Chapter 9. Calculations from Chemical Equations. to patients Introduction to General, Organic, and Biochemistry 10e throughout the
|
|
- Conrad York
- 6 years ago
- Views:
Transcription
1 Chapter 9 Calculations from Chemical Equations Accurate measurement and calculation of the correct dosage are important in dispensing the correct medicine to patients Introduction to General, Organic, and Biochemistry 10e throughout the John Wiley & Sons, Inc world. Morris Hein, Scott Pattison, and Susan Arena
2 Chapter Outline 9.1 A Short Review 9.2 Introduction to Stoichiometry 9.3 Mole-Mole Calculations 9.4 Mole-Mass Calculations 9.5 Mass-Mass Calculations 9.6 Limiting Reactant and Yield Calculations Copyright 2012 John Wiley & Sons, Inc 9-2
3 Molar Mass Molar Mass sum of atomic masses of all atoms in 1 mole of an element or compound ; the units are g/mol. 1 mole = 6.022x10 23 molecules 6.022x10 23 formula units 6.022x10 23 atoms 6.022x10 23 ions Copyright 2012 John Wiley & Sons, Inc 9-3
4 Molar Mass What is the molar mass of Al(ClO 3 ) 3? Al 1(26.98 g) 3Cl 3(35.45 g) 9O 9(16.00 g) Al(ClO 3 ) g/mol atomic mass Al Cl O Copyright 2012 John Wiley & Sons, Inc 7-4
5 Molar Mass Calculate the mass of 2.5 moles of aluminum chlorate. Plan 2.5 mol Al(ClO 3 ) 3 g Al(ClO 3 ) 3 1 mol Al(ClO 3 ) 3 = g Al(ClO 3 ) 3 Calculate g Al(ClO ) mol Al(ClO 3) 3 = 690 g Al(ClO 3) 3 1 mol Al(ClO 3) 3 Copyright 2012 John Wiley & Sons, Inc 9-5
6 Molar Mass Calculate the moles of 3.52g of aluminum chlorate. Plan 3.52 g Al(ClO 3 ) 3 mol Al(ClO 3 ) 3 1 mol Al(ClO 3 ) 3 = g Al(ClO 3 ) 3 Calculate 3.52 g Al(ClO 3) 3 1 mol Al(ClO ) g Al(ClO ) = mol Al(ClO 3) 3 Copyright 2012 John Wiley & Sons, Inc 9-6
7 Molar Mass Calculate the number of formula units contained in 12.4 g aluminum chlorate. Plan 12.4 g Al(ClO 3 ) 3 formula units Al(ClO 3 ) 3 Calculate 1 mol Al(ClO 3 ) 3 = g = 6.022x10 23 formula units formula units 12.4 g Al(ClO 3) 22 3 = formula units g Al(ClO 3) 3 Copyright 2012 John Wiley & Sons, Inc 9-7
8 Your Turn! What is the mass of 3.61 moles of CaCl 2? a g b. 272 g c g d. 401 g atomic mass Ca Cl Copyright 2012 John Wiley & Sons, Inc 9-8
9 You Turn! How many moles of HCl are contained in 18.2 g HCl? a mol b mol c mol d mol atomic mass H 1.01 Cl Copyright 2012 John Wiley & Sons, Inc 9-9
10 Your Turn! What is the mass of molecules of HCl? a g b. 137 g c g d g atomic mass H 1.01 Cl Copyright 2012 John Wiley & Sons, Inc 9-10
11 Stoichiometry Stoichiometry deals with the quantitative relationships between the reactants and products in a balanced chemical equation. 1N 2(g) + 3I 2(s) 2NI 3(s) 1 mol N mol I 2 2 mol NI 3 Mole ratios come from the coefficients in the balanced equation: 3 mol I2 3 mol I2 1 mol N2 1 mol N 2 mol NI 2 mol NI 2 The 3 other possibilities are the inverse of these ratios. 3 3 Copyright 2012 John Wiley & Sons, Inc 9-11
12 Your Turn! Which of these statements is not true about the reaction? 1N 2(g) + 3I 2(s) 2NI 3(s) a. 1 mole of nitrogen is needed for every 3 moles of iodine b. 1 gram of nitrogen is needed for every 3 grams of iodine c. Both statements are true Copyright 2012 John Wiley & Sons, Inc 9-12
