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## PowerPoint Slideshow about ' the Mole !' - aristotle-olson

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

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

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

It’s time to learn about . . .

the Mole !

What's The Difference Between Roast Beef And Pea Soup?

Anyone Can Roast Beef.

- Review the conversion of particles or grams to moles
- Determine mole ratios from a balanced chemical equation
- Determine the amount of product produced when given the amount of reactants

Review the Molar Mass of Compounds Product

- 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

20

Ca40.08

17Cl 35.45

Practice Product

- Calculate the Molar Mass of calcium phosphate
- Formula =
- Masses elements:
- Molar Mass =
310.18 g

Ca3(PO4)2

My new book on GOLF will give the reader valuable playing tips and insider information I've gained through my years of lessons, struggles and experiments. Here are just a few of the chapter titles:

Chapter 5 - When to Give the Ranger the Middle Digit.

Chapter 14 – The Best Time to Let a Foursome Play through Your Twosome.

Calculations tips and insider information I've gained through my years of lessons, struggles and experiments.

molar mass Avogadro’s number Grams Moles Particles

Everything must go through Moles!!!

Flowchart tips and insider information I've gained through my years of lessons, struggles and experiments.

Atoms or Molecules

Divide by 6.02 X 1023

Multiply by

6.02 X 1023

Multiply by atomic/molar mass from periodic table

Moles

Divide by atomic/molar mass from periodic table

Mass (grams)

Chocolate Chip Cookies!! tips and insider information I've gained through my years of lessons, struggles and experiments.

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 chips

Makes 3 dozen

How 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!?!? tips and insider information I've gained through my years of lessons, struggles and experiments.

- Just like chocolate chip cookies have recipes, chemists have recipes as well
- Instead of calling them recipes, we call them chemical equations
- Furthermore, instead of using cups and teaspoons, we use moles
- Lastly, instead of eggs, butter, sugar, etc. we use chemical compounds as ingredients

Chemistry Recipes tips and insider information I've gained through my years of lessons, struggles and experiments.

- 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!! tips and insider information I've gained through my years of lessons, struggles and experiments.

Practice tips and insider information I've gained through my years of lessons, struggles and experiments.

- 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 Ratios tips and insider information I've gained through my years of lessons, struggles and experiments.

- 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

x 1 mol Cl tips and insider information I've gained through my years of lessons, struggles and experiments.2

2 mol Ag

Question Answer2 Ag+ Cl2 2 AgCl

# moles of Cl2 =

5 mol Ag

= 2.5 mol Cl2

2 mol AgCl tips and insider information I've gained through my years of lessons, struggles and experiments.

1 mol Cl2

Mole-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

# moles of AgCl =

2.6 mol Cl2 x

= 5.2 mol AgCl

Mass-Mole tips and insider information I've gained through my years of lessons, struggles and experiments.

- 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

x 2 mol C tips and insider information I've gained through my years of lessons, struggles and experiments.2H6

6 mol H2O

x 1 mol H2O

18.02 g H2O

Mass-Mole- 2 C2H6 + 7 O2 4 CO2 + 6 H20

10.0 g H2O

= 0.185 mol C2H6

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Stoichiometry Continued: tips and insider information I've gained through my years of lessons, struggles and experiments.

- Review the conversion of particles or grams to moles
- Determine mole ratios from a balanced chemical equation
- Determine the amount of product produced when given the amount of reactants

Mass-Mass Conversions Product

- 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 Conversion Product

- 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-Mass Product

- 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

x 1 mol Ca Product3N2

x 148.26 g Ca3N2

3 mol Ca

1 mol Ca3N2

x 1 mol Ca

40.08 g Ca

Mass-Mole-Mass- 3 Ca + N2 Ca3N2

2.00 g Ca

= 2.47 g Ca3N2

- Review the conversion of particles or grams to moles
- Determine mole ratios from a balanced chemical equation
- Determine the amount of product produced when given the amount of reactants

x 3 mol N Product2

x 28.02 g N2

2 mol NaN3

1 mol N2

x 1 mol NaN3

65.02 g NaN3

Mass-Mole-Mass- NaN3 Na + N2
- Decomposition
- 2 NaN3 2 Na + 3 N2
- 65.02 g 22.99 g 28.02 g

94.5 g NaN3

= 61.1 g N2

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