Stoichiometry. Goal. Calculate quantities of reactants and products needed in chemical rxns using balanced chemical equations.
|
|
- Olivia Smith
- 6 years ago
- Views:
Transcription
1 Chapter 12
2 Stoichiometry Goal Calculate quantities of reactants and products needed in chemical rxns using balanced chemical equations.
3 Using an Equation as a Recipe Ingredients: Frame, Seat, Wheels, Handlebar, Pedals Balanced equation: 1F + 1S + 2W + 1H + 2P 1 FSW 2 HP 2
4 How many pedals are needed to make 128 bicycles? 128 FSW 2 HP 2 2P 1 FSW2HP2 = 256 pedals 1F + 1S + 2W + 1H + 2P 1 FSW 2 HP 2
5 Examining a Balanced Chemical Equation 2H 2 S(g) + 3O 2 (g) 2SO 2 (g) + 2H 2 O(g) 2 moles of H 2 S reacts with 3 moles of O 2 to produce 2 moles of SO 2 and 2 moles of H 2 O. 4 moles of H 2 S reacts with moles 6 of O moles of O 2 are needed to produce 7 moles of H 2 O How to solve these is on the next slide.
6 Mole-Mole Ratio Problems 4 mol H 2 S 3 mole O 2 2 mol H 2 S = 6 mol O 2 7mol H 2 O 3 mole O 2 2 mol H 2 O = 10.5 mol O 2 The mol-mol ratio comes from the coefficients in the balanced equation. In the balance equation, O 2 has a coefficient of 3, H 2 O has a coefficient of 2, and H 2 S has a coefficient of 2.
7 Mass-Mass Calculation Write the balanced chemical equation Label above the equation what you are given and what you are trying to find. Convert grams of your given to moles using molar mass Multiply by the mole-mole ratio from the balanced chemical equation Convert moles of unknown to grams
8 Bringing It All Together How many grams of ammonia ( NH 3 ) should be produced when 6.00g nitrogen react with excess hydrogen? Solve: Write the balanced equation with the information labeled above it g excess? g N 2 + 3H 2 2 NH 3
9 Bringing It All Together Convert given to moles: 6.00g N 2 1 mole N 2 28 g N 2 = mol N 2 Multiply by the mole ratio: mol N 2 1 mol N2 2 mol NH 3 = mol NH 3
10 Wrapping It Up Convert moles of unknown to grams: mol NH 3 17g NH 3 1 mol NH 3 = 7.28g NH 3 Summary: When 6.00g of nitrogen(n 2 ) reacts with an excess of Hydrogen (H 2 ), 7.28g of ammonia (NH 3 ) should be produced.
11 Now You Try! What mass of aluminum is required to completely react with 7.80g oxygen in a synthesis reaction?
12 Write the balanced equation 4Al + 3O 2 2Al 2 O 3
13 Label your given and unknown information 7.80 g Since you were not given info about this compound, don t worry about it and don t use it. 4Al + 3O 2 2Al 2 O 3
14 NEXT?... Convert given to moles: 7.80g O 2 1 mol O 2 = 0.244mol O2 32g O 2 Multiply by the mole ratio: 0.244mol O 2 4 mol Al 3 mol O 2 = mol Al
15 AND FINALLY!! Convert moles of unknown to grams: mol Al 27g Al 1 mol Al = 8.78g Al 8.78g of aluminum (Al) should be required to react completely with7.80g of oxygen (O 2 ) in the synthesis of aluminum oxide (Al 2 O 3 ).
16 Mass-Volume Calculation Write the balanced chemical equation Label above the equation what you are given and what you are trying to find. Convert grams of your given to moles using molar mass Multiply by the mole-mole ratio from the balanced chemical equation Convert moles of unknown to liters (a.k.a dm 3 ) using molar volume (22.4L/ 1mol)
17 Bringing It All Together How many liters of oxygen are necessary for the combustion of 134g of magnesium, assuming the reactions occurs at STP? Solve: Write the balanced equation with the information labeled above it. 134 g? L 2Mg + O 2 2 MgO
18 Bringing It All Together Convert given to moles: 134g Mg 1 mole Mg 24.3 g Mg Multiply by the mole ratio: = mol Mg mol Mg 1 mol O 2 2 mol Mg = mol O 2
19 Wrapping It Up Convert moles of unknown to liters: molo LO 2 1 mol O 2 = 61.8 L O L of O 2 are required to completely combust 134g Mg in the synthesis of MgO.
