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Chapter 3 Calculations with Chemical Formulas and Equations HSTMr. Watson
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HST Molar Mass Sum atomic masses represented by formula atomic masses => gaw molar mass => MM
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Mr. WatsonHST One Mole of each Substance Clockwise from top left: 1-Octanol, C 8 H 17 OH; Mercury(II) iodide, HgI 2 ; Methanol, CH 3 OH; and Sulfur, S 8.
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Mr. WatsonHST Example What is the molar mass of ethanol, C 2 H 5 OH?
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Mr. WatsonHST Example What is the molar mass of ethanol, C 2 H 5 O 1 H 1 ? MM = 2(gaw) C + (5 + 1)(gaw) H + 1(gaw) O
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Mr. WatsonHST Example What is the molar mass of ethanol, C 2 H 5 OH? MM = 2(gaw) C + (5 + 1)(gaw) H + 1(gaw) O = 2(12.011) C + 6(1.00794) H + 1(15.9994) O
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Mr. WatsonHST Example What is the molar mass of ethanol, C 2 H 5 OH? MM = 2(gaw) C + (5 + 1)(gaw) H + 1(gaw) O = 2(12.011) C + 6(1.00794) H + 1(15.9994) O = 46.069 g/mol
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Mr. WatsonHST The Mole a unit of measurement, quantity of matter present Avogadro’s Number 6.022 x 10 23 particles Latin for “pile”
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide?
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2 = (10.00g)
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2 = (10.00g)(1 mol/44.01g)
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2 = (10.00g)(1 mol/44.01g)
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2 = (10.00)(1 mol/44.01)
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Mr. WatsonHST Example How many moles of carbon dioxide molecules are there in 10.00g of carbon dioxide? MM = 1(gaw) C + 2(gaw) O = 44.01 g/mol #mol CO 2 = (10.00)(1 mol/44.01) = 0.2272 mol
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Mr. WatsonHST Combustion Analysis
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Mr. WatsonHST Percentage Composition description of a compound based on the relative amounts of each element in the compound
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = (12.011 + 1.00797 + 3*35.453)amu = 119.377amu
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = (12.011 + 1.00797 + 3*35.453)amu = 119.377amu 1(gaw) %C = ------------ X 100 MM
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = (12.011 + 1.00797 + 3*35.453)amu = 119.377amu 1(gaw) %C = ------------ X 100 MM 1(12.011) %C = -------------- X 100 = 10.061% C 119.377
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = (12.011 + 1.00797 + 3*35.453)amu = 119.377amu 1(1.00797) %H = ---------------- X 100 = 0.844359% H 119.377
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = (12.011 + 1.00797 + 3*35.453)amu = 119.377amu 3(35.453) %Cl = -------------- X 100 = 89.095% Cl 119.377
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Mr. WatsonHST EXAMPLE: What is the percent composition of chloroform, CHCl 3, a substance once used as an anesthetic? MM = 1(gaw) C + 1(gaw) H + 3(gaw) Cl = 119.377amu %C = 10.061% C %H = 0.844359% H %Cl = 89.095% Cl
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Mr. WatsonHST Simplest (Empirical) Formula formula describing a substance based on the smallest set of subscripts
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Mr. WatsonHST Acetylene, C 2 H 2, and benzene, C 6 H 6, have the same empirical formula. Is the correct empirical formula: C 2 H 2 CH C 6 H 6
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Mr. WatsonHST EXAMPLE: A white compound is formed when phosphorus burns in air. Analysis shows that the compound is composed of 43.7% P and 56.3% O by mass. What is the empirical formula of the compound? Relative Number of Atoms Element % (%/gaw) P 43.7 43.7/30.97 = 1.41 O 56.3 56.3/15.9994 = 3.52
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Mr. WatsonHST EXAMPLE: A white compound is formed when phosphorus burns in air. Analysis shows that the compound is composed of 43.7% P and 56.3% O by mass. What is the empirical formula of the compound? Relative Number of Atoms Element % (%/gaw) Divide by Smaller P 43.7 43.7/30.97 = 1.41 1.41/1.41 = 1.00 O 56.3 56.3/15.9994 = 3.52 3.52/1.41 = 2.50
