STOICHIOMETRY. - the study of the quantitative aspects of chemical
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1 STOICHIOMETRY - the study of the quantitative aspects of chemical
2 GENERAL PLAN FOR STOICHIOMETRY Mass reactant Mass product Moles reactant Stoichiometric factor Moles product
3 STOICHIOMETRY It rests on the principle of the conservation 2 Al(s) + 3 Br 2 (liq) f Al 2 Br 6 (s)
4 Conversion Factors from Eqns The mole ratio between two species, as given in the balanced chemical equation, is the PER expression that links moles of one species to moles of another:
5 Conversion Factors from Eqns Example: How many moles of oxygen are needed to completely react with 2.34 moles of ammonia in a reaction that yields nitrogen monoxide and water? Solution: First, write and balance the chemical
6 Conversion Factors from Eqns How many moles of oxygen are needed to completely react with 2.34 moles of ammonia in a reaction that yields nitrogen monoxide and water? 4 NH O 2 4 NO + 6 H 2 O The PER relationship comes from the balanced equation:
7 Conversion Factors from Eqns GIVEN: 2.34 mol NH 3, 4 NH O 2 4 NO + 6 H 2 O WANTED: mol O 2 PER:
8 Mass-Mass Stoichiometry Goal 2 Given a chemical equation, or a reaction for which the equation can be written, and the number of grams or moles of one species in the reaction, find the number of grams or moles of any other species.
9 Mass-Mass Stoichiometry Stoichiometry The quantitative relationships among substances involved in a chemical reaction. Established by the balanced equation for the reaction. A stoichiometry problem asks, How much or how many?
10 Mass Mass Stoichiometry Prerequisite Skills for Stoichiometry Write chemical formulas. Ch. 6 Calculate molar masses from chemical formulas. Sect. 7.4 Use molar masses to convert between moles and mass. Sect. 7.5 Write and balance chemical equations. Ch. 8 Use an equation to convert from moles
11 Mass Mass Stoichiometry Mass-to-Mass Stoichiometry Path Mass of Moles of Moles of Mass of Given Given Wanted Wanted Molar Mass Equation Molar Mass g PER mol mol PER mol g PER mol Mass Given
12 Mass Mass Stoichiometry How to Solve a Stoichiometry Problem: The Stoichiometry Path Step 1: Change the mass of the given species to moles. Step 2: Change the moles of the given species to the moles of the wanted species. Step 3: Change the moles of the wanted species
13 Mass Mass Stoichiometry Example: How many grams of carbon dioxide are produced when 10.0 g of methane, CH 4, is burned? Solution: GIVEN: 10.0 g CH 4 WANTED: g CO 2 CH O 2 CO H 2 O PER: g CH 4 /mol CH 4 PATH: g CH 4 mol CH 4 1 mol CO 2 /1 mol CH g CO 2 /mol CO 2
14 Mass Mass Stoichiometry 10.0 g CH 4 = 27.4 g CO 2
15 Percent Yield Goal 3 Given two of the following, or information from which two of the following may be determined, calculate the third: theoretical yield, actual yield, percent yield. Theoretical Yield = Maximum amount of product possible based on amount of reactant(s). Actual Yield = How much product was actually obtained.
16 Percent Yield The actual yield of a chemical reaction is usually less than the theoretical yield predicted by a stoichiometry calculation because: reactants may be impure the reaction may not go to completion other reactions may occur Actual yield is experimentally determined.
17 Percent Yield Percent yield expresses the ratio of actual yield to theoretical yield: % yield = 100
18 Percent Yield Example: Determine the percent yield if 6.97 grams of ammonia is produced from the reaction of 6.22 grams of nitrogen with excess hydrogen. Solution: Notice that two quantities are given in the problem statement g NH 3 is the actual yield 6.22 g N 2 is the amount of reactant. This can be used to
19 Percent Yield GIVEN: 6.22 g N 2 WANTED: g NH 3 (theo) N H 2 2 NH 3 PER: g N 2 /mol N 2 2 mol NH 3 /1 mol N 2 PATH: g N 2 mol N 2
20 Percent Yield 6.22 g N 2 = 7.56 g NH 3 (theo) % yield = 100 = 100 =
21 Percent Yield Once a percent yield has been determined for a reaction, it can be used in stoichiometry calculations. For example, the 92.2% yield from the prior example means: and
22 PROBLEM: If 454 g of NH 4 NO 3 decomposes, how much N 2 O and H 2 O are formed? What is the theoretical yield of products? STEP 1 Write the balanced chemical equation NH 4 NO 3 (s) f N 2 O(g) + 2 H 2 O(g)
23 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 2 Convert mass of reactant (454 g) to amount (mol) STEP 3 Convert amount of reactant (5.67 mol) to amount (mol) of product.
