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.
|
|
- Juliet Bryant
- 5 years ago
- Views:
Transcription
1 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 the study of the relative quantities of reactants and products in chemical reactions. It all begins with balanced chemical equations, which are essential for making calculations related to chemical reactions. 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. If we multiply each by 12 we could say: 1 dozen molecules of nitrogen gas reacts with 3 dozen molecules of hydrogen gas to produce 2 dozen molecules of ammonia gas. 2. If we wanted 100 molecules of ammonia gas, we would need 50 molecules of nitrogen gas and 150 molecules of hydrogen gas because the ratio is 1:3:2
2 4. If we multiply each by 6.02x10 23 we could say: 1 mole of nitrogen gas reacts with 3 moles of hydrogen gas to produce 2 moles of ammonia gas. The relationship between moles in a balanced chemical equation are known as MOLE RATIOS We use mole ratios to solve problems. 1. From the equation above, how much ammonia gas would be produced from 3.5 mol of hydrogen gas? 2. When carbon and oxygen combine 2 reactions are possible. The product can be CO 2 or CO. a. Write the balanced chemical equations. b. How much oxygen is needed to react with 0.75mol carbon to produce CO 2? c. How much oxygen is needed to react with 0.75mol carbon to produce CO?
3 Mole Ratios can also be used to find the mass ratios for chemical equations. N 2(g) + 3H 2(g) 2NH 3(g) If you know the amount of one substance in a chemical reaction (moles, particles, mass) you can calculate the amount of any other substances in the reaction using the BALANCED CHEMICAL EQUATION. Solving Stoichiometric Problems Follow this process: 1. Write a balanced equation. 2. If you are given the mass or # of particles of a substance, convert it to the # of moles. 3. Calculate the # of moles of the required substance based on the # of moles of the given substance, using mole ratios. 4. Convert the # of moles of the required substance to mass or # of particles. Ex 1. Mass to Mass Astronauts must be able to remove the CO 2 from their spacecraft. If not hypoxia (lack of O 2 ) would occur. CO 2 is removed using the following chemical reaction: CO 2(g) + 2LiOH (s) Li 2 CO 3(g) + H 2 O (g). If an astronaut produces 1.50x10 3 g of CO 2 a day, what mass of LiOH would be needed per day?
4 Ex 2. On Feb, 20, 2008 the US Navy shot down a spy satellite in space from a war ship in the Pacific ocean. They claimed the satellite contained hydrazine (rocket fuel), that could harm people if the satellite fell back to Earth. When hydrazine is combined with dinitrogen tetroxide it produces nitrogen gas and water. If 100g of hydrazine (N 2 H 4 ) is reacted, how much nitrogen gas would be produced? Ex 3. During WWI, chlorine gas was used as a weapon. When chlorine gas enters the lungs it reacts with water and forms corrosive hydrochloric acid and oxygen gas. How many molecules of chlorine react to produce 5.0g of HCl? Magnesium reacts with cuprous chloride in a single displacement reaction. How much magnesium is required to produce 200g of copper? The Limiting Reactant Chemical reaction equations give the ideal stoichiometric relationship among reactants and products. However, the reactants for a reaction in an experiment are not necessarily a stoichiometric mixture. What mass of cuprous chloride is needed?
5 In a chemical reaction, one of the reactants may not be used up when the reaction is finished. These are called excess reagents. The reagent that is completely used up or reacted is called the limiting reagent, because its quantity limit the amount of products formed. Think of when you put gas in your car: 2C 8 H O 2 16CO H 2 O Ideally, 25 moles of oxygen react with 2 moles of octane. But in reality O 2 is UNLIMITED in the air so octane would be the limiting reactant. When you run out of gas the reaction STOPS! In stoichiometric problems: IF YOU ARE GIVEN THE AMOUNTS OF 2 OR MORE REACTANTS, YOU MUST FIRST IDENTIFY THE LIMITING REACTANT!
6 Ex 1. Glucose reacts with oxygen gas to produce carbon dioxide and water during cellular respiration. If 1.25 g of glucose reacts with 7.51g of oxygen gas, find the limiting reactant. Warmup: 30g of aluminum oxide and 20g of water react to form aluminum hydroxide. What is the limiting reactant? Ex 2. A 2.00g piece of phosphorus is burned in a flask containing 6.91 g of oxygen gas. What mass of tetraphosphorus decaoxide is produced? Iron and carbon dioxide can be produced when iron(iii) oxide reacts with carbon monoxide gas. If 11.5 g of of iron(iii) oxide is reacted with 2.63x10 24 molecules of carbon monoxide, what mass of iron is expected?
