The document discusses limiting reactants and how to calculate percent yield in chemical reactions. It defines limiting and excess reactants, and explains that the limiting reactant determines the amount of product that can be formed. It provides two methods for identifying the limiting reactant and calculating theoretical yield. It also defines percent yield as a measure of the efficiency of a reaction, comparing the actual and theoretical yields.

1. &
Percentage
yield

2. Lesson Objectives
By the end of the lesson learners should be able to:
• To define the concept of limiting reactants
• To learn to recognize the limiting reactant in a reaction
• To use the limiting reactant to do stoichiometric calculations
• To calculate percent yield

5. Limiting Reactants
• Available Ingredients
– 4 slices of bread
– 1 jar of peanut butter
– 1/2 jar of jelly
• Limiting Reactant
– bread
• Excess Reactants
– peanut butter and jelly
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

6. Limiting Reactants
• Limiting Reactant
– used up in a reaction
– determines the amount of product
• Excess Reactant
– added to ensure that the other reactant is
completely used up
– cheaper & easier to recycle
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

7. Stoichiometry
Like many problems in chemistry, there are multiple ways of solving
these problems.
You can save yourself some work, by first identifying what you need
to solve for and then choosing the appropriate method.
Don’t worry if you choose the wrong method, you’ll get to the correct
answer, it will just take you a few more steps.

8. Limiting Reactants – Method
1. Write a balanced equation.
2. For each reactant, calculate the
amount of product formed.
3. Smaller answer indicates:
– limiting reactant
– amount of product
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

9. Limiting Reactants – Method 2
• Begin by writing a correctly balanced chemical equation
• Write down all quantitative values under equation (include
units)
• Convert ALL reactants to units of moles
• Divide by the coefficient in front of each reactant
• The smallest value is the limiting reactant!

10. Limiting Reactants
aluminum + chlorine gas  aluminum chloride
Al(s) + Cl2(g)  AlCl3
2 Al(s) + 3 Cl2(g)  2 AlCl3
100 g 100 g ? g
A. 200 g B. 125 g C. 667 g D. 494 g

11. Limiting Reactants
aluminum + chlorine gas  aluminum chloride
2 Al(s) + 3 Cl2(g)  2 AlCl3
100 g 100 g x g
Al AlCl3
x g AlCl3 = 100 g Al
27 g Al
= 494 g AlCl3
1 mol Al 2 mol AlCl3
2 mol Al
133.5 g AlCl3
1 mol AlCl3
How much product would be made if we begin with 100 g of aluminum?
Cl2 AlCl3
x g AlCl3 = 100 g Cl2
71 g Cl2
= 125 g AlCl3
1 mol Cl2 2 mol AlCl3
3 mol Cl2
133.5 g AlCl3
1 mol AlCl3
How much product would be made if we begin with 100 g of chlorine gas?

12. 12
Limiting/Excess/ Reactant and Theoretical Yield Problems :
Potassium superoxide, KO2, is used in rebreathing gas masks to generate oxygen.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
a. How many moles of O2 can be produced from 0.15 mol KO2 and 0.10 mol H2O?
b. Determine the limiting reactant.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
First copy down the
the BALANCED
equation!
Now place
numerical the
information below
the compounds.

13. 13
Limiting/Excess/ Reactant and Theoretical Yield Problems :
Potassium superoxide, KO2, is used in rebreathing gas masks to generate oxygen.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
a. How many moles of O2 can be produced from 0.15 mol KO2 and 0.10 mol H2O?
b. Determine the limiting reactant.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
0.15 mol 0.10 mol ? moles
Two starting
amounts?
Where do we
start?
Hide
one

14. 14
Limiting/Excess/ Reactant and Theoretical Yield Problems :
Potassium superoxide, KO2, is used in rebreathing gas masks to generate oxygen.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
a. How many moles of O2 can be produced from 0.15 mol KO2 and 0.10 mol H2O?
b. Determine the limiting reactant.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
0.15 mol 0.10 mol ? moles
Hide
Based on:
KO2
0.15 mol KO2
4 mol KO2
2 mol H2O
= 0.075 mol H2O are needed
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
0.15 mol 0.10 mol
We calculated that we need 0.075 moles of water, but we have 0.10
moles, thus water is in excess, thus our limiting reactant is KO2

15. 15
Potassium superoxide, KO2, is used in rebreathing gas masks to generate oxygen.
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
a. How many moles of O2 can be produced from 0.15 mol KO2 and 0.10 mol H2O?
b. Determine the limiting reactant. KO2(s)
c. Determine the moles of oxygen produced
4KO2(s) + 2H2O(l)  4KOH(s) + 3O2(g)
0.15 mol excess ? moles
Based on:
KO2 = mol O2
0.15 mol KO2
2
2
KO
4mol
O
mol
3
0.1125
Limiting/Excess/ Reactant and Theoretical Yield Problems :

16. Percent Yield
• The percent yield is a measure of the efficiency of a reaction carried
out in the laboratory.
• A batting average is actually a percent yield.
12.3

17. Percent Yield
– The theoretical yield is the maximum amount of product that could be formed
from given amounts of reactants.
– The actual yield mass that is always given in a question or statement
12.3

18. 12.9
Calculating Theoretical Yield is just Mass:Mass!!!!!!!!

19. 12.9

20. 12.9

22. Concept Map 12
• Solve the Concept Map with the help of an interactive guided tutorial.

23. Conclusion
N₂+ 3H2=2NH3
You are given 28g of N, and 10g of H Mass from periodic table: N=14 H=1
A) Determine the limiting reagent
B) Determine the mass of NH3 ,that will be produced
C) A student tries this reaction in a lab and only manages to produce
15g of NH3. What is the percentage yield?

24. .
END OF SHOW