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Mr. WatsonHST EXAMPLE: A white compound is formed when phosphorus burns in air. Analysis shows that the compound is composed of 43.7% P and 56.3% O by mass. What is the empirical formula of the compound? Relative Number of Atoms Multiply % (%/gaw) Divide by Smaller by Integer P 43.7 43.7/30.97 = 1.41 1.41/1.41 = 1.00 2*1.00 => 2 O 56.3 56.3/15.9994 = 3.52 3.52/1.41 = 2.50 2*2.50 => 5
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Mr. WatsonHST EXAMPLE: A white compound is formed when phosphorus burns in air. Analysis shows that the compound is composed of 43.7% P and 56.3% O by mass. What is the empirical formula of the compound? Relative Number of Atoms Multiply % (%/gaw) Divide by Smaller by Integer P 43.7 43.7/30.97 = 1.41 1.41/1.41 = 1.00 2*1.00 => 2 O 56.3 56.3/15.9994 = 3.52 3.52/1.41 = 2.50 2*2.50 => 5 Empirical Formula => P 2 O 5
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Mr. WatsonHST EXAMPLE: A sample of a brown-colored gas that is a major air pollutant is found to contain 2.34 g of N and 5.34 g of O. What is the empirical formula of the compound? 2.34 %N = ----------------- X 100 = 30.5% N 2.34 + 5.34 5.34 %O = ----------------- X 100 = 69.5% O 2.34 + 5.34
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Mr. WatsonHST EXAMPLE: A sample of a brown-colored gas that is a major air pollutant is found to contain 2.34 g of N and 5.34 g of O. What is the empirical formula of the compound? %N = 30.5% N%O = 69.5% O Relative # Atoms Element %(%/gaw) N 30.5 30.5/14.0067 = 2.18 O 69.5 69.5/15.9994 = 4.34
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Mr. WatsonHST EXAMPLE: A sample of a brown-colored gas that is a major air pollutant is found to contain 2.34 g of N and 5.34 g of O. What is the empirical formula of the compound? %N = 30.5% N%O = 69.5% O Relative # Atoms %(%/gaw) Divide by Smaller N 30.5 30.5/14.0067 = 2.18 2.18/2.18 = 1.00 O 69.5 69.5/15.9994 = 4.34 4.34/2.18 = 1.99
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Mr. WatsonHST EXAMPLE: A sample of a brown-colored gas that is a major air pollutant is found to contain 2.34 g of N and 5.34 g of O. What is the empirical formula of the compound? %N = 30.5% N%O = 69.5% O Relative # Atoms Multiply %(%/gaw) Divide by Smallerby Integer N 30.5 30.5/14.0067 = 2.18 2.18/2.18 = 1.00 1*1.00=>1 O 69.5 69.5/15.9994 = 4.34 4.34/2.18 = 1.99 1*1.99=>2
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Mr. WatsonHST EXAMPLE: A sample of a brown-colored gas that is a major air pollutant is found to contain 2.34 g of N and 5.34 g of O. What is the empirical formula of the compound? %N = 30.5% N%O = 69.5% O Relative # Atoms Multiply %(%/gaw) Divide by Smallerby Integer N 30.5 30.5/14.0067 = 2.18 2.18/2.18 = 1.00 1*1.00=>1 O 69.5 69.5/15.9994 = 4.34 4.34/2.18 = 1.99 1*1.99=>2 Empirical Formula => NO 2
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Mr. WatsonHST Molecular Formula the exact proportions of the elements that are formed in a molecule
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Mr. WatsonHST Molecular Formula from Simplest Formula empirical formula => EF molecular formula => MF MF = X * EF
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Mr. WatsonHST Molecular Formula from Simplest Formula formula mass => FM sum of the atomic weights represented by the formula molar mass = MM = X * FM
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Mr. WatsonHST Molecular Formula from Simplest Formula first, knowing MM and FM X = MM/FM then MF = X * EF
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Mr. WatsonHST EXAMPLE: A colorless liquid used in rocket engines, whose empirical formula is NO 2, has a molar mass of 92.0. What is the molecular formula? FM = 1(gaw) N + 2(gaw) O = 46.0 MM 92.0 X = ------- = -------- = 2 FM 46.0
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Mr. WatsonHST EXAMPLE: A colorless liquid used in rocket engines, whose empirical formula is NO 2, has a molar mass of 92.0. What is the molecular formula? FM = 1(gaw) N + 2(gaw) O = 46.0 MM 92.0 X = ------- = -------- = 2 FM 46.0 thus MF = 2 * EF
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Mr. WatsonHST What is the correct molecular formula for this colorless liquid rocket fuel? 2NO NO N 2 O 4
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Mr. WatsonHST Stoichiometry stoi·chi·om·e·try noun 1. Calculation of the quantities of reactants and products in a chemical reaction. 2. The quantitative relationship between reactants and products in a chemical reaction.