24 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 3 Convert moles reactant f moles product Relate moles NH 4 NO 3 to moles product expected. 1 mol NH 4 NO 3 f 2 mol H 2 O Express this relation as the STOICHIOMETRIC FACTOR
25 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 3 Convert moles reactant (5.67 mol) to amount (mol) of product = 11.3 mol H 2 O produced
26 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 4 Convert amount of product (11.3 mol) to mass of product Called the THEORETICAL YIELD ALWAYS FOLLOW THESE STEPS IN SOLVING STOICHIOMETRY PROBLEMS!
27 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 5 What mass of N 2 O is formed? Total mass of reactants = total mass of products 454 g NH 4 NO 3 = g N 2 O g H 2 O
28 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O Amounts Table (from page 159) 1.Compound NH 4 NO 3 N 2 O H 2 O 2. Initial (g) 3. Initial (mol) 4. Change (mol) 5. Final (mol) 6. Final (g)
29 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O Amounts Table 1.Compound NH 4 NO 3 N 2 O H 2 O 2.Initial (g) 454 g Initial (mol)5.67 mol Change (mol) (5.67) 5.Final (mol) Final (g) Note that matter is conserved!
30 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 6 Calculate the percent yield If you isolated only 131 g of N 2 O, what is the percent yield? This compares the theoretical (250.
31 454 g of NH 4 NO 3 f N 2 O + 2 H 2 O STEP 6 Calculate the percent yield
32 PROBLEM: Using 5.00 g of H 2 O 2, what mass of O 2 and of H 2 O can be obtained? 2 H 2 O 2 (liq) f 2 H 2 O(g) + O 2 (g) Reaction is catalyzed by MnO 2 Step 1: amount (mol) of H 2 O 2 Step 2: use STOICHIOMETRIC FACTOR to calculate amount (mol) of O 2
33 Reactions Involving a LIMITING REACTANT 1.In a given reaction, there is not enough of one reagent to use up the other reagent completely. 2.The reagent in short supply LIMITS the quantity of product that can be formed.
34 LIMITING REACTANTS Reactants Products 2 NO(g) + O 2 (g) f 2 NO 2 (g) Limiting reactant = Excess reactant =
35 LIMITING REACTANTS React solid Zn with mol HCl (aq) Zn + 2 HCl f ZnCl 2 + H 2 PLAY MOVIE Rxn 1: Balloon inflates fully, some Zn left * More than enough Zn to use up the mol HCl Rxn 2: Balloon inflates fully, no Zn left * Right amount of each (HCl and Zn) Rxn 3: Balloon does not inflate fully, no Zn left.
36 LIMITING REACTANTS React solid Zn with mol HCl (aq) Zn + 2 HCl f ZnCl 2 + H mol HCl [1 mol Zn/2 mol HCl] = mol Zn Rxn 1 Rxn 2 Rxn 3 mass Zn (g) mol Zn
37 Limiting Reactants Goal 4 Identify and describe or explain limiting reactants and excess reactants.
38 Limiting Reactants Three atoms of carbon react with two molecules of oxygen:
39 Limiting Reactants The reaction will stop when two molecules of oxygen are used up. Two carbon dioxide molecules will form; One carbon atom will remain unreacted: C + O 2 CO 2 Start Used (+) or Produced ( )
40 Limiting Reactants Limiting Reactant The reactant that is completely used up. (Oxygen) Excess Reactant The reactant initially present in excess. (some will remain unreacted) (Carbon)
41 Limiting Reactants Goal 5 Given a chemical equation, or information from which it may be determined, and initial quantities of two or more reactants, (a) identify the limiting reactant, (b) calculate the theoretical yield of a specified product, assuming complete use of the limiting reactant, and (c) calculate the quantity of reactant initially in excess that remains unreacted.
42 Limiting Reactants Comparison-of-Moles Method How to Solve a Limiting Reactant Problem: 1. Convert the number of grams of each reactant to moles. 2. Identify the limiting reactant. 3. Calculate the number of moles of each species that reacts or is produced. 4. Calculate the number of moles of each species that remains after the reaction. 5. Change the number of moles of each species to grams.
