Ch 9. Stoichiometry. The recipe of chemistry
|
|
- Christopher Bradley
- 5 years ago
- Views:
Transcription
1 Ch 9 Stoichiometry The recipe of chemistry
2 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. Write the balanced equation for making cake: à cake mix cups oil cup water + 2 eggs à 1.0 cake 2. If you have 2 cake mixes, 2 cups oil, 3 cups water, 4 eggs, how many cakes can you make, what and how much is left over? 2
3 1.0 cake mix cups oil cup water + 2 eggs à 1.0 cake Calculating Cakes Calculate the number of cakes (Ck) that can be made from 12 cake mixes (Cm) 12Cm x 1 Ck = 12 Ck 1 Cm Calculate the number of cakes (Ck) that can be made from 10.0 cups of oil (Oi) 10.0 Oi x 1 Ck = 20 Ck 0.5Oi If you need to make 29 cakes (Ck), how many eggs (Eg) do you need? 29 Ck x 2 Eg = 58 Eg 1 Ck
4 Stoichiometry: the calculation of quantities in chemical reactions Equations are a chemist s recipe. Eqs tell chemists what amounts of reactants to mix and what amounts of products to expect. When you know the quantity of onesubstance in a rxn, you can calculate the quantity of any other substance consumed or created in the rxn.
5 Why should you care? Nearly everything we use is manufactured from chemicals. Soaps, shampoos, conditioners, CD s, cosmetics, medications, clothes. u For a manufacturer to make a profit the chemical processes carried out in industry must be economical u A balanced equation is needed and used so chemicals are not wasted when making products
6 Reading Chemical Equations How would you read: N 2 (g) + H 2 (g) à NH 3 (g) Balance and read: N 2 (g) + 3H 2 (g) à 2NH 3 (g) Coefficients can represent different possible units Atoms/molecules Moles Mass in grams Mass of reactants equals mass of products Law of Conservation of mass Liters (if compound is a gas at STP)
7 N 2 + 3H 2 2NH 3 1 mol N mol N 2 2 mol NH g N (2.0 g H 2 ) 2 (17.0 g NH 3 ) 22.4 L 34.0 g reactants L L 34.0 g products 22.4 L N L H L NH 3 L L L
8
9 MOLE ratios: What are the possible mole ratios in: N 2 (g) + 3H 2 (g) à 2NH 3 (g) 1 mole of N 2 reacts with 3 moles of H 2 to produce 2 moles of NH 3. Possible mole ratios for this formula: 1N 2 1N 2 3H 2 3H 2 2NH 3 2NH 3 Reaction to form ammonia in this 1:3:2 ratio. Mole ratios are CONVERSION FACTORS! Once you have the ratios, you can perform calcs. (a.k.a. STOICHIOMETRY)
10 Conversion of Quan66es in Moles Amount of given (mol) Mole ra6o: from balanced equa6on X Mole unknown = Mole given Amount of unkown (mol) Pg 305 Ex: How many moles of water are produced from 5.80 moles of oxygen gas? O 2 + H 2 à H 2 O 1. Write equa6on 2. Balance! 3. Set up conversion factor O 2 + 2H 2 à 2H 2 O 5.80mole O 2 x 11.6 moles water 2 mol H 2 O 1 mol O 2
11 N 2 (g) + 3H 2 (g) à 2NH 3 (g) 1. How many moles of ammonia are produced from 0.60 moles of N 2? (1.2 mol NH 3 ) 2. How many moles of H 2 are needed to react with 0.43 moles of N 2 gas? (1.3 mol H 2 ) 3. How many moles of H 2 are needed to produce 1.98 moles of ammonia (NH 3 )? (2.97 mol H 2 )
12 Amount of given (mol) Mole ra6o: from balanced equa6on X Mole unknown = Mole given Amount of unkown (mol) 4. Ammonia, NH 3 is a widely used fer6lizer and used in household cleaners. How many moles of ammonia are produced when 6 mol of H gas react with excess nitrogen gas? 4 mol NH 3 5. The decomposi6on of potassium chlorate, KClO 3 into potassium chloride and oxygen gas is used as a source of oxygen in the lab. How many moles of potassium chlorate are needed to produce 15 mol of oxygen gas? 1. Write equa6on 2. Balance! 3. Set up conversion factor 10 mol KClO 3
13 Ch 9.1 Historical Chemistry: pg 303, #1-2
14 End day
15 Sn + 2HF à SnF 2 + H 2 1. How many moles of SnF 2 will be produced by 12.5 moles of HF? 2. How many moles HF are needed to produce 6.85 moles of SnF 2?