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Mr. WatsonHST The Mole and Chemical Reactions: The Macro-Nano Connection 2 H 2 + O 2 -----> 2 H 2 O 2 H 2 molecules 1 O 2 molecule 2 H 2 O molecules 2 H 2 moles molecules 1 O 2 mole molecules 2 H 2 O moles molecules 4 g H 2 32 g O 2 36 g H 2 O
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Mr. WatsonHST EXAMPLE How much H 2 O, in moles results from burning an excess of H 2 in 3.3 moles of O 2 ? H 2 + O 2 -----> H 2 O 2 H 2 + O 2 -----> 2 H 2 O
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Mr. WatsonHST EXAMPLE How much H 2 O, in moles results from burning an excess of H 2 in 3.3 moles of O 2 ? H 2 + O 2 -----> H 2 O 2 H 2 + O 2 -----> 2 H 2 O (3.3 mol O 2 ) (2 mol H 2 O) #mol H 2 O = ------------------------------------ (1 mol O 2 )
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Mr. WatsonHST EXAMPLE How much H 2 O, in moles results from burning an excess of H 2 in 3.3 moles of O 2 ? H 2 + O 2 -----> H 2 O 2 H 2 + O 2 -----> 2 H 2 O (3.3 mol O 2 ) (2 mol H 2 O) #mol H 2 O = ------------------------------------ (1 mol O 2 )
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Mr. WatsonHST EXAMPLE How much H 2 O, in moles results from burning an excess of H 2 in 3.3 moles of O 2 ? H 2 + O 2 -----> H 2 O 2 H 2 + O 2 -----> 2 H 2 O (3.3) (2 mol H 2 O) #mol H 2 O = ------------------------ = 6.6 mol H 2 O (1)
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Mr. WatsonHST Combination Reaction PbNO 3(aq) + K 2 CrO 4(aq) PbCrO 4(s) + 2 KNO 3(aq) Colorless yellow yellow colorless
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Mr. WatsonHST Stoichiometric Roadmap
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additional 10% mass of iron. http://www.cbu.edu/~mcondren/Demos/Thermite-Welding.ppt
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additional 10% mass of iron. The mass of iron in 1 inch of this rail is: #g/in = (132 #/yard) (1 yard/36 in) (454 g/#) = 1.67 X 10 3 g/in
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additional 10% mass of iron. The mass of iron in 1 inch of this rail is: #g/in = (132) (1/36 in) (454 g) = 1.67 X 10 3 g/in The mass of iron in a weld adding 10% mass: #g = (1.67 X 10 3 g) (0.10) = 167 g
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in 1 inch of this rail is: #g/in = (132 #/yard) (1 yard/36 in) (454 g/#) = 1.67 X 10 3 g/in The mass of iron in a weld adding 10% mass: #g = (1.67 X 10 3 g) (0.10) = 167 g Balanced chemical equation: Fe 2 O 3 + 2 Al ---> 2 Fe + Al 2 O 3
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in 1 inch of this rail is: #g/in = (132 #/yard) (1 yard/36 in) (454 g/#) = 1.67 X 10 3 g/in The mass of iron in a weld adding 10% mass: #g = (1.67 X 10 3 g) (0.10) = 167 g Balanced chemical equation: Fe 2 O 3 + 2 Al ---> 2 Fe + Al 2 O 3 What mass of Fe 2 O 3 is required for the thermite process?
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in a weld adding 10% mass: #g = (1.67 X 10 3 g) (0.10) = 167 g Balanced chemical equation: Fe 2 O 3 + 2 Al ---> 2 Fe + Al 2 O 3 What mass of Fe 2 O 3 is required for the thermite process? (1 mol Fe) (1 mol Fe 2 O 3 ) (159.7 g Fe 2 O 3 ) #g Fe 2 O 3 = (167 g Fe) * ------------------------------------------------------- (55.85 g Fe) (2 mol Fe) (1 mol Fe 2 O 3 ) = 238 g Fe 2 O 3
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in a weld adding 10% mass: #g Fe = 167 g Fe Balanced chemical equation: Fe 2 O 3 + 2 Al ---> 2 Fe + Al 2 O 3 What mass of Fe 2 O 3 is required for the thermite process? #g Fe 2 O 3 = 238 g Fe 2 O 3 What mass of Al is required for the thermite process?