13 Using the mole ratio Calculate the number of moles of NI 3 that can be made from 5.50 mol N 2 in the reaction: 1N 2(g) + 3I 2(s) 2NI 3(s) Plan Set-Up 5.50 mol N 2 mol NI 3 moles of desired substance in equation mole ratio = moles of starting substance in equation 2 mol NI mol ratio = 1 mol N 3 2 Calculate 2 mol NI 5.50 mol N mol N2 = 11.0 mol NI 3 Copyright 2012 John Wiley & Sons, Inc 9-13
14 Using the mole ratio Calculate the number of moles of I 2 needed to react with 5.50 mol N 2 in the reaction: 1N 2(g) + 3I 2(s) 2NI 3(s) Plan Set-Up 5.50 mol N 2 mol I 2 3 mol I mole ratio = 1 mol N 2 2 Calculate 5.50 mol N 2 3 mol I2 1 mol N 2 = 16.5 mol I 2 Copyright 2012 John Wiley & Sons, Inc 9-14
15 Your Turn! How many moles of HF will be produced by the complete reaction of 1.42 moles of H 2 in the following equation? a b c d H 2 + F 2 2HF Copyright 2012 John Wiley & Sons, Inc 9-15
16 Stoichiometry Problem Solving Strategy for stoichiometry problems: 1. Convert starting substance to moles. 2. Convert the moles of starting substance to moles of desired substance. 3. Convert the moles of desired substance to the units specified in the problem. Copyright 2012 John Wiley & Sons, Inc 9-16
17 Stoichiometry Copyright 2012 John Wiley & Sons, Inc 9-17
18 Mole-Mole Calculations How many moles of Al are needed to make mol of H 2? Plan Set-Up Calculate 2Al (s) + 6HCl (aq) 2AlCl 3(aq) + 3H 2(g) mol H 2 mol Al mole ratio = 2 mol Al 3 mol H2 2 mol Al 2 3 mol H mol H =.0623 mol Al Copyright 2012 John Wiley & Sons, Inc 9-18
19 Mole-Mole Calculations How many moles of HCl are needed to make mol of H 2? 2Al (s) + 6HCl (aq) 2AlCl 3(aq) + 3H 2(g) Plan Set-Up Calculate mol H 2 mol HCl 6 mol HCl mole ratio = 3 mol H2 6 mol HCl 3 mol H mol H 2 = mol HCl Copyright 2012 John Wiley & Sons, Inc 9-19
20 Your Turn! How many moles of H 2 are made by the reaction of 1.5 mol HCl with excess aluminum? a mol b. 3.0 mol c. 6.0 mol d. 4.5 mol 2Al (s) + 6HCl (aq) 2AlCl 3(aq) + 3H 2(g) Copyright 2012 John Wiley & Sons, Inc 9-20
21 Your Turn! How many moles of carbon dioxide are produced when 3.00 moles of oxygen react completely in the following equation? C 3 H 8 + 5O 2 3CO 2 + 9H 2 O a mol b mol c mol d mol Copyright 2012 John Wiley & Sons, Inc 9-21
22 Your Turn! How many moles of C 3 H 8 are consumed when 1.81x10 23 molecules of CO 2 are produced in the following equation? a b c d C 3 H 8 + 5O 2 3CO 2 + 4H 2 O Copyright 2012 John Wiley & Sons, Inc 9-22
23 Mole-Mass Calculations What mass of H 2 (2.02 g/mol) is made by the reaction of 3.0 mol HCl with excess aluminum? 2Al (s) + 6HCl (aq) 2AlCl 3(aq) + 3H 2(g) Plan 3.0 mol HCl mol H 2 g H 2 Calculate 3.0 mol HCl 3 mol H2 =1.5 mol H 2 6 mol HCl 2.02 g H 1 mol H2 1.5 mol H = 3.0 g H Copyright 2012 John Wiley & Sons, Inc 9-23
24 Mole-Mass Calculations How many moles of HCl are needed to completely consume 2.00 g Al (26.98g/mol)? 2Al (s) + 6HCl (aq) 2AlCl 3(aq) + 3H 2(g) Plan 2.00 g Al mol Al mol HCl Calculate 2.00 g Al 1 mol Al = mol Al g Al 6 mol HCl 2 mol Al mol Al = mol HCl Copyright 2012 John Wiley & Sons, Inc 9-24