7 Percentage Yield Chemists use stoichiometry to predict the amount of a product that can be expected from a chemical reaction. This amount is called the THEORETICAL YIELD. This amount is not always obtained. The actual amount obtained in an experiment is called the ACTUAL YIELD. The actual yield is usually less then the theoretical yield and for a variety of reasons. For example: a. Less than perfect collection techniques b. Competing reactions c. Poor experimental design d. Impure reactants % Yield = Actual Yield x100% Theoretical Yield Ex1. When 75g of nitrogen gas reacts with sufficient hydrogen gas, the theoretical yield of ammonia is 9.10 g. If 1.72 g of ammonia is obtained what is the percentage yield? PERCENTAGE YIELD compares the mass of product obtained by experiment (actual) to the mass predicted by stoichiometry (theoretical).
8 Ex 2. When Calcium carbonate is decomposed to calcium oxide and carbon dioxide there is a 92.4% yield of calcium oxide. How many grams of calcium oxide can you expect if 12.4 g of calcium carbonate is heated. % Purity is the percent of a specific compound in an impure substance.
UNIT 3 Chemical Quantities Chapter 5 Counting Atoms and Molecules The Mole
UNIT 3 Chemical Quantities Chapter 5 Counting Atoms and Molecules The Mole How does the mass of a substance relate to the number of atoms in the substance? Recall: Atomic mass units. Atomic mass units
More informationUNIT 3 Quantities in Chemical Reactions THE MOLE!
UNIT 3 Quantities in Chemical Reactions THE MOLE! In chemistry as in other aspects of life it is sometimes more convenient to count in groups of items rather than count items individually. Quantity Amount
More informationChapter 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
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationReading 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
More information2.9 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
More informationChapter 9: Stoichiometry The Arithmetic ti Of Equations
Chapter 9: Stoichiometry The Arithmetic of Equations Chemical Calculations Limiting Reagent and Percent Yield The Arithmetic ti Of Equations -- The Arithmetic of Equations -- Using Everyday Equations Stoichiometry
More informationAP 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
More informationUnit 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
More information**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
More informationBasic Concepts of Chemistry Notes for Students [Chapter 7, page 1] D J Weinkauff - Nerinx Hall High School
Basic Concepts of Chemistry Notes for Students [Chapter 7, page 1] Chapter 7 Quantitative Relationships in Chemical Reactions As you have begun to see, chemistry is a quantitative science involving a great
More informationStoichiometry 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
More informationQuantity 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
More informationStoichiometry 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
More informationOutcomes: 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
More informationUnit 7: Stoichiometry Homework Packet (85 points)
Name: Period: By the end of the Unit 7, you should be able to: Chapter 12 1. Use stoichiometry to determine the amount of substance in a reaction 2. Determine the limiting reactant of a reaction 3. Determine
More informationCHAPTER 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
More informationIf Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?
If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,
More informationNotes 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
More informationCounting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for
More informationCHAPTER 12: STOICHIOMETRY
Name: CHAPTER 12: STOICHIOMETRY Period: MOLE TO MOLE RATIO When nitrogen and hydrogen gas are heated under the correct conditions, ammonia gas (NH 3 ) is formed. a. RXN: 1N 2 + 3H 2 2NH 3 b. How many moles
More informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Table of Contents Click on the topic to go to that section Stoichiometry Calculations with Moles Stoichiometry Calculations with Particles
More informationChapter 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
More informationUnit 9 Stoichiometry Notes
Unit 9 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 to
More informationChapter 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
More information(DO NOT WRITE ON THIS TEST)
Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation
More informationName 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.
More informationStoichiometry 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
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Slide 4 / 109 Table of Contents Stoichiometry Calculations with Moles Click on the topic to go to that section Stoichiometry Calculations
More informationSection 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
More informationProportional Relationships
Stoichiometry Video Proportional Relationships 2 1/4 c. flour 1 tsp. baking soda 1 tsp. salt 1 c. butter 3/4 c. sugar 3/4 c. brown sugar 1 tsp vanilla extract 2 eggs 2 c. chocolate chips Makes 5 dozen
More informationChapter 3. Stoichiometry
Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average
More informationChapter 6 Chemical Reactions: Mole and Mass Relationships
Chapter 6 Chemical Reactions: Mole and Mass Relationships 6.1 The Mole and Avogadro s What is a Mole? - A Chemist s way of counting! - Cooks don t count out individual grains of sugar or rice when they
More informationName Date Class THE ARITHMETIC OF EQUATIONS
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 terms of interacting
More information1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?
Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of
More informationChemical 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
More informationUnit 6: React ions & St oichiom et ry, Chapt er s 11 & 12. Nam e: Period: Description Reaction Types Activty
Unit 6: React ions & St oichiom et ry, Chapt er s 11 & 12 Nam e: Period: Unit Goals- As you work through this unit, you should be able to: 1. Write formula equations from word equations using appropriate
More informationChapter 3 Test Bank. d. The decomposition of magnesium oxide produces 2.4 g of magnesium metal and 3.2 g of oxygen gas.
