Reinforced S.15.C.6 Identify the physical state for each substance in a reaction equation Reinforced Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Main Standards Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Stoichiometry Table of Contents Section 2 Ideal Stoichiometric Calculations Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Objective • Calculate the amount in moles of a reactant or a product from the amount in moles of a different reactant or product. • Calculate the mass of a reactant or a product from the amount in moles of a different reactant or product. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Objectives, continued • Calculate the amount in moles of a reactant or a product from the mass of a different reactant or product. • Calculate the mass of a reactant or a product from the mass of a different reactant or product. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Quantities in Moles Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Visual Concepts Conversion of Quantities in Moles Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/ Visual Concept student/ch09/sec02/vc00/hc609_02_v00 fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Mass-Mass Stoichiometry Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Quantities in Moles, continued Sample Problem A In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following balanced chemical equation. CO2(g) + 2LiOH(s) Li2CO3(s) + H2O(l) How many moles of lithium hydroxide are required to react with 20 mol CO2, the average amount exhaled by a person each day? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Quantities in Moles, continued Sample Problem A Solution CO2(g) + 2LiOH(s) Li2CO3(s) + H2O(l) Given: amount of CO2 = 20 mol Unknown: amount of LiOH (mol) Solution: mol ratio mol LiOH mol CO2 mol LiOH mol CO2 2 mol LiOH 20 mol CO2 40 mol LiOH 1 mol CO2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Practice problems pg. 306 • Write the balanced equation for practice problems pg. 306 and answer the question in your notes. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 ANSWERS Practice problems pg. 306 • Write the balanced equation for practice problems pg. 306 and answer the question in your notes. Make sure you understand why. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Amounts in Moles to Mass Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Stoichiometry Problems with Moles or Grams Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Amounts in Moles to Mass, continued Sample Problem B In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6, and oxygen from the reaction of carbon dioxide and water. What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Amounts in Moles to Mass, continued Sample Problem B Solution Given: amount of H2O = 3.00 mol Unknown: mass of C6H12O6 produced (g) Solution: Balanced Equation: 6CO2(g) + 6H2O(l) C6H12O6(s) + 6O2(g) mol ratio mol H2O 3.00 mol H2O mol C6H12O6 mol H2O 1 mol C6H12O6 6 mol H2O molar mass factor g C6H12O6 mol C6H12O6 g C6H12O6 180.18 g C6H12O6 1 mol C6H12O6 = 90.1 g C6H12O6 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Practice problems pg. 308 • Write the balanced equation for practice problems pg. 308 #1-2 and answer the question in your notes. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 ANSWERS Practice problems pg. 308 • Write the balanced equation for practice problems pg. 308 #1-2 and answer the question in your notes. Make sure you understand why. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Mass to Amounts in Moles Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Visual Concepts Mass and Number of Moles of an Unknown Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_00303680 Visual Concept 9x/student/ch09/sec02/vc01/hc609_0 2_v01fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Mass to Amounts in Moles, continued Sample Problem D The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia. NH3(g) + O2(g) NO(g) + H2O(g) (unbalanced) The reaction is run using 824 g NH3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H2O are formed? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Conversions of Mass to Amounts in Moles, continued Sample Problem D Solution Given: mass of NH3 = 824 g Unknown: a. amount of NO produced (mol) b. amount of H2O produced (mol) Solution: Balanced Equation: 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) molar mass factor a. b. g NH3 mol NH3 g NH3 mol NH3 g NH3 g NH3 mol ratio mol NO mol NH3 mol NO mol H2O mol H2O mol NH3 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Section 2 Ideal Stoichiometric Calculations Chapter 9 Conversions of Mass to Amounts in Moles, continued Sample Problem D Solution, continued molar mass factor a. 824 g NH3 b. 824 g NH3 1 mol NH3 17.04 g NH3 1 mol NH3 17.04 g NH3 mol ratio 4 mol NO 48.4 mol NO 4 mol NH3 6 mol H2O 4 mol NH3 Chapter menu 72.5 mol H2O Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Practice problems pg. 309 • Write the balanced equation for practice problems pg. 309 #1-2 and answer the question in your notes. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 ANSWERS Practice problems pg. 309 • Write the balanced equation for practice problems pg. 309 #1-2 and answer the question in your notes. Make sure you understand why. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Mass-Mass to Calculations Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Visual Concepts Mass-Mass Calculations Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/stu Visual Concept dent/ch09/sec02/vc02/hc609_02_v02fs.htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Mass-Mass Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Mass-Mass to Calculations, continued Sample Problem E Tin(II) fluoride, SnF2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation. Sn(s) + 2HF(g) SnF2(s) + H2(g) How many grams of SnF2 are produced from the reaction of 30.00 g HF with Sn? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Mass-Mass to Calculations, continued Sample Problem E Solution Given: amount of HF = 30.00 g Unknown: mass of SnF2 produced (g) Solution: molar mass factor mol ratio molar mass factor mol SnF2 g SnF2 mol HF g HF g SnF2 g HF mol HF mol SnF2 1 mol SnF2 156.71 g SnF2 1 mol HF g HF 20.01 g HF 2 mol HF 1 mol SnF2 = 117.5 g SnF2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Practice Problems p.311 #1-3 Chapter 9 • Write a balanced equation before answering questions. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Practice Problems p.311 #1-3 ANSWERS Chapter 9 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Various Types of Stoichiometry Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Various Types of Stoichiometry Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Volume-Volume Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Particle Problems Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 9 Visual Concepts Ideal Stoichiometric Calculations Click below to watch the PROBLEM ACTIVITIES CALCULATING MOLES REACTED MASS TO MOLES PROBLEM MOLES TO MASS PROBLEM MOLES TO MASS #2 MASS TO MASS PROBLEM Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Online Self-Check Quiz Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 9.2 (7 questions) You must be in the “Play mode” for the slideshow for hyperlink to work. Slide of 25 © Copyright Pearson Prentice Hall End Show VIDEOS FOR ADDITIONAL INSTRUCTION Additional Videos for Section 9.2: Ideal Stoichiometric Calculations None at this time Slide of 28 © Copyright Pearson Prentice Hall End Show End of Chapter 9.2 Show Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.