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in a weld adding 10% mass: #g Fe = 167 g Fe Balanced chemical equation: Fe 2 O 3 + 2 Al ---> 2 Fe + Al 2 O 3 What mass of Fe 2 O 3 is required for the thermite process? #g Fe 2 O 3 = 238 g Fe 2 O 3 What mass of Al is required for the thermite process? (1 mol Fe) (2 mol Al) (26.9815 g Al) #g Al = (167 g Fe) * ----------------------------------------------- (55.85 g Fe) (2 mol Fe) (1 mol Al) = 80.6 g Al
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Mr. WatsonHST EXAMPLE How much iron(III) oxide and aluminum powder are required to field weld the ends of two rails together? Assume that the rail is 132 lb/yard and that one inch of the rails will be covered by an additonal 10% mass of iron. The mass of iron in a weld adding 10% mass: #g Fe = 167 g Fe #g Fe 2 O 3 = 238 g Fe 2 O 3 #g Al = 80.6 g Al
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Mr. WatsonHST Limiting Reactant reactant that limits the amount of product that can be produced
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Mr. WatsonHST EXAMPLE What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S)
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Mr. WatsonHST EXAMPLE What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) balanced equation relates: 2Fe 2 S 3(S) 6H 2 O (l) 3O 2(g)
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Mr. WatsonHSTEXAMPLE What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) balanced equation relates: 2Fe 2 S 3(S) 6H 2 O (l) 3O 2(g) have only: 1Fe 2 S 3(S) 2H 2 O (l) 3O 2(g)
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Mr. WatsonHST EXAMPLE What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) balanced equation relates: 2Fe 2 S 3(S) 6H 2 O (l) 3O 2(g) have only: 1Fe 2 S 3(S) 2H 2 O (l) 3O 2(g) not enough H 2 O to use all Fe 2 S 3 plenty of O 2
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Mr. WatsonHST EXAMPLE What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) if use all Fe 2 S 3 : (1.0 mol Fe 2 S 3 ) (4 mol Fe(OH) 3 ) #mol Fe(OH) 3 = ------------------------------------------ (2 mol Fe 2 S 3 ) = 2.0 mol Fe(OH) 3
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) if use all H 2 O: (2.0 mol H 2 O) (4 mol Fe(OH) 3 ) #mol Fe(OH) 3 = ----------------------------------------- (6 mol H 2 O) = 1.3 mol Fe(OH) 3
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) if use all O 2 (3.0 mol O 2 ) (4 mol Fe(OH) 3 ) #mol Fe(OH) 3 = --------------------------------------- (3 mol O 2 ) = 4.0 mol Fe(OH) 3
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) 1.0 mol Fe 2 S 3 => 2.0 mol Fe(OH) 3 2.0 mol H 2 O => 1.3 mol Fe(OH) 3 3.0 mol O 2 => 4.0 mol Fe(OH) 3
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) 1.0 mol Fe 2 S 3 => 2.0 mol Fe(OH) 3 2.0 mol H 2 O => 1.3 mol Fe(OH) 3 3.0 mol O 2 => 4.0 mol Fe(OH) 3 Since 2.0 mol H 2 O will produce only 1.3 mol Fe(OH) 3, then H 2 O is the limiting reactant. Thus the correct number of moles of Fe(OH) 3 is 1.33 moles.
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) 1.0 mol Fe 2 S 3 => 2.0 mol Fe(OH) 3 2.0 mol H 2 O => 1.3 mol Fe(OH) 3 least amount 3.0 mol O 2 => 4.0 mol Fe(OH) 3 Since 2.0 mol H 2 O will produce only 1.3 mol Fe(OH) 3, then H 2 O is the limiting reactant.