1. Which of the following correctly provides evidence for the unit formula of magnesium oxide? a. The decomposition of magnesium oxide produces 1.2 g of magnesium metal and 1.6 g of oxygen gas. b. The
More informationCh 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry
Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry Name /108 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing
More informationSTOICHIOMETRY. Measurements in Chemical Reactions
STOICHIOMETRY Measurements in Chemical Reactions STOICHIOMETRY Stoichiometry is the analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE-MOLE
More informationChapter 9 STOICHIOMETRY
Chapter 9 STOICHIOMETRY Section 9.1 The Arithmetic of Equations OBJECTIVE Calculate the amount of reactants required or product formed in a nonchemical process. Section 9.1 The Arithmetic of Equations
More informationSlide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»
Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent
More informationChemical Quantities: Stoichiometry and the Mole
Chemical Quantities: Stoichiometry and the Mole This is trying to summarize what we have learned up to this point: formulas, names, conversions, moles, quantities, reaction types, balancing equations,
More informationChapter 3 The Mole and Stoichiometry
Chapter 3 The Mole and Stoichiometry Chemistry, 7 th Edition International Student Version Brady/Jespersen/Hyslop Brady/Jespersen/Hyslop Chemistry7E, Copyright 015 John Wiley & Sons, Inc. All Rights Reserved
More information5.7 Quantity Relationships in Chemical Reactions (Stoichiometry)
5.7 Quantity Relationships in Chemical Reactions (Stoichiometry) We have previously learned that atoms combine in simple whole number ratios to form compounds. However, to perform a chemical reaction,
More informationName: Unit 9- Stoichiometry Day Page # Description IC/HW
Name: Unit 9- Stoichiometry Day Page # Description IC/HW Due Date Completed ALL 2 Warm-up IC 1 3 Stoichiometry Notes IC 1 4 Mole Map IC X 1 5 Mole to Mole Practice IC 1 6 Mass to Mole Practice IC 1/2 X
More informationName: 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.
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 informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More informationChapter 9. Table of Contents. Chapter 9. Lesson Starter. Chapter 9. Objective. Stoichiometry. Section 1 Introduction to Stoichiometry
Stoichiometry Table of Contents Section 1 Introduction to Stoichiometry Section 3 Limiting Reactants and Percentage Yield Section 1 Introduction to Stoichiometry Lesson Starter Mg(s) + 2HCl(aq)? MgCl 2
More informationChapter 12 Stoichiometry. Mr. Mole
Chapter 12 Stoichiometry Mr. Mole Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double or triple the amount
More informationLimiting Reactants. and Percentage Yield. Section 3
GO ONLINE Section 3 8E Main Ideas One reactant limits the product of a reaction. Comparing the actual and theoretical yields helps chemists determine the reaction s efficiency. 8E perform stoichiometric
More informationChem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 11.1 notes 1 MOLE = 6.02 x 10 23 representative particles representative particles
More informationStoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction.
Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting
More information7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.
Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation
More informationChapter 9. Preview. Lesson Starter Objective Stoichiometry Definition Reaction Stoichiometry Problems Mole Ratio Stoichiometry Calculations
Preview Lesson Starter Objective Stoichiometry Definition Reaction Stoichiometry Problems Mole Ratio Stoichiometry Section 1 Introduction to Stoichiometry Lesson Starter Mg(s) + 2HCl(aq) MgCl 2 (aq) +
More informationChapter 9. Stoichiometry. Mr. Mole. NB page 189
Chapter 9 Stoichiometry Mr. Mole NB page 189 review Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double
More informationPERCENT POTASSIUM CHLORATE IN A MIXTURE - Worksheet
35 PERCENT POTASSIUM CHLORATE IN A MIXTURE - Worksheet This lab will introduce the concept of reaction stoichiometry. We will use the mole ratios in a balanced chemical equation to calculate the amount
More informationStoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT
Unit 10 Resournces Name Academic Chemistry Stoichiometry Homework On-Time LATE DATE ASSIGNMENT 100 70 10.1 10.2 10.3 10.4 10.5 10.6 EC 16 cincochem.pbworks.com Stoichiometry Live in the now. Garth Algar
More informationCH. 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
More informationStoichiometry. Mr. Mole
Stoichiometry Mr. Mole Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double or triple the amount Thus, a
More informationChemistry Chapter 9. Unit 6 Stoichiometry
Chemistry Chapter 9 Unit 6 Stoichiometry The arithmetic of equations Equations are recipes. They tell chemists what amounts of reactants to mix and what amounts of products to expect. What is Stoichiometry?
