1. CHAPTER 9
Design: Winter
Colors: Elemental
STOICHIOMETRY

2. 9.1 & 9.2
INTRODUCTION TO STOICHIOMETRY AND IDEAL STOICHIOMETRIC CALCULATIONS

3. 9.1
All chemical reactions are represented by a balanced chemical equation.

4. 9.1
All chemical reactions are represented by a balanced chemical equation. The coefficients represent the mole ratio between the reactants and products.

5. 9.1
All chemical reactions are represented by a balanced chemical equation. The coefficients represent the mole ratio between the reactants and products. 2Al + 6HCl  2AlCl3 + 3H2

6. 9.1
All chemical reactions are represented by a balanced chemical equation. The coefficients represent the mole ratio between the reactants and products. 2Al + 6HCl  2AlCl3 + 3H2 How could this ratio be used to predict that amount of product that theoretically will be produced in a chemical reaction?

7. 9.1
All chemical reactions are represented by a balanced chemical equation. The coefficients represent the mole ratio between the reactants and products. 2Al + 6HCl  2AlCl3 + 3H2 How could this ratio be used to predict that amount of product that theoretically will be produced in a chemical reaction? Why does it say “theoretically”?

8. 9.1
All chemical reactions are represented by a balanced chemical equation. The coefficients represent the mole ratio between the reactants and products. 2Al + 6HCl  2AlCl3 + 3H2 Once the number of moles is known, conversion factors (using these molar ratios) will be used to change from one compound to another.

9. 2Al + 6HCl  2AlCl3 + 3H2

10. 9.1
2Al + 6HCl  2AlCl3 + 3H2 How many moles of HCl are required to react with 8 moles of Al? How many moles of hydrogen gas would theoretically be produced?

11. 9.1
CaCO3 + 2HCl  CaCl2 + H2O + CO2 How many moles of hydrochloric acid would be required to react with 2.5 moles of calcium carbonate? How many grams of carbon dioxide would theoretically be produced?

12. 9.1
Ex 1: Determine the mass of lithium hydroxide theoretically produced when 0.38g of lithium nitride reacts with water according to the following equation: Li3N + 3H2O  NH3 + 3LiOH

13. 9.1
Ex 2: What mass of sodium chloride is theoretically produced when chlorine reacts with 0.29g of sodium iodide?

14. 9.1
Ex 3: Determine the liters of carbon dioxide that are theoretically produced when 0.85g of butane (C4H10) undergoes a complete combustion reaction. (Assume STP conditions)

15. 9.1
Ex 4: Determine the mass of antimony theoretically produced when 0.46g of antimony (III) oxide reacts with carbon to produce antimony metal and carbon monoxide.

16. 9.1
Ex 5: What mass of hydrogen peroxide must decompose to theoretically produce 2.58 x 1022 molecules of water?

17. 9.1
Ex 6: What volume of carbon monoxide (at STP) must react with oxygen to theoretically produce 0.69g of carbon dioxide?

18. 9.1
Ex 7: Determine the mass of sodium nitrate theoretically produced when 0.73g of nickel (II) nitrate reacts with sodium hydroxide in a double displacement reaction.

19. 9.1
Ex 8: Determine the mass of calcium hydroxide theoretically produced when calcium carbide (CaC2) reacts with 0.64g of water to produce calcium hydroxide and dicarbon dihydride (acetylene gas).

20. 9.1
Ex 9: How many grams of ozone (O3) must decompose to theoretically produce 0.61L of oxygen (at STP)?

21. 9.1
Ex 10: If chlorine gas is bubbled through a potassium iodide solution, elemental iodine is produced. Calculate the theoretical mass of iodine collected when 4.50 x 103g of chlorine gas is used. Assume an excess of potassium iodide.