1. Stoichiometry

2. Look back at Moles

3. Practice
45.3 g of carbon is how many moles?
5.00 liters of carbon dioxide at STP is how many moles?
How many molecules of hydrogen are there in 40.0 L of hydrogen gas at STP?

4. Arithmetic of Equations
Stoichiometry – calculation of quantities in chemical reactions
A chemical reaction tells us a few things: (recipe)
N2 + 3H2 → 2NH3
We can compare number of atoms, number of molecules, moles, mass and volume
Which of these are conserved? (same on both side)

5. How to interpret a reaction
Given the reaction: N2 + 3H2 → 2NH3
We can easily get number of each atom, each molecule, and volume of each gas.
The tricky one is the mass of the reactants and products.
By the law of conservation of mass, we know that each side of an equation needs to have an equal mass, but we need to find the mass of each side to show that they are equal.

6. Mass of Reactants and Products
N2 + 3H2 → 2NH3
Reactants: 1 mol N2 = 28 g
3 mol H2 = 3 X 2 g = 6 g
Total = 34 g
Products: 2 mol NH3 = 2 X 17 g = 34 g
Both sides are 34 g, which is a good sign the calculation was done right

7. Now try this out Given the reaction 2Mg + O2 → 2MgO
Find the number of moles and mass of reactants and products
Next do the same for this unbalanced reaction
That means YOU need to balance it!
H2SO4 + NaOH → Na2SO4 + H2O

8. Mole Ratios
Mole ratio: conversion factor derived from the coefficients of a balanced chemical reactions in terms of moles
N2 + 3H2 → 2NH3
This equation gives us three mole ratios
Nitrogen to hydrogen, nitrogen to ammonia, and hydrogen to ammonia or
1 mol N2 1 mol N2 3 mol H2
3 mol H2 2 mol NH3 2 mol NH3

9. Get all mole ratios for this reaction
2Mg + O2 → 2MgO

10. Using mole ratios
We can use mole ratios to convert from moles of one substance to moles of a different one.
If we have 3.50 mol N2 and excess H2 in the reaction: N2 + 3H2 → 2NH3
How many moles of NH3 will be formed?
What if we had 3.50 mol H2 and excess N2?

11. Now you try these Given the equation: 2Mg + O2 → 2MgO
How many moles of oxygen will react with 5.00 mol Mg?
How many moles of Mg and O2 reacted if we ended up with 3.70 mol MgO?

12. Mass-Mass Calculations
With our new tool, the mole ratio, we can calculate the mass of any other substance in a reaction if we are given the mass of one.
It will take THREE steps:
Convert given grams to given moles (molar mass)
Convert given moles to wanted moles(Mole Ratio)
Convert wanted moles to wanted grams (molar mass)

13. Example Given the reaction: N2 + 3H2 → 2NH3
How many grams of ammonia will be formed if 50 g of nitrogen react?
Given the same amount of nitrogen, how much hydrogen reacted?

14. Your turn Given the reaction: 2Mg + O2 → 2MgO
How many grams of Mg reacted if 75.3 g MgO were formed?
How many grams of O2 reacted if 75.3 g MgO were formed?

15. Other Stoichiometric Calculations
Instead of doing a mass-mole conversion, we can do the two other conversions from Ch 10.
Instead of giving a mass, we could get a volume or number of particles
Also, instead of calculating mass at the end, we can get volume or number of particles
Look at Figure 12.8 on page 363

16. Modified Steps Convert given grams, liters or particles to given moles
Convert given moles to wanted moles(Mole Ratio)
Convert wanted moles to wanted grams, liters or particles

17. Examples Given the reaction: 2Mg + O2 → 2MgO
How many atoms of Mg reacted if 75.3 g MgO were formed?
Given the reaction: N2 + 3H2 → 2NH3
How many liters of ammonia will be formed if 3.50 L of nitrogen react?

18. Limiting Reagent and Percent Yield
Limiting reagent is the more practical application of stoichiometry that can be used in the laboratory
Percent yield compares the amount of product formed in an experiment compared to what the maximum would be

19. Limiting and Excess Reactants
Limiting Reactant- reactant that is used up in a reaction, which limits that amount of product
Excess Reactant- reactant that remains after the reaction has stopped

20. Determining a limiting reactant
For these problems, we will be given the starting amounts of two reactants
We need to use both and use each to get the amount of one of the products formed

21. N2 + 3H2 → 2NH3
If 5.3 moles of nitrogen gas react with 5.3 moles of hydrogen gas, how many moles of ammonia is produced? Which reactant is limiting?

22. N2 + 3H2 → 2NH3
If 30.0 g of nitrogen gas react with 30.0 g of hydrogen gas, how many grams of ammonia is produced? Which reactant is limiting?

23. Your turn
2Mg + O2 → 2MgO
Which reactant is limiting if 20.0 g of magnesium react with 20.0 g of oxygen? How much product will be formed?

24. Yield Definitions
Theoretical Yield- maximum amount of product that can be formed by the given amount of reactants
Actual Yield- amount of product actually formed when an experiment is performed
Percent Yield- ratio of the actual yield to the theoretical yield expressed as a percent

25. Percent Yield Tells us how efficient an experiment was
Can be as a result of an error made or may just be a result of the procedure of the experiment
Actual yield is determined in the laboratory or given in the problem
Theoretical yield is determined with a calculation

26. Example
N2 + 3H2 → 2NH3
If 10.0 g nitrogen react with 3.00 g hydrogen and 10.0 g ammonia is formed, what is the percent yield?

27. Practice
2Mg + O2 → 2MgO
If 15.0 g magnesium react with 10.0 g oxygen to form 16.5 g magnesium oxide, what is the percent yield?