16 Calculating using MASS quantities No lab balance measures moles directly, instead grams is a more practical unit. To calculate grams: 1. convert to moles first, then grams Using our same example, you can calculate how many grams of each compound: N 2 (g) + 3H 2 (g) à 2NH 3 (g) REMEMBER: when you use a gram/mole conversion factor: 1 mol = molar mass 1 mol 2 mol NH 3.00 g N 2 x x 3 x 28g 1 mol N 2 17 g 1 mol
17
18 Conversion of amount in Moles & Mass Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Par>cle B Mass B Volume B Ex 1: What mass, in grams, of glucose is produced when 3.00 mol of water reacts with excess carbon dioxide to produce glucose and oxygen? 1. Write equa6on 2. Balance! 3. Set up conversa6on factor 6CO 2 + 6H 2 O à C 6 H 12 O 6 + 6O mol x 1 mol glucose 180.2g x 6 mol water 1 mole 90.1g glucose
19 examples Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Par>cle B Mass B Volume B 2. What mass of carbon dioxide is needed to react with 3.00 mol water? 6CO 2 + 6H 2 O à C 6 H 12 O 6 + 6O 2 3. How many moles of H 2 O are formed from a reac6on using 824g NH 3 is the reac6on: NH 3 + O 2 à NO + H 2 O (unbalanced) 4NH 3 + 5O 2 à 4NO + 6H 2 O 132g CO mol H 2 O
20 Sn + 2HF à SnF 2 + H 2 Warm up 1. How many moles of SnF 2 will be produced by 12.5 moles of HF? 2. How many moles HF are needed to produce 685g of SnF 2? 3. How many moles of Sn are needed to produce 2.50L of H 2 Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Par>cle B Mass B Volume B
21 Conversion of amount: Mass to Mass Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Ex 1: How many grams of SnF 2 are produced from the reac6on of 30.00g HF with Sn. Sn (s) + 2HF (g) à SnF 2(s) +H 2(g) Par>cle B Mass B Volume B 1 mol HF 30.00g HF x 20.0 g HF x 1 mol SnF 2 x 2 mol HF 156.7g SnF 2 1 mol SnF g SnF 2 2. How many grams of NH 4 NO 3 are required to produce 33.0g N 2 O? (the laughing gas needed for an anesthe6c in den6stry) 60.0g NH 4 NO 3 NH 4 NO 3(s) à N 2 O (g) + 2H 2 O (l) 3. How many molecules of oxygen gas are produced when 29.2 g of water is decomposed? (4.88 * molecules of O 2 )
22 More Problems to Practice 1. Carbon dioxide is produced from the synthesis of oxygen gas with carbon monoxide. Write and balance this chemical equation and then tell how many liters of oxygen gas are required to burn 3.86 liters of carbon monoxide. Assume STP. (1.93 L O 2 ) 2. How many grams of NH 4 NO 3 are required to produce 33.0g N 2 O? (the laughing gas needed for an anesthe6c in den6stry) NH 4 NO 3(s) à N 2 O (g) + 2H 2 O 60.0g NH (l) 4 NO 3 3. How much water in grams is produced in this reac6on? 27.0g H 2 O
23 Stoichiometry Practice Answer in classwork section of notebook: N 2 (g) + 3H 2 (g) à 2NH 3 (g) 1. Calculate the number of grams of ammonia produced by the reaction of 5.40 g of H 2 with N 2. (30.6 g NH 3 ) 2. Calculate the number of liters of N 2 needed in order to react with 0.78 moles of H 2. (5.8 L N 2 ) 3. Calculate the grams of N 2 needed in order to produce 9.23 x molecules of NH 3. (21.5 g N 2 ) Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Par>cle B Mass B Volume B
