CHAPTER 9STOICHIOMETRY

9.1 & 9.2INTRODUCTION TO STOICHIOMETRY AND

IDEAL STOICHIOMETRIC CALCULATIONS

All chemical reactions are represented by a balanced chemical equation.

9.1

All chemical reactions are represented by a balanced chemical equation.

The coefficients represent the mole ratio between the reactants and products.

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

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?

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”?

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.

9.1

2Al + 6HCl 2AlCl3 + 3H2

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?

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?

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

9.1

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

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)

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.

9.1

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

9.1

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

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.

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).

9.1

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

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.

9.1