20 Volume-Mass Calculation Write the balanced chemical equation Label above the equation what you are given and what you are trying to find. Convert liters of your given to moles using molar volume Multiply by the mole-mole ratio from the balanced chemical equation Convert moles of unknown to grams using molar mass
21 Bringing It All Together Find the mass of sulfur (S 8 ) required to react with oxygen to produce 2.47L of sulfur dioxide gas at STP. Solve: Write the balanced equation with the information labeled above it.? g 2.47L S O 2 8 SO 2
22 Bringing It All Together Convert given to moles: 2.47L SO 2 1 mole SO L SO 2 = mol SO 2 Multiply by the mole ratio: mol SO 2 1 mol S 8 8 mol SO2 = mol S 8
23 Wrapping It Up Convert moles of unknown to grams: mol S 8 256g S 8 1 mol S 8 = 3.53 g S g of sulfur (S 8 ) are required to produce 2.47 L of sulfur dioxide (SO 2 ).
24 Volume-Volume Calculations Write the balanced chemical equation Label above the equation what you are given and what you are trying to find. Convert liters of your given to moles using molar volume (22.4L/1mol) Multiply by the mole-mole ratio from the balanced chemical equation Convert moles of unknown to liters using molar volume (22.4L/1 mol)
25 Bringing It All Together What volume of H 2 S gas is needed to produce 14.2 L of water at STP? Solve: Write the balanced equation with the information labeled above it.?l 14.2L 2H 2 S + 3O 2 2 SO H 2 O
26 Bringing It All Together Convert given to moles: 14.2 L H 2 O 1 mole H 2 O 22.4 L H 2 O Multiply by the mole ratio: = mol H 2 O mol H 2 O 2 mol H 2 S 2mol H 2 O = mol H 2 S
27 Wrapping It Up Convert moles of unknown to liters: mol H 2 S 22.4 LH 2 S 1 mol H 2 S = 14.2 L H 2 S 14.2 L of H 2 S are required to produce 14.2 L H 2 O.
Chemistry 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 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 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 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 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 information9.1 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
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 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 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.
More informationCHAPTER 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
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 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 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 informationSTOICHIOMETRY. 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
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 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 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 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 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 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 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 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 informationChemical Reactions and Stoichiometry. Ms. Grobsky
Chemical Reactions and Stoichiometry Ms. Grobsky Wrapping Up the Lab As we know, the function of the airbags is to protect the occupant from injuring themselves by hitting against the windshield, steering
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 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 informationIdeal Gas & Gas Stoichiometry
Ideal Gas & Gas Stoichiometry Avogadro s Law V a number of moles (n) V = constant x n Constant temperature Constant pressure V 1 /n 1 = V 2 /n 2 Ammonia burns in oxygen to form nitric oxide (NO) and water
More informationStoichiometry. 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
More informationChemical Reactions. Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions. (ionic equations and solubility rules)
Chemical Reactions Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions (ionic equations and solubility rules) Writing Equations REACTANTS PRODUCTS gold (III) sulfide is
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 informationStoichiometry. 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.
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 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 informationSTOICHIOMETRY 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
More informationName 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
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. 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 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 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 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 informationTopic 1 Review. Ms. Kiely Coral Gables Senior High IB Chemistry SL
Topic 1 Review Ms. Kiely Coral Gables Senior High IB Chemistry SL Bell-Ringer A 4 g sample of sodium hydroxide, NaOH, is dissolved in water and made up to 500 cm³ of aqueous solution. What is the concentration
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. 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 informationMoles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How
More informationHonors 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
More informationCalculations From Chemical Equations
Calculations From Chemical Equations Chapter 9 Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons, Inc. A Short Review 2 The molar mass of an element
More informationUNIT 1 Chemical Reactions Part II Workbook. Name:
UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the
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 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 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 informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
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 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 informationSTOICHIOMETRY ANALOGY
STOICHIOMETRY ANALOGY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant
More 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 informationPercent 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
More informationChapter 7: Stoichiometry in Chemical Reactions
Chapter 7: Stoichiometry in Chemical Reactions Mini Investigation: Precipitating Ratios, page 315 A. ZnCl 2 (aq) + Na 2 CO 3 (aq) ZnCO 3 (s) + 2 NaCl(aq) 3 AgNO 3 (aq) + Na 3 PO 4 (aq) Ag 3 PO 4 (s) +
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 informationStoichiometry 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
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 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 informationCh 9. Stoichiometry. The recipe of chemistry
Ch 9 Stoichiometry The recipe of chemistry Warm up Analogy Suppose you are preparing a cake. Each Cake (Ck) requires 1.0 cake mix (Cm), 0.5 cup of oil (Oi), 1.0 cup of water (Wa) and 2.0 eggs (Eg). 1.
