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Stoichiometry
Learning Objectives
The study of the
amount of
substances
consumed and
produced in a
chemical reaction.
Stoichiometry
It’s All About Proportions
When making muffins, you use
proportions to determine how much of
each ingredient is needed.
8 C flour
2 C sugar
Yields…
12 muffins
4 C flour
1 C sugar
Yields…
6 muffins
Balanced equation revision
Matter can not be created nor
destroyed.
The number of atoms of each element on
both sides of the equation must be equal.
Change the coefficients of the reactants
and products to balance.
Balanced Equations Show Proportions
2H2 + O2  2H2O
2 mol H2 reacts with 1 mol O2 to produce 2
mol H2O.
If you double the reactants…
– 4H2 + 2O2  ?? H2O
If you triple the products…
– ? H2 + ? O2  6H2O
The mole ratio is the key…
The coefficients of a balanced equation
give us the mole ratio.
The mole ratio gives us the correct
proportions.
Using the Mole Ratio:
Mole-Mole Stoichiometry
N2 + 3H2  2 NH3
How many moles of hydrogen are needed
to prepare 312 moles of ammonia?
312 moles NH3
2 moles NH3 Mole Ratio
from Balanced
Equation!
3 moles H2
= 468 mol H2
Using the Mole Ratio
Fe2O3 + 2 Al  2 Fe + Al2O3
–3.30 mole Fe2O3 reacts with
how many moles of Al?
–3.30 moles Fe2O3 produces
how many moles of Fe?
–3.30 moles Fe2O3 produces
how many moles Al2O3?
6.60 mol
6.60 mol
3.30 mol

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Lesson #4-Stoichiometry.ppt

  • 3. The study of the amount of substances consumed and produced in a chemical reaction. Stoichiometry
  • 4. It’s All About Proportions When making muffins, you use proportions to determine how much of each ingredient is needed. 8 C flour 2 C sugar Yields… 12 muffins 4 C flour 1 C sugar Yields… 6 muffins
  • 5. Balanced equation revision Matter can not be created nor destroyed. The number of atoms of each element on both sides of the equation must be equal. Change the coefficients of the reactants and products to balance.
  • 6. Balanced Equations Show Proportions 2H2 + O2  2H2O 2 mol H2 reacts with 1 mol O2 to produce 2 mol H2O. If you double the reactants… – 4H2 + 2O2  ?? H2O If you triple the products… – ? H2 + ? O2  6H2O
  • 7. The mole ratio is the key… The coefficients of a balanced equation give us the mole ratio. The mole ratio gives us the correct proportions.
  • 8. Using the Mole Ratio: Mole-Mole Stoichiometry N2 + 3H2  2 NH3 How many moles of hydrogen are needed to prepare 312 moles of ammonia? 312 moles NH3 2 moles NH3 Mole Ratio from Balanced Equation! 3 moles H2 = 468 mol H2
  • 9. Using the Mole Ratio Fe2O3 + 2 Al  2 Fe + Al2O3 –3.30 mole Fe2O3 reacts with how many moles of Al? –3.30 moles Fe2O3 produces how many moles of Fe? –3.30 moles Fe2O3 produces how many moles Al2O3? 6.60 mol 6.60 mol 3.30 mol