24 Stoichiometry Practice Answer in classwork section of notebook: N 2 (g) + 3H 2 (g) à 2NH 3 (g) 1. Calculate the number of grams of ammonia produced by the reaction of 5.40 g of H 2 with N 2. (30.6 g NH 3 ) 2. Calculate the number of liters of N 2 needed in order to react with 0.78 moles of H 2. (5.82 L N 2 ) 3. Calculate the grams of N 2 needed in order to produce 9.23 x molecules of NH 3. (21.5 g N 2 ) Pg 311 Section Review #4 (assume silver has +1 charge) pg 313 Practice #1 Pg 318 Section Review #1-3 (next class)
25 MOLE-MOLE RATIO You will ALWAYS use the new MOLE-MOLE ratio step to get you from where you are to where you are are going. Par>cle A Mass A Volume A 6.022x x10 23 Molar Mass Mole Mole Mole Molar Mass A Ratio B 22.4 L 22.4 L Par>cle B Mass B Volume B
26 More Problems to Practice Carbon dioxide is produced from the synthesis of oxygen gas with carbon monoxide. Write and balance this chemical equation and then tell how many liters of oxygen gas are required to burn 3.86 liters of carbon monoxide. Assume STP. (1.93 L O 2 )
27 Problems to Practice Aluminum reacts with oxygen to produce Aluminum Oxide. How many moles of aluminum are needed to form 3.7 moles of Aluminum Oxide? Write the balanced equation and solve. (7.4 mol Al)
28 More Problems to Practice How many molecules of oxygen gas are produced when 29.2 g of water is decomposed? The balanced chemical equation is given for you. Use your new mole map to solve. 2H 2 O electricityà 2H 2 + O 2 (4.88 * molecules of O 2 ) How many molecules of oxygen are produced by the decomposition of 6.54 g of Potassium Chlorate? The balanced chemical equation is given for you. Use your new mole map to solve. 2KClO 3 à 2KCl + 3O 2 (4.82 * molecules of O 2 )
29 Even More Problems Sodium hydroxide reacts with Sulfuric acid to produce water and Sodium Sulfate. Calculate the amount of water (in grams) that would be produced from g of the acid. (15.0 g H 2 O) In a combustion reaction, C 2 H 4 reacts with oxygen to produce H 2 O and CO 2 in the following reaction. Balance it and then determine the amount of oxygen (in grams) that is consumed if 2.69g of water is produced. C 2 H 4 + O 2 à CO 2 + H 2 O (7.17 g O 2 )
30 Mole to mass Amount of given (mol) Mole ra6o: (balanced equa6on) Molar mas: (periodic table) Mole unknown molar mass unknown(g) Mole given 1 mole unkown X x = mass of unkown (g) Mass of given (g) Molar mas: (periodic table) 1 mole given mol unknown molar mass mol given given (g) Mole ra6o: (balanced equa6on) X x = Amount unkown (mol)
31 Mass of given (g) X x X = 1 mole given mol unknown mole mass molar mass mol given 1 mol given (g) unknown mass of unknown (g)
32 End day
33 Warm up 1. Carbon dioxide is produced from the synthesis of oxygen gas with carbon monoxide. Write and balance this chemical equation and then tell how many liters of oxygen gas are required to burn 3.86 liters of carbon monoxide. Assume STP. (1.93 L O 2 ) Par>cle A 6.022x x10 23 Par>cle B Mass A Molar Mass Mole A Mole Ratio Mole B Molar Mass Mass B Volume A 22.4 L 22.4 L Volume B
