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TRANSCRIPT
Stoichiometry – Ch. 9
Stoichiometry
Stoichiometry problems consist of predicting the
amount of grams of product that will form from a
reaction if you know how many grams of
reactant you have, or predicting the number of
grams of reactant that will be needed to produce
a certain amount of product.
Proportional Relationships
I have 5 eggs. How many cookies can I make?
3/4 c. brown sugar
1 tsp vanilla extract
2 eggs
2 c. chocolate chips
Makes 5 dozen cookies.
2 1/4 c. flour
1 tsp. baking soda
1 tsp. salt
1 c. butter
3/4 c. sugar
5 eggs 5 doz.
2 eggs= 12.5 dozen cookies
Ratio of eggs to cookies
Proportional Relationships
Stoichiometry
• mass relationships between substances in a chemical reaction
• based on the mole ratio
Mole Ratio
• indicated by coefficients in a balanced equation
2 Mg + O2 2 MgO
Mole Ratio
• A mole ratio is a ratio between the numbers of moles of any two substances in a balanced equation. Refer to coefficients in the balanced equation to determine the mole ratio.
Stoichiometry Steps
1. Write a balanced equation.
2. Identify known & unknown.
3. Line up conversion factors.
• Mole ratio - moles moles
• Molar mass - moles grams
• Molarity - moles liters soln
• Molar volume - moles liters gas
Core step in all stoichiometry problems!!
• Mole ratio - moles moles
4. Check answer.
C. Conversion Factors
of the Mole
Molar Mass(g/mol)
6.02 1023
particles/mol
MASS
IN
GRAMS
MOLES
NUMBER
OF
PARTICLES
LITERS
OF
SOLUTION
Molar Volume(22.4 L/mol)
LITERS
OF GAS
AT STP
Molarity (mol/L)
Grams-Mole Problems
How many grams of Copper are
needed to produce 5 moles of
copper oxide?
2Cu + O2 2CuO
5 mol CuO
2 mol CuO
2 mol Cu
1 mol Cu
63.55 g Cu
1 mol of a gas=22.4 Lat STP
C. Molar Volume at STP
Standard Temperature & Pressure0°C and 1 atm
Limiting and Excess Reactants
Why do reactions stop?
• Reactions proceed until one of the reactants is used up and one is left in excess.
• The limiting reactant limits the extent of the reaction and, thereby, determines the amount of product formed.
• The excess reactants are all the leftover unused reactants.
Calculating the Product when a Reactant
is Limiting
• S8 + 4Cl2→ 4S2Cl2
• Given the following equation and reactant amounts of 200.0g S8 and 100.0g Cl2
• Determine which is the limiting reactant
• Determine which reactant is in excess and how much excess you have
• Determine how much product would be made
Percent Yield
• The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant.
• ***This comes from a stoichiometry calculation of the limiting reactant
• The actual yield is the amount of product actually produced when the chemical reaction is carried out in an experiment.
• The percent yield of a product is the ratio of the actual yield expressed as a percent.
• This tells you how close you were!!!!