More informationUnit VI Stoichiometry. Applying Mole Town to Reactions
Unit VI Stoichiometry Applying Mole Town to Reactions Learning Goals I can apply mole town to reactions to determine the amount of product based on the amount of a reactant. I can apply mole town to reaction
More informationStoichiometry 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
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 informationExample Exercise 10.1 Interpreting Chemical Equation Calculations
Example Exercise 10.1 Interpreting Chemical Equation Calculations Given the chemical equation for the combustion of methane, CH 4, balance the equation and interpret the coefficients in terms of (a) moles
More informationFrom Greek: stoicheion (= element) metron (= measure)
Stoichiometry Chapter 12 the relationship between the relative quantities of substances taking part in a reaction or forming a compound, typically a ratio of whole integers. Origin From Greek: stoicheion
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 informationGuide for Reading. chemical equations. Vocabulary stoichiometry. Section 12.1 The Arithmetic of Equations 353
12.1 The Arithmetic of Equations Connecting to Your World Silk is one of the most beautiful and luxurious of all fabrics. It is spun from the cocoons of silkworms. Silk manufacturers know from experience
More informationHow many molecules are in 0.25 moles of CH 4?
Mass Moles- Particle Particles can be atoms, molecules, ions, etc. In one mole of particles, there are 6.02x10 23 particles These particles are so small and we need so many of them to be on a human scale,
More informationPOGIL- Stoichiometry How do chemists use balanced chemical equations?
POGIL- Stoichiometry How do chemists use balanced chemical equations? What happened to Avogadro when he got bit by 6.02 x 10 23 mosquitoes? He got Mol-aria Why? Chemists use balanced chemical equations
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 informationSolutions 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.
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 informationChemical Quantities: Stoichiometry. UNIT 4: Ch. 12 Ms. Kiely, Coral Gables Senior High
Chemical Quantities: Stoichiometry UNIT 4: Ch. 12 Ms. Kiely, Coral Gables Senior High 1 BELL RINGER How many moles are in 62.0g of hydrogen gas? ANSWER How many moles are in 62.0g of hydrogen gas? 30.7
More informationSupplemental Activities. Module: States of Matter. Section: Reaction Stoichiometry Key
Supplemental Activities Module: States of Matter Section: Reaction Stoichiometry Key Balancing Chemical Reactions Activity 1 The purpose of this activity is to check your understanding of the concept Law
More informationNOTES: 10.3 Empirical and Molecular Formulas
NOTES: 10.3 Empirical and Molecular Formulas What Could It Be? Empirical Formulas Indicate the lowest whole number ratio of the atoms in a compound: 1) Determine moles of each element present in the compound
More informationIdeal 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
More informationQuestions Q1. Which of the following contains the greatest number of hydrogen atoms? 2 moles of water, H 2 O. B 1.5 moles of ammonia, NH 3
Questions Q1. Which of the following contains the greatest number of hydrogen atoms? 2 moles of water, H 2 O B 1.5 moles of ammonia, NH 3 C 1 mole of hydrogen gas, H 2 D 0.5 moles of methane, CH 4 Q2.
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 informationStudent Version Notes: Unit 5 Moles & Stoichiometry
Name: Regents Chemistry: Mr. Palermo Student Version Notes: Unit 5 Moles & Stoichiometry Name: KEY IDEAS A compound is a substance composed of two or more different elements that are chemically combined
More information9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 )
Homework Stoichiometry 1.) An oxide of iron has the formula Fe 3 O 4. What mass percent of iron does it contain? (72.360%) 2.) Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed
More informationToday is Tuesday, May (!) 1 st, 2018
In This Lesson: Stoichiometry (Lesson 4 of 4) Today is Tuesday, May (!) 1 st, 2018 Stuff You Need: Calculator Periodic Table Pre-Class: How does an airbag work? In solving a problem of this sort, the grand
More informationChapter 11. Molecular Composition of Gases
Chapter 11 Molecular Composition of Gases PART 1 Volume-Mass Relationships of Gases Avogadro s Law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Recall
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 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 informationChemical 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
More informationBalancing Chemical Equations Stoichiometry. Packet #24
Balancing Chemical Equations Stoichiometry Packet #24 Introduction When baking cookies, there is a high probability that one would use a recipe. The recipe is used to indicate how much of each ingredient
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 informationEquation Stoichiometry.notebook. November 23, 2015
1 The coefficients in a balanced chemical equation represent moles of reactants and moles of products. The mole ratio (or proportion) of reactants and products in a balanced equation must remain constant.
More informationNotes: Unit 7 Moles & Stoichiometry
Regents Chemistry: Notes: Unit 7 Moles & Stoichiometry 1 KEY IDEAS In all chemical reactions there is a conservation of mass, energy, and charge. (3.3a) A balanced chemical equation represents conservation
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 informationUsual 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
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 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 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 information1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq)
1) Write the reaction for Calcium and nitrogen reacting 3) What element on the periodic table is the largest? 3)Name these a) H2S (aq) b) HNO 3 (aq) Stoichiometry: mathematical relationships in formulas
More informationStoichiometry Ch. 11. I. Stoichiometric Calculations
Stoichiometry Ch. 11 I. Stoichiometric Calculations Background on things you NEED to know how to do: 1. Name/write correct chemical formula 2. Write chemical equations 3. Balance chemical equations 4.
More informationCH 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,
More information