34
35 How many sandwiches, how much excess?
36 Limiting Reagent (Ch. 9.3) Limiting reagent: reactant that determines the amount of product that can be produced. It limited Excess reagent: reactant that is not used up in the reaction - there is more available than needed Steps to determine LR Calculate theoretical yield (g or mol) Determine limited reagent Use the original actual yield of the limiting reactant to calculate product produced (in moles or grams)
37 Problems to Practice Ex 1. Given the following balanced equation, determine which is the LR if 2.70 moles of C 2 H 4 is reacted with 6.30 moles of O 2. How much water is made? C 2 H 4 + 3O 2 à 2H 2 O + 2CO 2 (O 2 is LR) 2.70 mol C 2 H 4 x 2 mole H 2 O = 5.4 mol H 2 O 1 mole C 2 H mol O 2 x 2 mole H 2 O = 4.20 mol O 2 3 mole O 2 Less= limi6ng reagent=o 2 2. Using the info gathered from above, calculate the GRAMS of water that will be produced. 4.20mol x 18g/mol = 75.6 g H 2 O
38 Warm Up #2 (March) 2H 2 + O 2 2H 2 + O 2 è 2Η 2 Ο è 2Η 2 Ο 3 O 2 & 7 H 2 1. How many mole of hydrogen molecules are needed to reac6on with one mole of oxygen molecules? 2. How many water molecules are produced if one mole of oxygen molecules completely reacts? 3. How many water molecules could form in container Q? 4. Which reactant (oxygen or hydrogen) limited the produc6on of water in container Q? 5. Which reactant (oxygen or hydrogen) was present in excess and remained aber the produc6on of water was complete??
39 Limi6ng Reactant More Problems to Practice 3. Identify the LR when 6.00 g HCl reacts with 5.00 g Mg in the following reaction: Mg + 2HCl à MgCl 2 + H 2 (HCl is LR) 4. Using the info gathered from above, calculate the GRAMS of hydrogen gas that will be produced. How much of the excess reactant is left? (0.164 g H 2 )
40 Flask Volume ace>c acid (ml) Demo 25ml 25ml 25ml 25ml 25ml 25ml Sodium bicarbona te (g) 0.50g 1.00g 1.50g 2.00g 2.50g 3.00g Which system will produce the most CO 2 product?
41 Theoretical yield vs Actual yield: Ch 9.3 The difference in the op6mal, expected outcome and the actual tested outcome Experimenta6on is not perfect Not all reactant are react so some may be leb over Condi6ons may not be perfect for a full reac6on Actual: get in an experiment Theore>cal: maximum produced in perfect theore6cal condi6ons
42 Percent Yield % yield = actual yield x 100% theoretical yield measure of the efficiency of a reaction carried out in lab. Actual yield would be given in problem or determined from actually performing the lab. Theoretical yield can be calculated using the Limiting Reagent.