25 Mole-Mass Calculations What mass of Al(NO 3 ) 3 (213g/mol) is needed to react with.093 mol Na 2 CO 3? 3Na 2 CO 3(aq) + 2Al(NO 3 ) 3(aq) Al 2 (CO 3 ) 3(s) + 6NaNO 3(aq) Plan mol Na 2 CO 3 mol Al(NO 3 ) 3 g Al(NO 3 ) 3 Calculate.093 mol Na CO mol Al(NO ) 3 mol Na 2CO mol Al(NO 3) 3 1 mol Al(NO 3) g Al(NO ) =.062 mol Al(NO 3) 3 =13 g Al(NO ) Copyright 2012 John Wiley & Sons, Inc 9-25
26 Mole-Mass Calculations How many moles of Al 2 (CO 3 ) 3 are made by the reaction of 3.45g Na 2 CO 3 ( g/mol) with excess Al(NO 3 ) 3? 3Na 2 CO 3(aq) + 2Al(NO 3 ) 3(aq) Al 2 (CO 3 ) 3(s) + 6NaNO 3(aq) Plan 3.45g Na 2 CO 3 mol Na 2 CO 3 g Al 2 (CO 3 ) 3 Calculate 3.45g Na CO mol Na 2CO mol Na CO g Na CO mol Al (CO ) 3 mol Na 2CO = mol Na 2CO3 = mol Na 2CO3 Copyright 2012 John Wiley & Sons, Inc 9-26
27 Your Turn! How many moles of oxygen are consumed when 38.0g of aluminum oxide are produced in the following equation? atomic mass 4Al (s) + 3O 2(g) 2Al 2 O 3(s) Al a O b c d Copyright 2012 John Wiley & Sons, Inc 9-27
28 Your Turn! What mass of HCl is produced when 1.81x10 24 molecules of H 2 react completely in the following equation? a. 54.7g b. 72.9g c. 109g d. 219g H 2(g) + Cl 2(g) 2HCl (g) H 1.01 atomic mass Cl Copyright 2012 John Wiley & Sons, Inc 9-28
29 Mass-Mass Calculations Now we will put it all together. What mass of Br 2 ( g/mol) is needed to completely consume 7.00 g Al (26.98 g/mol)? 2Al (s) + 3Br 2(l) 2AlBr 3(s) 7.00 g Al mol Al mol Br 2 g Br 2 Copyright 2012 John Wiley & Sons, Inc 9-29
30 Mass-Mass Calculations What mass of Br 2 ( g/mol) is needed to completely consume 7.00 g Al (26.98 g/mol)? Plan Calculate 2Al (s) + 3Br 2(l) 2AlBr 3(s) 7.00 g Al mol Al mol Br 2 g Br g Al 1 mol Al 26.98g Al 3 mol Br mol Al = mol Br2 2 mol Al g Br 1 mol Br2 = mol Al = 62.2 g Br mol Br Copyright 2012 John Wiley & Sons, Inc 9-30
31 Mass-Mass Calculations What mass of Fe 2 S 3 (207.91g/mol) can be made from the reaction of 9.34 g FeCl 3 ( g/mol) with excess Na 2 S? Plan Calculate 2FeCl 3(aq) + 3Na 2 S (aq) Fe 2 S 3(s) + 6NaCl (aq) 9.34 g FeCl 3 mol FeCl 3 mol Fe 2 S 3 g Fe 2 S 3 1 mol FeCl g FeCl 9.34 g FeCl mol Fe S mol FeCl mol FeCl g Fe S = mol FeCl 3 = mol Fe S mol Fe 2 3 2S mol Fe S 2 3 = 5.99 g Fe S Copyright 2012 John Wiley & Sons, Inc 9-31
32 Your Turn! What mass of oxygen is consumed when 54.0g of water is produced in the following equation? a g b g c g d g 2H 2 + O 2 2H 2 O H 1.01 atomic mass O Copyright 2012 John Wiley & Sons, Inc 9-32
33 Your Turn! What mass of H 2 O is produced when 12.0g of HCl react completely in the following equation? a g b g c g d g 6HCl + Fe 2 O 3 2FeCl 3 + 3H 2 O H 1.01 atomic mass O Cl Copyright 2012 John Wiley & Sons, Inc 9-33
34 Limiting Reactant Determine the number of that can be made given these quantities of reactants and the reaction equation: + + Copyright 2012 John Wiley & Sons, Inc 9-34
35 Limiting Reactant The limiting reactant is the reactant that limits the amount of product that can be made. The reaction stops when the limiting reactant is used up. What was the limiting reactant in the reaction: + The small blue balls. Copyright 2012 John Wiley & Sons, Inc 9-35
36 Excess Reactant The excess reactant is the reactant that remains when the reaction stops. There is always left over excess reactant. What was the excess reactant in the reaction: + The excess reactant was the larger blue ball. Copyright 2012 John Wiley & Sons, Inc 9-36
