction: 2H 2 + O 2 2H 2 O The coefficients in the equation tell us that two hydrogen molecules react with
Chemical Formulas and Equations
Chemical Formulas and Equations 8.5D recognize that chemical formulas are used to identify substances and determine the number of atoms of each element in chemical formulas containing substances; 8.5F
Chem 1075 Chapter 10 Stoichiometry Lecture Notes
Chem 1075 Chapter 10 Stoichiometry Lecture Notes Slide 2 What is stoichiometry? Chemists and chemical engineers must perform calculations based on balanced chemical reactions to predict the cost of processes.
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 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
Chapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 9 REVIEW Stoichiometry SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. The coefficients in a chemical equation represent the (a) masses in grams of all reactants
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH Chapter Outline Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly.
Energy and Chemical Change
Energy and Chemical Change Section 15.1 Energy In your textbook, read about the nature of energy. In the space at the left, write true if the statement is true; if the statement is false, change the italicized
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
CH 221 Chapter Four Part I Concept Guide
1. Balancing Chemical Equations CH 221 Chapter Four Part I Concept Guide Description When chlorine gas, Cl 2, is added to solid phosphorus, P 4, a reaction occurs to produce liquid phosphorus trichloride,
Reactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of McGraw-Hill Education. Titrations In
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
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
Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in