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Chapter 8

Chapter 8. Chemical Quantities In Reactions. Homework. Assigned Problems (odd numbers only) “Questions and Problems” 8.1 to 8.31 (begins on page 230) “Additional Questions and Problems” 8.39 to 8.51 (begins on page 247) “Challenge Questions” 8.53 and 8.55, page 248

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Chapter 8

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  1. Chapter 8 Chemical Quantities In Reactions

  2. Homework • Assigned Problems (odd numbers only) • “Questions and Problems” 8.1 to 8.31 (begins on page 230) • “Additional Questions and Problems” 8.39 to 8.51 (begins on page 247) • “Challenge Questions” 8.53 and 8.55, page 248 • “Combining Ideas” CI 11 and CI 13, page 250

  3. Mole Relationships in Chemical Equations:Conservation of Mass • As a chemical reaction proceeds: • Reactants are consumed and new materials with new chemical properties are produced • Bonds are broken, formed, or atoms are rearranged which produces new substances • No material is lost or gained as original substances change to new substances

  4. Mole Relationships in Chemical Equations:Conservation of Mass • Law of Conservation of Mass • Quantity of matter does not change during a chemical reaction • The sum of the masses of products is equal to the sum of masses of reactants • Atoms are neither created nor destroyed in chemical reactions

  5. Mole Relationships in Chemical Equations:Conservation of Mass • A balanced equation has the same number of atoms on each side of the arrow 2 2

  6. Information Available from a Balanced Chemical Equation • “1 mole of methane gas reacts with 2 moles of oxygen gas to produce 1 mole of carbon dioxide and 2 moles of water vapor.” • Multiplying each of the molar masses by the coefficient will give the total mass of reactants and products

  7. Information Available from a Balanced Chemical Equation • Balanced chemical equations tell us: • Relative number of atoms reacting and produced • Number can be in terms of single atoms, or moles of atoms 2

  8. Mole-Mole Factors • In a balanced equation, conversion from moles of one substance to another will be determined by the values of the coefficients • To determine how many moles of methanol would be produced if 0.295 moles of hydrogen gas is consumed • Will require a mole to mole conversion • Converting the given mole amount of hydrogen gas to the needed mole amount of methanol 2

  9. Mole-Mole Factors 2 • Coefficients of the balanced equation can be used to make ratios (conversion factors) between the different reactants and products

  10. Mole-Mole Factors • Write all of the possible mole ratios for the following chemical equation 2 2

  11. Using Mole-Mole Factors in Calculations • Calculations based on balanced equations require the use of mole to mole conversions • Equation must be balanced • Identify the known and needed substances • Make the conversion factor based on

  12. Stoichiometry grams B grams A MM of A MM of B Stoichiometry moles B moles A moles A moles B • Using mole ratios from a BALANCED chemical equation • Can convert moles of one compound to moles of another compound using the correct mole ratio Mol-mol factor

  13. Using Mole-Mole Factors in Calculations:Calculating Moles of a Product • Calculate the moles of CO2 formed when 4.30 moles of C3H8 reacts with (the required) 21.5 moles of O2 • Balance the equation • Plan to convert the given amount of moles to the needed amount of moles • Use coefficients to state the relationships and mole-mole factors • Set up the problem using the mole-mole factor and canceling units 4 5 3

  14. Using Mole-Mole Factors in Calculations:Calculating Moles of a Product 5 4 3 Mol-mol factor Given: Needed: Mole-mole factor Mole-mole relation 1 mol C3H8 = 3 mol CO2

  15. Using Mole-Mole Factors in Calculations:Calculating Moles of a Product • Set up the problem using the mole-mole factor that cancels given moles and provides needed moles 5 4 3 Mole-mole factor

  16. Mass Calculations for Reactions • From the balanced equation • It is also possible to start with a known mass of one substance • Then convert to moles of another substance • Start with a known amount of moles of a substance • Then convert to the sought mass of another substance

  17. Mass Calculations • Convert the moles of one substance to moles of another substance • Find the mole-mole factor using the coefficients in the balanced equation • Ratios ONLY apply to moles, NOT grams • Convert grams to moles, then use mole ratio Mol-mol factor