37 Limiting reactant Figure 9.2 The number of bicycles that can be built from these parts is determined by the limiting reactant (the pedal assemblies). Copyright 2012 John Wiley & Sons, Inc 9-37
38 Limiting Reactant Calculations Technique for solving limiting reactant problems: 1. Convert reactant 1 to moles or mass of product 2. Convert reactant 2 to moles or mass of product 3. Compare answers. The smaller answer is the maximum theoretical yield. Copyright 2012 John Wiley & Sons, Inc 9-38
39 Limiting Reactant Calculation Calculate the number of moles of water that can be made by the reaction of 1.51 mol H 2 with mol O 2. 2H 2(g) + O 2(g) 2H 2 O (g) 1. Calculate the theoretical yield of H 2 O assuming H 2 is the limiting reactant and that O 2 is the excess reactant. 2. Calculate the theoretical yield of H 2 O assuming that O 2 is the limiting reactant and that H 2 is the excess reactant. Copyright 2012 John Wiley & Sons, Inc 9-39
40 Limiting Reactant Calculation continued Assuming that H 2 is limiting and O 2 is excess: 2 mol H2O 1.51 mol H 2 =1.51 mol H2O 2 mol H2 Assuming that O 2 is limiting and H 2 is excess: 2 mol H2O mol O 2 =1.86 mol H2O 1 mol 02 So what is the maximum yield of H 2 O? Copyright 2012 John Wiley & Sons, Inc 9-40
41 Limiting Reactant Calculation continued How much H 2 and O 2 remain when the reaction stops? H 2 : Limiting Reactant None remains. It was used up in the reaction. O 2 : Excess Reactant Calculate the amount of O 2 used in the reaction with H 2. Then subtract that from the original amount mol H 1 mol O x =0.755 mol O mol H mol O 2 to start mol O 2 = mol of excess O2 Copyright 2012 John Wiley & Sons, Inc 9-41
42 Limiting Reactant Calculation Calculate the mass of copper that can be made from the combination of 15.0 g aluminum with 25.0 g copper(ii) sulfate. 2Al (s) + 3CuSO 4(aq) Al 2 (SO 4 ) 3(aq) + 3Cu (s) Plan 15 g Al mol Al mol Cu g Cu 25 g CuSO 4 mol CuSO 4 mol Cu g Cu Compare answers. The smaller number is the right answer. Copyright 2012 John Wiley & Sons, Inc 9-42
43 Limiting Reactant Calculation continued 2Al (s) + 3CuSO 4(aq) Al 2 (SO 4 ) 3(aq) + 3Cu (s) 1. Assume Al is limiting and CuSO 4 is in excess g Al x 1 mol Al g Al 3 mol Cu 2 mol Al g Cu = 1 mol Cu 2. Assume CuSO 4 is limiting and Al is in excess. 1 mol CuSO 3 mol Cu 3 mol CuSO g CuSO g CuSO 4 3. Compare answers g Cu = 1 mol Cu 53.0 g Cu CuSO 4 is the limiting reagent. The theoretical yield of Cu is 9.96 g g Cu Copyright 2012 John Wiley & Sons, Inc 9-43
44 Your Turn! True/False: You can compare the quantities of reactant when you work a limiting reactant problem. The reactant you have the least of is the limiting reactant. a. True b. False Copyright 2012 John Wiley & Sons, Inc 9-44
45 Your Turn! Which is the limiting reactant when 3.00 moles of copper are reacted with 3.00 moles of silver nitrate in the following equation? Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag a. Cu b. AgNO 3 c. Cu(NO 3 ) 2 d. Ag Copyright 2012 John Wiley & Sons, Inc 9-45