43 Limiting Reactants Example: A 24.0-g piece of solid sodium is added to 24.0 g of liquid water. How many grams of hydrogen will be produced? How many grams of which reactant will be left over? Solution: Step 1 is to convert the number of grams of each reactant to moles g Na = 1.04 mol Na
44 Limiting Reactants Step 2 is to identify the limiting reactant. This requires a balanced chemical equation so that the mole ratio of the reacting substances can be identified. 2 Na + 2 H 2 O H NaOH For every 2 mol of Na that react, 2 mol of H 2 O react, a 2:2 or 1:1 ratio. Thus, the 1.04 mol Na will be the limiting reactant.
45 Limiting Reactants Step 3 is to calculate the number of moles of each species that reacts or is produced. This can be done by assembling the data into a table. 2 Na + NaOH 2 H 2 O H 2 +2 Grams at start Molar mass, g/mol Moles at start Moles used ( ),
46 Limiting Reactants Step 4 is to calculate the number of moles of each species that remains after the reaction. 2 Na + 2 H 2 O H NaOH Grams at start Molar mass, g/mol Moles at start
47 Limiting Reactants Step 5 is to change the number of moles of each species to grams. 2 Na + 2 H 2 O H NaOH Moles at end mol H 2 O = 5.2 g H 2 O 0.52 mol H 2 = 1.0 g H 2
48 Limiting Reactants Returning to the original problem statement: A 24.0-g piece of solid sodium is added to 24.0 g of liquid water. How many grams of hydrogen will be produced? How many grams of which reactant will be left over? The questions can now be answered: 1.0 g H 2 is produced
49 Limiting Reactants Goal 5 Given a chemical equation, or information from which it may be determined, and initial quantities of two or more reactants, (a) identify the limiting reactant, (b) calculate the theoretical yield of a specified product, assuming complete use of the limiting reactant, and (c) calculate the quantity of reactant initially in excess that remains unreacted.
50 Limiting Reactants Smaller-Amount Method How to Solve a Limiting Reactant Problem: 1. Calculate the amount of product that can be formed by the initial amount of each reactant. a) The reactant that yields the smaller amount of product is the limiting reactant. b) The smaller amount of product is the amount that will be formed when all of the limiting reactant is used up. 2. Calculate the amount of excess reactant that is used by the total amount of limiting reactant. 3. Subtract from the amount of excess reactant present initially the amount that is used by all of
51 Limiting Reactants Example: A 24.0-g piece of solid sodium is added to 24.0 g of liquid water. How many grams of hydrogen will be produced? How many grams of which reactant will be left over? Solution: Step 1 is to calculate the amount of product that can be formed by the initial amount of each reactant.
52 Limiting Reactants GIVEN: 24.0 g Na WANTED: g H 2 2 Na + 2 H 2 O H NaOH 24.0 g Na = 1.05 g H 2 GIVEN: 24.0 g H 2 O WANTED: g H g H 2 O
53 Limiting Reactants 24.0 g Na and excess H 2 O produces 1.05 g H g H 2 O and excess Na produces 1.34 g H 2 Step 1a: The reactant that yields the smallest amount of product is the limiting reactant, so Na is the limiting reactant. Step 1b: The smaller amount of product is the amount that will be formed when all of the limiting reactant is
54 Limiting Reactants Step 2 is to calculate the amount of excess reactant that is used by the total amount of limiting reactant. The total amount of limiting reactant is 24.0 g Na. The excess reactant is H 2 O. GIVEN: 24.0 g Na WANTED: g H 2 O 2 Na + 2 H 2 O H NaOH
55 Limiting Reactants Step 3 is to subtract from the amount of excess reactant present initially the amount that is used by all of the limiting reactant. The difference is the amount of excess reactant left g H 2 O initially 18.8 g H 2 O reacted
56 Reaction to be Studied 2 Al(s) + 3 Cl 2 (g) f Al 2 Cl 6 (s)
57 PROBLEM: Mix 5.40 g of Al with 8.10 g of Cl 2. What mass of Al 2 Cl 6 can form? Mass reactant Mass product Moles reactant Stoichiometric factor Moles product
58 Step 1 of LR problem: compare actual mole ratio of reactants to theoretical mole ratio. 2 Al(s) + 3 Cl 2 (g) f Al 2 Cl 6 (s) Reactants must be in the mole
59 Step 2 of LR problem: Calculate moles of each reactant We have 5.40 g of Al and 8.10 g of Cl 2
60 Find mole ratio of reactants 2 Al(s) + 3 Cl 2 (g) f Al 2 Cl 6 (s) mol Al x = mol Cl 2 2.needed to react with mol Al, but we only have mole of Cl 2, so Limiting reactant is Cl 2
61 Mix 5.40 g of Al with 8.10 g of Cl 2. What mass of Al 2 Cl 6 can form? 2 Al(s) + 3 Cl 2 (g) f Al 2 Cl 6 (s) Limiting reactant = Cl 2 Base all calcs. on Cl 2 mass Cl 2 mass Al 2 Cl 6 moles Cl 2 moles Al 2 Cl 6
62 CALCULATIONS: calculate mass of Al 2 Cl 6 expected. Step 1: Calculate moles of Al 2 Cl 6 expected based on LR. Step 2: Calculate mass of Al 2 Cl 6 expected based on LR.
