the Mole !

It’s time to learn about . . .It’s time to learn about . . .

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Anyone Can Roast Beef.

StoichiometryStoichiometry

Stoichiometry : Mole Ratios to Stoichiometry : Mole Ratios to Determining Grams of ProductDetermining Grams of ProductAt the conclusion of our time At the conclusion of our time together, you should be able to:together, you should be able to:

1. Review the conversion of particles or grams to moles

2. Determine mole ratios from a balanced chemical equation

3. Determine the amount of product produced when given the amount of reactants

Review the Molar Mass of Review the Molar Mass of CompoundsCompounds

The molar mass (MM) of a compound is determined by adding up all the atomic masses for the molecule (or compound)

◦Ex. Molar mass of CaCl2◦Avg. Atomic mass of Calcium = 40.08g◦Avg. Atomic mass of Chlorine = 35.45g◦Molar Mass of calcium chloride =

40.08 g/mol Ca + (2 X 35.45) g/mol Cl 110.98 g/mol CaCl2

17Cl

35.45

20

Ca  40.08

PracticePractice

Calculate the Molar Mass of calcium phosphate◦Formula = ◦Masses elements:

◦Molar Mass =310.18 g

Ca3(PO4)2

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CalculationsCalculations

molar mass Avogadro’s

number Grams MolesMoles

Particles

Everything must go through Moles!!!Everything must go through Moles!!!

FlowchartFlowchartAtoms or Molecules

Moles

Mass (grams)

Divide by 6.02 X 1023

Multiply by 6.02 X 1023 Multiply by

atomic/molar mass from periodic tableDivide by

atomic/molar mass from periodic table

Chocolate Chip Cookies!!Chocolate Chip Cookies!!1 cup butter 2 eggs 1/2 cup white sugar 1

teaspoon salt 1 cup packed brown sugar 1 teaspoon vanilla extract 2 1/2 cups all-purpose flour 1 teaspoon baking soda 2 cups semisweet chocolate chipsMakes 3 dozenHow many eggs are needed to make 3 dozen cookies?

How much butter is needed for the amount of chocolate chips used?

How much brown sugar would I need if I had 1½ cups white sugar?

Cookies and Chemistry…Huh!?!?Cookies and Chemistry…Huh!?!?

Just like chocolate chip Just like chocolate chip cookies have recipes, cookies have recipes, chemists have recipes as wellchemists have recipes as well

Instead of calling them Instead of calling them recipes, we call them recipes, we call them chemical equationschemical equations

Furthermore, instead of using Furthermore, instead of using cups and teaspoons, we use cups and teaspoons, we use molesmoles

Lastly, instead of eggs, Lastly, instead of eggs, butter, sugar, etc. we use butter, sugar, etc. we use chemical compounds as chemical compounds as ingredientsingredients

Chemistry RecipesChemistry Recipes

Looking at a reaction tells us how much of something you need to react with something else to get a product (like the cookie recipe)

Be sure you have a balanced reaction before you start! Balance #1 on your worksheet!!

Example: 2 Ag+ Cl2 2 AgCl This reaction tells us that by mixing 2

moles of silver with 1 mole of chlorine we will get 2 moles of silver chloride

What if we wanted 4 moles of AgCl? 10 moles? 50 moles?

Let’s sit down and figure this out!!

PracticePractice

Write the balanced reaction for hydrogen gas reacting with oxygen gas.

2 H2 + O2 2 H2O

◦How many moles of reactants are needed?◦What if we wanted 4 moles of water?◦What if we had 3 moles of oxygen, how

much hydrogen would we need to react, and how much water would we get?

◦What if we had 50 moles of hydrogen, how much oxygen would we need, and how much water would be produced?

Mole RatiosMole Ratios

These mole ratios can be used to calculate the moles of one chemical from the given amount of a different chemical

Example: How many moles of chlorine are needed to react with 5 moles of silver (without any silver left over)?

2 Ag + Cl2 2 AgCl

5 Ag + 2.5 Cl2 5 AgCl

5 mol Ag

Question AnswerQuestion Answer

2 Ag+ Cl2 2 AgCl

# moles of Cl2 =

x 1 mol Cl22 mol Ag

= 2.5 mol Cl2

Mole-Mole ConversionsMole-Mole Conversions

How many moles of silver chloride will be produced if you react 2.6 moles of chlorine gas with an excess (more than you need) of silver metal?

2 Ag + Cl2 2 AgCl

2.6 mol Cl2 x

# moles of AgCl =

2 mol AgCl

1 mol Cl2

= 5.2 mol AgCl

Mass-MoleMass-Mole

We can also start with mass and convert to moles of product or another reactant

We use molar mass and the mole ratio to get to moles of the compound of interest◦Calculate the number of moles of the

combustion of ethane (C2H6) needed to produce 10.0 g of water

◦ 2 C2H6 + 7 O2 4 CO2 + 6 H20

Mass-MoleMass-Mole

2 C2H6 + 7 O2 4 CO2 + 6 H20

= 0.185 mol C2H6

10.0 g H2O x 1 mol H2O

18.02 g H2O

x 2 mol C2H6

6 mol H2O

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Stoichiometry Continued:Stoichiometry Continued:

Stoichiometry : Mole Ratios to Stoichiometry : Mole Ratios to Determining Grams of ProductDetermining Grams of ProductAt the conclusion of our time At the conclusion of our time together, you should be able to:together, you should be able to:

1. Review the conversion of particles or grams to moles

2. Determine mole ratios from a balanced chemical equation

3. Determine the amount of product produced when given the amount of reactants

Mass-Mass ConversionsMass-Mass Conversions

Most often we are given a starting mass and want to find out the mass of a product we will get (called theoretical yield) or how much of another reactant we need to completely react with it (no leftover ingredients!)

Now we must go from grams to moles, to mole ratios, and back to grams of the compound we are interested in.

Mass-Mass ConversionMass-Mass Conversion

Ex. Calculate how many grams of ammonia are produced when you react 2.00 g of nitrogen with excess hydrogen.

N2 + 3 H2 2 NH3

2.00 g N2 1 mol N2 2 mol NH3 17.04 g NH3

28.02 g N2 1 mol N2 1 mol NH3

= 2.43 g NH3

Practice Mass-Mole-MassPractice Mass-Mole-Mass

How many grams of calcium nitride are produced when 2.00 g of calcium reacts with an excess of nitrogen?

Ca + N2 Ca3N2

3 Ca + N2 Ca3N2

Mass-Mole-MassMass-Mole-Mass

3 Ca + N2 Ca3N2

= 2.47 g Ca3N2

2.00 g Ca x 1 mol Ca

40.08 g Cax 1 mol Ca3N2

3 mol Ca

x 148.26 g Ca3N2

1 mol Ca3N2

Some Things Just Take a Lot of Work!!!

Stoichiometry : Mole Ratios to Stoichiometry : Mole Ratios to Determining Grams of ProductDetermining Grams of ProductLet’s see if you can:Let’s see if you can:

1. Review the conversion of particles or grams to moles

2. Determine mole ratios from a balanced chemical equation

3. Determine the amount of product produced when given the amount of reactants

NaN3 Na + N2

Decomposition 2 NaN3 2 Na + 3 N2

65.02 g 22.99 g28.02 g

Mass-Mole-MassMass-Mole-Mass

= 61.1 g N2

94.5 g NaN3x 1 mol NaN3

65.02 g NaN3

x 3 mol N2

2 mol NaN3

x 28.02 g N2

1 mol N2

Don’t you just love these types of problems???