46 Your Turn! What is the mass of silver ( g/mol) produced by the reaction of 3.00 moles of copper with 3.00 moles of silver nitrate? Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag a. 162g b. 216g c. 324g d. 647g Copyright 2012 John Wiley & Sons, Inc 9-46
47 Percent Yield To determine the efficiency of a process for making a compound, chemists compute the percent yield of the reaction. Actual Yield % Yield = 100 Theoretical Yield The theoretical yield is the result calculated using stoichiometry. The actual yield of a chemical reaction is the experimental result, which is often less than the theoretical yield due to experimental losses and errors along the way. Copyright 2012 John Wiley & Sons, Inc 9-47
48 Percent Yield Calculate the % yield of PCl 3 that results from reacting 5.00 g P with excess Cl 2 if only 17.2 g of PCl 3 were recovered. 2P + 3Cl 2 2PCl 3 Compute the expected yield of PCl 3 from 5.00 g P with excess Cl g P x 1 mol P g P Compute the % Yield. 2 mol PCl3 2 mol P g PCl 1 mol PCl3 3 = 22.2g PCl 3 Actual Yield 17.2 g % Yield = 100%= 100%=77.5% Theoretical Yield 22.2 g Copyright 2012 John Wiley & Sons, Inc 9-48
49 Your Turn! In a reaction to produce ammonia, the theoretical yield is 420. g. What is the percent yield if the actual yield is 350. g? A. 83.3% B. 20.0% C. 16.7% D. 120.% Copyright 2012 John Wiley & Sons, Inc 9-49
Unit 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 informationLimiting Reactants. In other words once the reactant that is present in the smallest amount is completely consumed the reaction will stop.
In any type of chemical reaction, the amount of product that can be produced is determined by the reactant which is in the smallest amount. In any type of chemical reaction, the amount of product that
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 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 informationChapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
More informationChemistry Stoichiometry and Heat Exam (ver.1) Mr. Thaler. Please do not write on this exam. Mark your answers on the scantron only.
1. Identify from the unbalanced equations below the one that does not represent a redox reaction. a. H 2O 2(aq) + MnO 4 - (aq) O 2(g) + Mn 2+ (aq) b. H 2(g) + N 2(g) NH 3(g) c. NaCl (aq) + AgNO 3(aq) NaNO
More informationMolar Mass. The total of the atomic masses of all the atoms in a molecule:
Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu
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 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 informationStudy Guide: Stoichiometry
Name: Study Guide: Stoichiometry Period: **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
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 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. 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 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 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 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 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 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 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 informationChapter 13. This ratio is the concentration of the solution.