63 How much of which reactant will remain when reaction is complete? 1.Cl 2 was the limiting reactant. Therefore, Al was present in excess. But how much? 2. First find how much Al was required.
64 Calculating Excess Al 2 Al + 3 Cl 2 products mol mol = LR Excess Al = Al available - Al required = mol mol = mol Al in excess
65 Energy Goal 6 Given energy in one of the following units, calculate the other three: joules, kilojoules, calories, and kilocalories.
66 Energy Energy The ability to do work or transfer heat. Energy Unit: Joule Joule (J) The amount of energy exerted when a force of one newton (force required to cause a mass of 1 kg to accelerate at a rate of 1 m/s 2 ) is applied over a displacement of one meter: 1 joule = 1 newton 1 meter 1 J = 1 kg m 2 /sec 2
67 Energy Energy Unit: Calorie calorie (historical definition): Amount of energy required to raise the temperature of 1 g of water by 1 C. calorie (modern definition) 1 cal J A food Calorie (Cal) is a thermochemical kilocalorie. In scientific writing it is capitalized; in everyday writing, interpret the context. 1 kcal = kj
68 Energy Example: How many joules are equivalent to food Calories? Solution: A food Calorie is a thermochemical kilocalorie. GIVEN: kcal WANTED: J PER: 1000 cal/kcal J/cal PATH: kcal cal J
69 Thermochemical Equations Goal 7 Given a chemical equation, or information from which it may be written, and the heat (enthalpy) of reaction, write the thermochemical equation either (a) with H to the right of the conventional equation or (b) as a reactant or product.
70 Thermochemical Equations Enthalpy Heat content of a system. Symbol: H H is the enthalpy of reaction, or, as chemists commonly call it, the heat of reaction. means change in : It is determined by subtracting the initial quantity from the final quantity: A = final value of A initial value of A
71 Thermochemical Equations Enthalpy of Reaction, H If the final heat content of a system is less than its initial heat content, H is negative, and the change is exothermic. If the final heat content of a system is greater than its initial heat content, H is positive, and the change is endothermic.
72 Thermochemical Equations Thermochemical Equation A conventional equation plus its associated H term. Thermochemical equations are typically written in one of two different ways, depending on the context for which it is needed. Example: When one mole of acetylene gas reacts with two moles of hydrogen gas, one mole of ethane gas is formed and 311 kj of energy is released. Write the thermochemical equation in two forms. Solution: C 2 H 2 (g) + 2 H 2 (g) C 2 H 6 (g) kj C 2 H 2 (g) + 2 H 2 (g) C 2 H 6 (g) H = 311 kj
73 Thermochem Stoichiometry Goal 8 Given a thermochemical equation, or information from which it may be written, calculate the amount of energy released or added for a given amount of reactant or product; alternately, calculate the mass of reactant required to produce a given amount of energy.
74 Thermochem Stoichiometry The energy term in a thermochemical equation is directly proportional to the number of moles of all species in the reaction. C 2 H 2 (g) + 2 H 2 (g) C 2 H 6 (g) kj 311 kj 1 mol C 2 H 2
75 Thermochem Stoichiometry
76 Thermochem Stoichiometry Example: When propane, C 3 H 8 (g), is burned to form gaseous carbon dioxide and liquid water, kj of heat is released for every mole of propane burned. What quantity of heat is released when g of propane is burned? Solution: First, write and balance the thermochemical equation to determine the stoichiometric relationships.
77 Thermochem Stoichiometry GIVEN: g C 3 H 8 WANTED: quantity of heat (assume kj) PER: 1 mol C 3 H 8 /44.09 g C 3 H 8 PATH: g C 3 H 8 C 3 H 8 mol kj/1 mol C 3 H 8 kj
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