More informationSlide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass
Stoichiometry HW Slide 1 / 90 Grade:«grade» Subject: ate:«date» 1 The calculation of quantities in chemical equations is called. Slide 2 / 90 accuracy and precision dimensional analysis percent composition
More informationCh. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles representative particles = ATOMS, IONS,
More informationChapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
More informationUnit IV: Stoichiometry
Unit IV: Stoichiometry D. Calculations from chemical equations 1. Mol-mol calculations 2. Mol-gram calculations 3. Gram-gram calculations E. Limiting reactant (or reagent) F. Other applications of stoichiometry
More informationUNIT 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
More informationTOPIC 4: THE MOLE CONCEPTS
TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationStoichiometry. 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.
More informationStoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction.
Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting
More informationName 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
More informationStoichiometry. The study of quantities of substances in chemical reactions
Stoichiometry The study of quantities of substances in chemical reactions Interpreting Chemical Equations N 2 + 3 H 2 2 NH 3 Particles: 1 molecule of Nitrogen reacts with 3 molecules of Hydrogen to produce
More informationUnit 3. Stoichiometry
Unit 3. Stoichiometry Upon successful completion of this unit, the students should be able to: 3.1 Define atomic mass and solve related problems. 1. Gallium has two naturally occurring isotopes, and gallium-70
More informationCHAPTER 12. Chemists use balanced to calculate how much reactant is needed or product is formed in a reaction. + 3H 2NH. Hon Chem 12.
CHAPTER 12 Stoichiometry is the calculation of quantities using different substances in chemical equations. Based on the Law of Conservation of Mass. Mg(s) + How many moles of H Chemists use balanced to
More informationStoichiometry study of the relationships in a
Note Taking Guide: Episode 801 Name Stoichiometry study of the relationships in a based on equations 2 Mg + O 2 2 MgO The in a give the for the involved in the. Ex. Problem: When elemental aluminum reacts
More informationUNIT 9 - STOICHIOMETRY
General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount
More informationUnit IV: Chemical Equations & Stoichiometry
Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations
More informationName 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
More informationTOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.
TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses
More informationreaction stoichiometry
2.10.12 If you decomposed 4 moles of hydrogen peroxide, how many moles of oxygen gas would you produce if you used manganese (IV) oxide as a catalyst? HW page 301 1-3, and page 311 1-4 TYGAGT Use mole
More informationUnit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction.
Unit 10: Stoichiometry Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Info given by a chemical equation: Chemical changes involve
More informationGraspIT AQA GCSE Quantitative changes
A. Chemical measurements part 1 Chemical changes and conservation of mass 1. A piece of magnesium was heated in a crucible. a) Write a balance equation to show how the magnesium reacts with oxygen. (2)
More informationChapter 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
More informationStoichiometry is the relationship between the amount of reactants used and the amount of products produced in a chemical reaction.
Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting
More informationApply 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
More informationVOCABULARY Define. 1. stoichiometry. 2. composition stoichiometry. 3. reaction stoichiometry. 4. unknown. 5. mole ratio
CHAPTER 9 HOMEWORK 9-1 (pp. 275 279) Define. 1. stoichiometry 2. composition stoichiometry 3. reaction stoichiometry 4. unknown 5. mole ratio SKILL BUILDER On a separate sheet of paper, write five possible
More informationStoichiometry. 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
More informationChapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry
Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are
More informationTHE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
THE MOLE - PART 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which one of the following statements is a quantitative observation? a.
More informationCalculations 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
More informationPractice 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
More informationChapter 3: STOICHIOMETRY: MASS, FORMULAS, AND REACTIONS
Chapter 3: STOICHIOMETRY: MASS, FORMULAS, AND REACTIONS Problems: 3.1-3.8, 3.11, 3.14-3.90, 3.103-3.120, 3.122-3.125, 3.128-3.131, 3.134, 3.137-36.138, 3.140-3.142 3.2 THE MOLE Stoichiometry (STOY-key-OM-e-tree):
More informationSTOICHIOMETRY. Engr. Yvonne Ligaya F. Musico 1
STOICHIOMETRY Engr. Yvonne Ligaya F. Musico 1 Stoichiometry The study in chemistry dealing with calculations based on balanced chemical equations. The branch of chemistry dealing with mass relationships
More informationCHAPTER 8. Stoichiometry
CHAPTER 8 Stoichiometry So far in your chemistry course, you have learned that chemists count quantities of elements and compounds in terms of moles and that they relate moles of a substance to mass by
More information( ) Natural Sciences Department. Chemical Reactions
Chemical Reactions Why do atoms cluster? The attraction which keeps atoms united one to each other to form a molecule is called chemical bond. The atoms place themselves in the molecule so that the energy
More informationChemistry 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:
More information