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Mr. WatsonHST EXAMPLE: What is the number of moles of Fe(OH) 3 (S) that can be produced by allowing 1.0 mol Fe 2 S 3, 2.0 mol H 2 O, and 3.0 mol O 2 to react? 2Fe 2 S 3(S) + 6H 2 O (l) + 3O 2(g) -----> 4Fe(OH) 3(S) + 6S (S) 1.0 mol Fe 2 S 3 => 2.0 mol Fe(OH) 3 2.0 mol H 2 O => 1.3 mol Fe(OH) 3 least amount 3.0 mol O 2 => 4.0 mol Fe(OH) 3 Since 2.0 mol H 2 O will produce only 1.3 mol Fe(OH) 3, then H 2 O is the limiting reactant. Thus the maximum number of moles of Fe(OH) 3 that can be produced by this reaction is 1.3 moles.
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Mr. WatsonHST Theoretical Yield the amount of product produced by a reaction based on the amount of the limiting reactant
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Mr. WatsonHST Actual Yield amount of product actually produced in a reaction
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Mr. WatsonHST Percent Yield actual yield % yield = --------------------- * 100 theoretical yield
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00 kg Cl 2 ) #kg N 2 H 4 = ---------------------
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00 kg Cl 2 ) (1000 g Cl 2 ) #kg N 2 H 4 = ----------------------------------- (1 kg Cl 2 ) metric conversion
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00) (1000 g Cl 2 ) (1 mol Cl 2 ) #kg N 2 H 4 = ----------------------------------------- (1) (70.9 g Cl 2 ) molar mass
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1 mol Cl 2 ) #kg N 2 H 4 = ----------------------------------------- (1)(70.9)
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1 mol Cl 2 )(1 mol N 2 H 4 ) #kg N 2 H 4 = ------------------------------------------------- (1) (70.9) (1 mol Cl 2 )
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1)(1 mol N 2 H 4 ) #kg N 2 H 4 = ------------------------------------------------- (1) (70.9)(1)
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1)(1 mol N 2 H 4 ) (32.0 g N 2 H 4 ) #kg N 2 H 4 = -------------------------------------------------------- (1)(70.9) (1) (1 mol N 2 H 4 ) molar mass
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1)(1) (32.0 g N 2 H 4 )(1 kg N 2 H 4 ) #kg N 2 H 4 = ---------------------------------------------------------- (1)(70.9)(1)(1) (1000 g N 2 H 4 ) metric conversion
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1)(1) (32.0)(1 kg N 2 H 4 ) #kg N 2 H 4 = ---------------------------------------------------------- (1)(70.9)(1)(1)(1000)
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) to calculate the theoretical yield, use the net equation for the overall process (1.00)(1000)(1)(1) (32.0)(1 kg N 2 H 4 ) #kg N 2 H 4 = ---------------------------------------------------------- (1)(70.9)(1)(1)(1000) = 0.451 kg N 2 H 4
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) theoretical yield#kg N 2 H 4 = 0.451 kg N 2 H 4 (b) actual yield (0.299 kg product) # kg N 2 H 4 = --------------------------
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) theoretical yield#kg N 2 H 4 = 0.451 kg N 2 H 4 (b) actual yield (0.299 kg product) (98.0 kg N 2 H 4 ) # kg N 2 H 4 = -------------------------------------------- (100 kg product) purity factor
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) theoretical yield#kg N 2 H 4 = 0.451 kg N 2 H 4 (b) actual yield (0.299 kg product) (98.0 kg N 2 H 4 ) # kg N 2 H 4 = -------------------------------------------- (100 kg product) = 0.293 kg N 2 H 4
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) theoretical yield#kg N 2 H 4 = 0.451 kg N 2 H 4 (b) actual yield# kg N 2 H 4 = 0.293 kg N 2 H 4
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Mr. WatsonHST EXAMPLE A chemical plant obtained 0.299 kg of 98.0% N 2 H 4 for every 1.00 kg of Cl 2 that is reacted with excess NaOH and NH 3. What are the: (a) theoretical, (b) actual, and (c) percent yield of pure N 2 H 4 ? 2NaOH + Cl 2 + 2NH 3 -----> N 2 H 4 + 2NaCl + 2H 2 O (a) theoretical yield#kg N 2 H 4 = 0.451 kg N 2 H 4 (b) actual yield# kg N 2 H 4 = 0.293 kg N 2 H 4 (c) percent yield 0.293 kg % yield = -------------- X 100 = 65.0 % yield 0.451kg
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