  18. Mass Calculations • You can only relate moles of two compounds • Ratios ONLY apply to moles, NOT grams • Convert grams to moles, then use mole ratio

  19. Mass Calculations For Reactions: Mass of Product from Mass of Reactant grams CO2 grams C3H8 MM of A MM of B Stoichiometry moles CO2 moles C3H8 moles CO2 moles C3H8 • What mass of carbon dioxide is produced when 96.1 g of propane react with sufficient oxygen? • Balance the equation • Plan to convert the given mass to given moles • Convert the given moles to needed moles by the use of mole-mole factor • Convert the needed moles to needed mass 3 4 5

  20. Mass Calculations Example 1 grams CO2 grams C3H8 MM of A MM of B Stoichiometry moles CO2 moles C3H8 moles A moles B • Write the equalities • 1 mol C3H8 = 44.09 g C3H8 • 1 mol CO2 = 44.01 g CO2 • 1 mol C3H8 = 3 mol CO2 to create mole-mole factor 5 4 3 Mass needed: g of CO2 Given: 96.1 g C3H8

  21. Mass Calculations Example 1 5 4 3 Xg CO2

  22. Mass Calculations Example 2 • What mass of carbon monoxide and what mass of hydrogen are required to form 6.0 kg of methanol by the following reaction: 2

  23. Mass Calculations Example 2 2

  24. Mass Calculations Example 2

  25. Limiting Reactants • Chemical reactions with two or more reactants will continue until one of the reactants is used up • The reactant used up is called the limiting reactant (reagent) • This limits the amount of product that can be made

  26. Reactions • In the lab, reactants do not always combine in exact mole ratios • Often reactions are run with more of one reactant than is needed (excess) • A reaction will continue until one of the reactants runs out • Reactant that runs out first is the Limiting Reactant

  27. Calculating Moles of Product from a Limiting Reactant • To determine the limiting reactant between two reactants • Balance the equation • Determine the number of moles of each reactant • Calculate the number of moles of product that each of the reactants (moles) would produce • The reactant producing the least amount of product (moles) is the limiting reactant

  28. Calculating Moles of Product from a Limiting Reactant • Determine the number of moles of product that each reactant can make • The smallest number is the MAXIMUM product you can make • The reactant that gives the smallest amount of product is the limiting reactant

  29. Calculating Mass of Product from a Limiting Reactant • Balance the equation • Determine the amount of product that can be made by each reactant • Compare numbers • Reagent that gives the smaller number is limiting and that is the maximum amount of product that can be made

  30. Limiting Reactant Problem • Lithium nitride, an ionic compound containing Li+ and N3- ions, is prepared by the reaction of lithium metal and nitrogen gas. Calculate the mass of lithium nitride formed from 56.0 g of nitrogen gas and 56.0 g of lithium metal. 2 6

  31. Limiting Reactant Problem Grams Li3N grams Li MM of Li MM of Li3N Stoichiometry moles Li3N moles Li moles Li3N moles Li 3 6 Needed: g of Li3N Given: 56.0 g N2 Given: 56.0 g Li Equalities and Conversion Factors 1 mol Li3N= 34.83 g Li3N 1 mol Li = 6.941g Li 1 mol N2 = 28.00 g N2

  32. Calculate the Limiting Reactant Limiting reactant 8.07 mol Li 2.69 mol Li3N 2.00 mol N2 3.997 mol Li3N

  33. Limiting Reactant Problem Lithium is the limiting reagent. Calculate the number of grams of lithium nitride formed in the reaction based on the limiting reactant: 2.69 mol of lithium 93.7 g Li3N

  34. Product Yield • The calculated amount of product that should be obtained is called the theoretical yield • Assumes all reactants are converted to product based on the mole-mole ratios of reactant to product • Rarely do you get the maximum amount of product • Side reactions • Loss during transfer • Accidental spills

  35. Percent Yield • Theoretical Yield • The calculated amount of product • Actual Yield • The actual amount of product • Something less than the theoretical • Percent Yield • The fraction of the theoretical yield actually obtained is expressed as a percent

  36. Percent Yield Example • In the previous limiting reactant problem, you actually produced 90.8 g of Li3N. What is the percent yield of this reaction? 96.9 % yield

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