43 Percent Yield: Problem to Practice If 15.0 g of nitrogen gas reacts with 15.0 g of hydrogen gas, 10.5 g of ammonia (NH 3 ) is produced. Calculate the percent yield. N 2 yields 1.07 mol NH 2 H 2 yields 5.0mol NH 2 Limiting reactant: N 2 (theoretical yield: 18.2 g NH 3 ) (percent yield: 57.7%) 1. Balance chemical equa>on 2. Find limi>ng reactant 3. Calculate theore>cal yield 4. Find percent yield % yield = actual yield x 100 theoretical yield
44 Stoichiometry Practice Answer in classwork section of notebook: N 2 (g) + 3H 2 (g) à 2NH 3 (g) 1. Calculate the number of grams of ammonia produced by the reaction of 5.40 g of H 2 with N 2. (30.6 g NH 3 ) 2. Calculate the number of liters of N 2 needed in order to react with 0.78 moles of H 2. (5.82 L N 2 ) 3. Calculate the grams of N 2 needed in order to produce 9.23 x molecules of NH 3. (21.5 g N 2 ) Pg 311 Section Review #4 (assume silver has +1 charge) pg 313 Practice #1 Pg 318 Section Review #1-3
45 Warm up 15.0 g Mg is used in the following reaction: Mg + 2HCl à MgCl 2 + H 2 1. Calculate the theore6cal yield, in grams, of hydrogen gas. 1.23g H 2 2. Calculate the percent yield if 1.15 grams of H 2 are produced. 93.5% Then con6nue Stoichiometry Prac6ce- classwork if not finished
46 True or False #1 The limi6ng reactant will be the reactant that produces the most product. (F)
47 True or False #2 To calculate percent yield, you must be given the actual yield and have to use the balanced equa6on to calculate the theore6cal yield (T)
48 True or False #3 Actual yield is 3.00g and theore6cal yield is 4.00g. What is the %yield? (75%)
49 I m not sure I ve got this.
50 More Review? Pg 325 Standardized Test Prep #1-12
51 Par>cle A 6.022x x10 23 Par>cle B Mass A Molar Mass Mole A Mole Ratio Mole B Molar Mass Mass B Volume A 22.4 L 22.4 L Volume B
52
53 Common Core Standards HS- PS1-7. Use mathema>cal representa>ons to support the claim that atoms, and therefore mass, are conserved during a chemical reac>on. HS- PS1-6. Refine the design of a chemical system by specifying a change in condi>ons that would produce increased amounts of products at equilibrium. HS- PS1-5. Apply scien>fic principles and evidence to provide an explana>on about the effects of changing the temperature or concentra>on of the reac>ng par>cles on the rate at which a reac>on occurs. HS- PS1-3. Plan and conduct an inves>ga>on to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between par>cles.
54 Common Core Standards HS- PS1-7. Use mathema>cal representa>ons to support the claim that atoms, and therefore mass, are conserved during a chemical reac>on. CA State Standards D2. Inves1gate quan1ta1ve rela1onships in chemical reac1ons, and solve related problems; D3. Demonstrate an understanding of the mole concept and its significance to the quan1ta1ve analysis of chemical reac1ons.
55 Common Core Standards HS- PS1-6. Refine the design of a chemical system by specifying a change in condi>ons that would produce increased amounts of products at equilibrium.
56 Common Core Standards HS- PS1-5. Apply scien>fic principles and evidence to provide an explana>on about the effects of changing the temperature or concentra>on of the reac>ng par>cles on the rate at which a reac>on occurs.
57 Common Core Standards HS- PS1-3. Plan and conduct an inves>ga>on to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between par>cles.
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
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 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 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 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 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 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 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 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 informationName. Academic Chemistry Stoichiometry Notes. Unit #10 Test Date: cincochem.pbworks.com
Name Academic Chemistry Stoichiometry Notes Unit #10 Test Date: cincochem.pbworks.com Resources Unit 10 Common Polyatomic Ions List 20 Name Common Polyatomic Ion Ions Name Ion acetate C 2 H 3 O 2 or CH3
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 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 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 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 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 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 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 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 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 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 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 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 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 informationStoichiometry. Stoichiometry. Calcula1ng Molecular Mass. Formula Stoichiometry. Chemical Reac1ons. Stoichiometry 10/3/09
Chemistry Preparatory Topics Lecture 5 Dr. Gondran Composi?on (Chemical Formula) Stoichiometry: The propor?ons of elements in stoichiometric compounds. In H 2 O, hydrogen and oxygen is 2:1. Reac?on (Chemical
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 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 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 informationCHAPTER 9 CHEMICAL QUANTITIES
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter
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 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 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 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 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 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. Goal. Calculate quantities of reactants and products needed in chemical rxns using balanced chemical equations.
