Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.

Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois

Chapter 9 Chemical Quantities

Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers of reacting molecules and product molecules. 2 CO + O 2 2 CO 2 2 CO molecules react with 1 O 2 molecules to produce 2 CO 2 molecules Copyright Houghton Mifflin Company. All rights reserved. 9 3

Information Given by the Chemical Equation Since the information given is relative: 2 CO + O 2 2 CO 2 1. 200 CO molecules react with 100 O 2 molecules to produce 200 CO 2 molecules 2. 2 billion CO molecules react with 1 billion O 2 molecules to produce 20 billion CO 2 molecules 3. 2 moles CO molecules react with 1 mole O 2 molecules to produce 2 moles CO 2 molecules 4. 12 moles CO molecules react with 6 moles O 2 molecules to produce 12 moles CO 2 molecules Copyright Houghton Mifflin Company. All rights reserved. 9 4

Information Given by the Chemical Equation The coefficients in the balanced chemical equation show the molecules and the mole ratio of the reactants and products. Since moles can be converted to masses, we can determine the mass ratio of the reactants and products as well. Copyright Houghton Mifflin Company. All rights reserved. 9 5

Information Given by the Chemical Equation 2 CO + O 2 2 CO 2 2 moles CO = 1 mole O 2 = 2 moles CO 2 Since 1 mole of CO = 28.01 g, 1 mole O 2 = 32.00 g, and 1 mole CO 2 = 44.01 g 2(28.01) g CO = 1(32.00) g O 2 = 2(44.01) g CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 6

Example #1 Determine the number of moles of carbon monoxide required to react with 3.2 moles oxygen, and determine the moles of carbon dioxide produced. Copyright Houghton Mifflin Company. All rights reserved. 9 7

Example #1 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 8

Example #1 (cont.) Use dimensional analysis: Copyright Houghton Mifflin Company. All rights reserved. 9 9

Example #2 Determine the number of moles of carbon monoxide required to react with 3.2 moles oxygen, and determine the moles of carbon dioxide produced. Copyright Houghton Mifflin Company. All rights reserved. 9 10

Example #2 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Determine the molar mass of each: 1 mol CO = 28.01 g 1 mol O 2 = 32.00 g 1 mol CO 2 = 44.01 g Copyright Houghton Mifflin Company. All rights reserved. 9 11

Example #2 (cont.) Use the molar mass of the given quantity to convert it to moles. Use the mole relationship to convert the moles of the given quantity to the moles of the desired quantity: Copyright Houghton Mifflin Company. All rights reserved. 9 12

Example #2 (cont.) Use the molar mass of the desired quantity to convert the moles to mass: Copyright Houghton Mifflin Company. All rights reserved. 9 13

Limiting and Excess Reactants Limiting reactant: a reactant that is completely consumed when a reaction is run to completion Excess reactant: a reactant that is not completely consumed in a reaction Theoretical yield: the maximum amount of a product that can be made by the time the limiting reactant is completely consumed Copyright Houghton Mifflin Company. All rights reserved. 9 14

Example #3 Determine the number of moles of carbon dioxide produced when 3.2 moles oxygen reacts with 4.0 moles of carbon monoxide. Copyright Houghton Mifflin Company. All rights reserved. 9 15

Example #3 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Copyright Houghton Mifflin Company. All rights reserved. 9 16

Example #3 (cont.) Use dimensional analysis to determine the number of moles of reactant A needed to react with reactant B: Copyright Houghton Mifflin Company. All rights reserved. 9 17

Example #3 (cont.) Compare the calculated number of moles of reactant A to the number of moles given of reactant A. If the calculated moles is greater, then A is the limiting reactant; if the calculated moles is less, then A is the excess reactant. The calculated moles of CO (6.4 moles) is greater than the given 4.0 moles; therefore CO is the limiting reactant. Copyright Houghton Mifflin Company. All rights reserved. 9 18

Example #3 (cont.) Use the limiting reactant to determine the moles of product: Copyright Houghton Mifflin Company. All rights reserved. 9 19

Example #4 Determine the mass of carbon dioxide produced when 48.0 g of oxygen reacts with 56.0 g of carbon monoxide. Copyright Houghton Mifflin Company. All rights reserved. 9 20

Example #4 (cont.) Write the balanced equation: 2 CO + O 2 2 CO 2 Use the coefficients to find the mole relationship: 2 moles CO = 1 mol O 2 = 2 moles CO 2 Determine the molar mass of each: 1 mol CO = 28.01 g 1 mol O 2 = 32.00 g 1 mol CO 2 = 44.01 g Copyright Houghton Mifflin Company. All rights reserved. 9 21

Example #4 (cont.) Determine the moles of each reactant: Copyright Houghton Mifflin Company. All rights reserved. 9 22

Example #4 (cont.) Determine the number of moles of reactant A needed to react with reactant B: Copyright Houghton Mifflin Company. All rights reserved. 9 23

Example #4 (cont.) Compare the calculated number of moles of reactant A to the number of moles given of reactant A. If the calculated moles is greater, then A is the limiting reactant; if the calculated moles is less, then A is the excess reactant. The calculated moles of O 2 (1.00 moles) is less than the given 1.50 moles; therefore O 2 is the excess reactant. Copyright Houghton Mifflin Company. All rights reserved. 9 24

Example #4 (cont.) Use the limiting reactant to determine the moles of product, then the mass of product: Copyright Houghton Mifflin Company. All rights reserved. 9 25

Percent Yield Most reactions do not go to completion. Actual yield: the amount of product made in an experiment Percent yield: the percentage of the theoretical yield that is actually made Percent Yield = Actual Yield Theoretical Yield x 100% Copyright Houghton Mifflin Company. All rights reserved. 9 26

Example #4a If in the last problem 72.0 g of carbon dioxide is actually made, what is the percentage yield? Copyright Houghton Mifflin Company. All rights reserved. 9 27

Example #4a (cont.) Divide the actual yield by the theoretical yield, then multiply by 100% The actual yield of CO 2 is 72.0 g The theoretical yield of CO 2 is 88.0g Copyright Houghton Mifflin Company. All rights reserved. 9 28