Concentration Calculation Concentration In a solution, the solute is distributed evenly throughout the solvent. This means that any part of a solution has the same ratio of solute to solvent as any other
More informationReview Package #2 Measurement and Communication The Mole Chemical Reactions and Equations Stoichiometry
Chemistry 11 Review Package #2 Measurement and Communication The Mole Chemical Reactions and Equations Stoichiometry 1. Measurement and Communication: A. Scientific Notation: - Conversion of numbers from
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 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 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 informationAP Chemistry Multiple Choice Questions - Chapter 4
1 Which of the following contains 6.00 x 10 16 atoms? a 6.00 x 10 16 H 2 O molecules b 3.00 x 10 16 Cl 2 molecules c 2.00 x 10 16 P 4 molecules d 1.50 x 10 16 CaSO 4 empirical units 4.1 2 How many atoms
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. 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 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 informationChemistry B11 Chapter 5 Chemical reactions
Chapter 5 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl A + BC AC +
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 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 informationSCH4U Chemistry Review: Fundamentals
SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.
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 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 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 informationSTOICHIOMETRY HONORS CHEMISTRY
STOICHIOMETRY HONORS CHEMISTRY MOLE RATIO A mole ratio is the ratio of coefficients used to compare amounts of reactants and products. 1 ZnCl 2 (aq) + 2 NaOH (aq) 1 Zn(OH) 2 (aq) + 2 NaCl (aq) What is
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 informationSteward Fall 08. Moles of atoms/ions in a substance. Number of atoms/ions in a substance. MgCl 2(aq) + 2 AgNO 3(aq) 2 AgCl (s) + Mg(NO 3 ) 2(aq)
Dealing with chemical stoichiometry Steward Fall 08 of Not including volumetric stoichiometry of Chapter 6.0x10 A 6.0x10 Mol/mol ratio from balanced equation B 6.0x10 6.0x10 s, Equations, and Moles: II
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 informationAP Chemistry. Mole, Molecular Formula Review One Mole = o This is Avogadro s number. Molar Mass: The mass of one mole of a substance in grams.
AP Chemistry Ms Ye Name Date Block Mole, Review One Mole = o This is Avogadro s number Molar Mass: The mass of one mole of a substance in grams Percent Composition: Identifies the elements present in a
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 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 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 information15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g
CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO
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 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 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 informationNotes: Stoichiometry (text Ch. 9)
Name Per. Notes: Stoichiometry (text Ch. 9) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to get missing information
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 informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 10 Chemical Equation Calculations by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 10 1 What
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 informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More informationTest bank chapter (3)
Test bank chapter (3) Choose the correct answer 1. What is the mass, in grams, of one copper atom? a) 1.055 10 - g b) 63.55 g c) 1 amu d) 1.66 10-4 g. Determine the number of moles of aluminum in 96.7
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:
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 information9.2 Chemical Calcualtions. Chapter 9 Stoichiometry. 9.1 The Arithmetic of Equations. 9.2 Chemical Calculations. 9.3 Limiting Reagent and Percent Yield
9.2 Chemical Calcualtions Chapter 9 Stoichiometry 9.1 The Arithmetic of Equations 9.2 Chemical Calculations 9.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates.
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 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 informationReaction Stoichiometry and Solution Concentration Q1. FeS(S) + 2HCl(aq) FeCl2(S) + H2S(g) Q2. C6H10(g) + O2(g) CO2(g) + H2O(g) Q3.