Chapter 12 Stoichiometry Goal Calculate quantities of reactants and products needed in chemical rxns using balanced chemical equations. Using an Equation as a Recipe Ingredients: Frame, Seat, Wheels, Handlebar,
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 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 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 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 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 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 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 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 informationSeptember 18, reaction stoichiometry.notebook. May 18 10:07 AM. Sep 13 8:55 AM REACTION STOICHIOMETRY
REACTION STOICHIOMETRY COMPOSITION STOICHIOMETRY: The mass relationships of elements in a compound REACTION STOICHIOMETRY : the mass relationships between products and reactants May 18 10:07 AM Sep 13
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 informationWhat does this equation tell you? 1. 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to produce 2 molecules of ammonia gas.
Chapter 7 Quantities in Chemical Reactions Stoichiometry For example, the Haber Process (used to make ammonia gas) is based on the following balanced equation: N 2(g) + 3H 2(g) 2NH 3(g) Stoichiometry is
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. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas.
1 1. Interpreting Chemical Equations Stoichiometry Calculations using balanced equations are called stoichiometric calculations. The starting point for any problem involving quantities of chemicals in
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 informationCh 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated
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 informationUNIT 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 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 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 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 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. 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 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 informationChapter 3: Chemical Reactions and the Earth s Composition
Chapter 3: Chemical Reactions and the Earth s Composition Problems: 3.1-3.3, 3.5, 3.11-3.86, 3.95-3.115, 3.119-3.120, 3.122, 3.125-3.128, 3.132, 3.134, 3.136-3.138-3.141 3.2 The Mole Stoichiometry (STOY-key-OM-e-tree):
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 informationStoichiometry Chapter 9 Practice Assessment B
NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions:
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 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 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 informationGeneral Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction
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 informationStoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)
Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number
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 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 information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
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 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 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 informationChapter 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
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 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 informationName: 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
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 informationStoichiometry Practice Problems
Name Period CRHS Academic Chemistry Stoichiometry Practice Problems Due Date Assignment On-Time (100) Late (70) 9.1 9.2 9.3 9.4 9.5 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located on CRHS
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 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 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 informationUnit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations
Unit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations 1. Describe the following word equation with a statement or sentence: Iron + Oxygen iron (III) oxide 2. In a
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 informationSTOICHIOMETRY. Greek: Stoicheon = element metron = element measuring
STOICHIOMETRY Greek: Stoicheon = element metron = element measuring Stoichiometry is the science of measuring the quantitative proportions or mass ratios in which chemical elements stand to one another
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 informationHow did JJ Thomson conclude that the mobile charged particle in the atom had a ( ) charge.
Name Veritas Class Period Chemistry: Final Exam Practice Problems The final exam will focus on material covered in the spring semester. However, note that much of the material learned early in the year
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 informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More informationGeneral Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction
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 informationSpring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
More informationRight Side NOTES ONLY
Ch. 8 Stoichiometry Title and Highlight TN Ch 8.1 Topic: EQ: Right Side NOTES ONLY Date Write Question out (left side of red line) and answer it (Highlight answer) based on from what you read. Write out
More informationFunsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017
Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +
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 information9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses
9/14/1 Chemistry Second Edition Julia Burdge Stoichiometry: Ratios of Combination Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Stoichiometry: Ratios
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 informationPowerPoint 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
More informationEXTRA CREDIT REMINDER
EXTRA CREDIT REMINDER Due Tonight at Midnight (January 21 at 11:59 pm) via email kimberlyn.jackson@hcbe.net *** Kinesthetic: If you do not know how to use Prezi you may do a power point otherwise email
More informationStoichiometry ( ) ( )
Stoichiometry Outline 1. Molar Calculations 2. Limiting Reactants 3. Empirical and Molecular Formula Calculations Review 1. Molar Calculations ( ) ( ) ( ) 6.02 x 10 23 particles (atoms or molecules) /
More informationSummer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem
Summer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem 1, but AP Chem will be a little different. Rather than
More information