Limiting Reactant II and Percent Yield A.K.A. Stoichiometry.
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Transcript of Limiting Reactant II and Percent Yield A.K.A. Stoichiometry.
The reactant that limits the amount of product produced
Limiting reactant is consumed fully in a chemical reaction
Excess reactant remains in a chemical reaction
What is a Limiting Reactant?
Remember The Sundae Example…
The chocolate syrup was consumed fully.The ice cream and cherries are left over.
Calculate using mass-mass conversion; find which reactant produces the least amount of product
Or use mole-mole conversion to determine which reactant is consumed first
How do we determine which reactant is the limiting
reactant?
What is the limiting reactant when 10.0 g of SiO2 react with 5.0 g of HF?
Create a conversion pathway using mass-mass conversion
SiO2(s) + 4 HF(l) → SiF4(g) + 2 H2O(l)
How efficient is a chemical reaction?
Does the reaction go to completion?
How much product is produced?
How can we predict the amount of product produced?
How Does Sundae Production and Percent Yield Relate?
• If you made only 25 sundaes but You really needed 40, what was
your production yield?• Actual yield = 25 sundaes• Production (theoretical) yield = 40
sundaes• Percent yield = 25 x 100 % =
63% 40
5.00 g of Cu is mixed with an excess of AgNO3.
The reaction produces 15.2 g of Ag
What is the percent yield for this reaction?
We want to know how much product is produced?
Create your conversion pathway using mass-mass conversion
Cu + 2 AgNO3 2 Ag + Cu(NO3)2
17.0 g Ag is our theoretical yield; need to use it to calculate percent yield
Percent Yield
Percent Yield = Actual yield x 100
Theoretical yield
Actual/Theoretical
Percent Percent Yield
Percent Yield = 15.2 g Ag x 100 = 89.4 %
17.0 g Ag
What is the percent yield when 24.8 g of CaCO3 decomposes to give 13.1 g CaO? CaCO3CaO + CO2
Plan your conversion pathwayUtilize mass-mass conversion
One more example
CaCO3CaO + CO2
The theoretical yield is 13.9 g of CaO; what is our percent yield? The reaction made 13.1 g CaO
Actual/Theoretical
Percent Percent Yield
= 13.1 g x 100 = 94.2 %
13.9 g