Reaction Stoichiometry and Solution Concentration Q1. The reaction between Iron(II) sulfide and HCl is as follows; FeS (S) + 2HCl (aq) FeCl 2(S) + H 2 S (g) What will be the number of moles of each reactant
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 informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Semester 1/2012 3.1 Atomic Mass 3.2 Avogadro s Number and the Molar Mass of an element 3.3 Molecular Mass 3.5 Percent Composition of Compounds 3.6 Experimental
More informationUnit 5. Chemical Composition
Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles
More informationSample Problem Set. Limiting Reactants
Skills Worksheet Sample Problem Set Limiting Reactants At the beginning of Chapter 8, a comparison was made between solving stoichiometry problems and making turkey sandwiches. Look at the sandwich recipe
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 informationUnit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
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: Calculations with Chemical Formulas and Equations (Chapter 3) Past Quiz and Test Questions
Stoichiometry: Calculations with Chemical Formulas and Equations (Chapter 3) Past Quiz and Test Questions 1. Balance the following equations Al 2 (SO 4 ) 3 (aq) + Ba(NO 3 ) 2 (aq) ----> Al(NO 3 ) 3 (aq)
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 17. Oxidation-Reduction. Cu (s) + 2AgNO 3(aq) 2Ag (s) + Cu(NO 3 ) 2(aq) pale blue solution. colorless solution. silver crystals.
Chapter 17 Oxidation-Reduction Cu (s) + 2AgNO 3(aq) 2Ag (s) + Cu(NO 3 ) 2(aq) copper wire colorless solution silver crystals pale blue solution Introduction to General, Organic, and Biochemistry 10e John
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationProblem Solving. Limiting Reactants
Skills Worksheet Problem Solving Limiting Reactants At the beginning of Chapter 8, a comparison was made between solving stoichiometry problems and making turkey sandwiches. Look at the sandwich recipe
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 informationCartoon courtesy of NearingZero.net. Stoichiometry
Cartoon courtesy of NearingZero.net Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Reactants appear on the left side of the equation. Anatomy of a Chemical Equation CH 4 (g)
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 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 informationChapter 9. Slide 1. Chemical Quantities. Slide 2. Table of Contents
1 Chapter 9 Chemical Quantities 2 Chapter 9 Table of Contents 9.1 Information Given by Chemical Equations 9.2 9.3 3 Copyright Cengage Learning. All rights reserved 2 Section 9.1 Information Given by Chemical
More informationTopic: Balancing Equations. 1. Balance the following equation. What is the sum of the coefficients of the reactants and products?
PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTRIALS; pp. Khuda Baksh Library, Ashok Rajpath, Patna PIN PINT STUDY CIRCLE; House No. 5A/65, pp. Mahual Kothi, Alpana Market,
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 informationReview Exam 2. 2.What is the mass of 4 atom(s) of copper in grams? A) g B) g C) g D) g E) 4.
Review Exam 2 1.Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate
More informationPractice questions for Chapter 4
Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar
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 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 Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More information14 Stoichiometry CHAPTER CHAPTER OUTLINE. 293
www.ck12.org 293 CHAPTER 14 Stoichiometry CHAPTER OUTLINE 14.1 INTRODUCTION TO 14.2 STOICHIOMETRIC CALCULATIONS 14.3 LIMITING REACTANT 14.4 PERCENT YIELD 294 www.ck12.org 14.1 Introduction to Stoichiometry
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 informationChapter. Measuring Concentration. Table of Contents
Measuring Concentration Table of Contents Introduction 1. Percent Concentration 2. Molarity 3. Preparation of a with a Desired Concentration Measuring Concentration Warm Up How do you classify solutions
More informationChapter 3 Chemical Reactions and Equations
Chapter 3 Chemical Reactions and Equations Chemical Reactions Reactions involve rearrangement and exchange of atoms to produce new pure substances. Reactants Products Chemical Equations Shorthand way
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 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 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 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 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 informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationMole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units )
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units ) N A 6.0 10 mol -1 1 mol substance contains N A Molar mass (g/mol)
More informationactual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information
12 Study Guide 12 Study Guide Study Tip Prioritize Schedule your time realistically. Stick to your deadlines. If your class subscribes to the Interactive Textbook with ChemASAP, your students can go online
More information