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Stoichiometry Chapter 12.

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Presentation on theme: "Stoichiometry Chapter 12."— Presentation transcript:

1 Stoichiometry Chapter 12

2 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.

3 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? ______

4 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___

5 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? ___

6 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_

7 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!

8 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 mol N2 Solve and round to significant digits!

9 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 mol N2 = 1.2 moles of NH3

10 2Fe + 3CuSO4  Fe2(SO4)3 + 3 Cu You have 1.5 moles of Fe. How many moles of Fe2(SO4)3 can be made?

11 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 mol Fe Solve, round, label!

12 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 mol Fe = 0.75 mol Fe2(SO4)3

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

14 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 moles Ag mole Mg

15 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 moles Ag mole Mg = 10 moles Ag (remember, 3 or LESS significant digits)

16 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

17 4Al + 3O2  2Al2O3 You have grams Al. How much Al2O3 can be made? 1. Convert the mass of the reactant to moles

18 4Al + 3O2  2Al2O3 You have 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 = mol Al g Al Don’t round until the very end!

19 4Al + 3O2  2Al2O3 You have grams Al. How much Al2O3 can be made? 2. Calculate the moles of the product mol Al x mol Al2O3 = mol Al mol Al2O3 (don’t round yet!)

20 4Al + 3O2  2Al2O3 You have grams Al. How much Al2O3 can be made? 3. Convert the moles of the product to mass mol Al2O3 x g Al2O3 = mol Al2O3 g Al2O3 (now you round!) = 60.46 g Al2O3

21 2HCl + Mg  MgCl2 + H2 You have 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

22 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles

23 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles g HCl x mol HCl = g HCl

24 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 1. Convert the mass of the reactant to moles g HCl x mol HCl g HCl = mol HCl

25 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product

26 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product mol HCl x mol H = mol HCl

27 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 2. Calculate the moles of the product mol HCl x mol H = mol HCl = mol H2

28 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass

29 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass mol H2 x g H2 = mol H2

30 2HCl + Mg  MgCl2 + H2 You have g of HCl. How many grams of H2 can be produced? 3. Convert the moles of the product to mass mol H2 x g H2 = mol H2 = = g H2

31 2O2 + CH4  CO2 + 2H2O You have 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

32 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 1. Convert the mass of the reactant to moles

33 2O2 + CH4  CO2 + 2H2O You have 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 g O2

34 2O2 + CH4  CO2 + 2H2O You have 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 g O2 = mol O2

35 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product

36 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product mol O2 x 1 mol CO2 mol O2

37 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 2. Calculate the moles of the product mol O2 x 1 mol CO2 mol O2 = mol CO2

38 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass

39 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass mol CO2 x g CO2 mol CO2

40 2O2 + CH4  CO2 + 2H2O You have g of O2. How many grams of CO2 can be produced? 3. Convert the moles of the product to mass mol CO2 x g CO2 mol CO2 = = g CO2

41 Agenda Now, we will practice!!!

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