Stoichiometry Chapter 12.

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Presentation transcript:

Stoichiometry Chapter 12

Stoichiometry The calculation of quantities in chemical reactions is a subject of chemistry called stoichiometry. Using a balanced equation, we will calculate the amount of reactant or product needed.

Coefficients = Moles Use the equation below to determine the number of moles of each compound: N2 + 3H2  2 NH3 How many moles of N2? _____ How many moles of H2? _____ How many moles of NH3? ______

Coefficients = Moles Use the equation below to determine the number of moles of each compound: N2 + 3H2  2 NH3 How many moles of N2? __1___ How many moles of H2? __3___ How many moles of NH3? ___2___

Coefficients = Moles Use the equation below to determine the number of moles of each compound: N2 + 3H2  2 NH3 If you have 3 moles of H2 available for the reaction, how many moles of NH3 can you make? ___

Coefficients = Moles Use the equation below to determine the number of moles of each compound: N2 + 3H2  2 NH3 If you have 3 moles of H2 available for the reaction, how many moles of NH3 can you make? _2_

Calculating the MOLES of a Product Using the same equation, N2 + 3H2  2 NH3 Calculate the number of moles of NH3 that are produced when 0.60 moles of N2 reacts with H2 Start with what you know, put it over 1!

N2 + 3H2  2 NH3 Calculate the number of moles of NH3 that are produced when 0.60 moles of N2 reacts with H2 0.60 moles N2 x 2 mol NH3 1 1 mol N2 Solve and round to significant digits!

N2 + 3H2  2 NH3 Calculate the number of moles of NH3 that are produced when 0.60 moles of N2 reacts with H2 0.60 moles N2 x 2 mol NH3 1 1 mol N2 = 1.2 moles of NH3

2Fe + 3CuSO4  Fe2(SO4)3 + 3 Cu You have 1.5 moles of Fe. How many moles of Fe2(SO4)3 can be made?

2Fe + 3CuSO4  Fe2(SO4)3 + 3 Cu You have 1.5 moles of Fe. How many moles of Fe2(SO4)3 can be made? 1.5 moles Fe x 1 mol Fe2(SO4)3 1 2 mol Fe Solve, round, label!

2Fe + 3CuSO4  Fe2(SO4)3 + 3 Cu You have 1.5 moles of Fe. How many moles of Fe2(SO4)3 can be made? 1.5 moles Fe x 1 mol Fe2(SO4)3 1 2 mol Fe = 0.75 mol Fe2(SO4)3

Mg + 2AgNO3  Mg(NO3)2 + 2Ag You have 5.00 moles of Mg. How many moles of silver can be made?

Mg + 2AgNO3  Mg(NO3)2 + 2Ag You have 5.00 moles of Mg. How many moles of silver can be made? 5.00 moles Mg x 2 moles Ag 1 1 mole Mg

Mg + 2AgNO3  Mg(NO3)2 + 2Ag You have 5.00 moles of Mg. How many moles of silver can be made? 5.00 moles Mg x 2 moles Ag 1 1 mole Mg = 10 moles Ag (remember, 3 or LESS significant digits)

Calculating the MASS of a product 1. Convert the mass of the reactant to moles 2. Calculate the moles of the product 3. Convert the moles of the product to mass

4Al + 3O2  2Al2O3 You have 32.00 grams Al. How much Al2O3 can be made? 1. Convert the mass of the reactant to moles

4Al + 3O2  2Al2O3 You have 32.00 grams Al. How much Al2O3 can be made? 1. Convert the mass of the reactant to moles 32.00 g Al x 1 mole Al = 1.185975836 mol Al 1 26.982 g Al Don’t round until the very end!

4Al + 3O2  2Al2O3 You have 32.00 grams Al. How much Al2O3 can be made? 2. Calculate the moles of the product 1.185975836 mol Al x 2 mol Al2O3 = 1 4 mol Al 0.592987918 mol Al2O3 (don’t round yet!)

4Al + 3O2  2Al2O3 You have 32.00 grams Al. How much Al2O3 can be made? 3. Convert the moles of the product to mass 0.592987918 mol Al2O3 x 101.961 g Al2O3 = 1 1 mol Al2O3 60.461641 g Al2O3 (now you round!) = 60.46 g Al2O3

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles 2. Calculate the moles of the product 3. Convert the moles of the product to mass

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles 125.00 g HCl x 1 mol HCl = 1 36.4609 g HCl

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles 125.00 g HCl x 1 mol HCl 1 36.4609 g HCl = 3.428330074 mol HCl

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product 3.428330074 mol HCl x 1 mol H2 = 1 2 mol HCl

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product 3.428330074 mol HCl x 1 mol H2 = 1 2 mol HCl =1.714165037 mol H2

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass 1.714165037 mol H2 x 2.0158 g H2 = 1 1 mol H2

2HCl + Mg  MgCl2 + H2 You have 125.00 g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass 1.714165037 mol H2 x 2.0158 g H2 = 1 1 mol H2 = 3.455413882 = 3.4554 g H2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 1. Convert the mass of the reactant to moles 2. Calculate the moles of the product 3. Convert the moles of the product to mass

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 1. Convert the mass of the reactant to moles

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 1. Convert the mass of the reactant to moles 75.00 g O2 x 1 mol O2 1 31.998 g O2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 1. Convert the mass of the reactant to moles 75.00 g O2 x 1 mol O2 1 31.998 g O2 = 2.343896494 mol O2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product 2.343896494 mol O2 x 1 mol CO2 1 2 mol O2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product 2.343896494 mol O2 x 1 mol CO2 1 2 mol O2 = 1.171948247 mol CO2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass 1.171948247 mol CO2 x 44.009 g CO2 1 1 mol CO2

2O2 + CH4  CO2 + 2H2O You have 75.00 g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass 1.171948247 mol CO2 x 44.009 g CO2 1 1 mol CO2 = 51.5762704 = 51.58 g CO2

Agenda Now, we will practice!!!