1. CH 3: Stoichiometry
Moles

2. Mole Defined
Mole = number equal to the # of carbon atoms in exactly 12 grams of pure C-12.
Mole = x 1023
Called Avogadro’s number
One mole of protons = 1g
One mole of neutrons = 1g
One mole of an element = atomic mass in grams

3. Molar Mass and related terms
Molar mass – mass in grams of one mole of a substance
– molecular weight, mass of 1 molecule in amu
Formula weight, mass of 1 formula unit for an ionic compound in amu
Calculate by summing the masses of the component atoms, units:
molar mass – grams or grams/mole
molecular wt & formula wt - amu

4. Moles, mass and # particles
Molar mass links the mass of a substance to the number of particles present
1 mole Mg = 24.31g = x 1023 Mg atoms

5. Molar Mass Related Calculations:
Molar mass of a substance.
Moles present in a given mass of substance.
Mass of a given number of moles of a substance.
Number of particles in a given mass or a given number of moles of a substance.

6. What is the molar mass of glucose. The formula for glucose is C6H12O6.
What is the mass of moles of glucose?

7. How many glucose molecules are present in 0.023 moles of the compound?
How many moles of glucose are present in 3.5 x 10-3 grams of the substance?

8. Mass Percent
Compounds are typically described by either their chemical formula or their percent by mass of the component elements.
Mass % X = n (molar mass X) x 100%
molar mass of compound

9. Mass Percent Calculations
Calculate the mass percent of each element in C6H12O6
Assume one mole of the substance.

10. Empirical and Molecular Formulas
Molecular formula – ratio of atoms in a molecule
Empirical formula – simplest ratio of elements in a molecule
Glucose:
Molecular formula: C6H12O6
Empirical Formula:
Molecular formula = n (empirical formula)

11. Mass %  Empirical Formula
Given mass percent data:
“Calculate” mass in grams of each element in 100 g of compound.
Convert each mass into moles of the element.
Divide each molar answer by the smallest of the values.
If the numbers obtained in step 3 are not whole numbers, multiply all by an integer so the results are whole numbers
Whole numbers obtained in step ¾ are the subscripts in the empirical formula.

12. Empirical Formula  Molecular Formula
Molar mass needed
Calculate mass of one mole of the empirical formula.
Molar Mass = integer (n)
empirical formula weight
(n)(empirical formula) = molecular formula

13. Caffeine Molar mass = 194 g/mol 49.49 % C 5.19 % H 28.85 % N 16.48 % O
What is the empirical and molecular formula of caffeine?

14. Acetaminophen (Tylenol)
Molar mass = 151 g/mol
63.56 % C
6.00 % H
9.27 % N
21.17 % O
What is the empirical and molecular formula of acetaminophen?

15. CH 3: #86
Urea: Molar Mass 60 g/mol (I looked this up – not in question)
1.121 g N
0.161 g H
0.480 g C
0.640 g O
What is the empirical and molecular formula of urea?

16. 3.7/3.8 Chemical Reactions Writing chemical reactions
Write the correct chemical formula for each reactant and product.
Use a subscript after each formula to indicate the state of each substance
(s) – solid
(l) – liquid
(g) – gas
(aq) – aqueous (dissolved in water)

17. Chemical equations must obey the law of conservation of matter – balancing does this.
Balance the equation by adding coefficients in front of reactants and products as needed
DO NOT CHANGE THE FORMULAS FOR THE COMPOUNDS

18. One of my favorite chemical reactions:
Mg(s) HCl(aq)  MgCl2 (aq) + H2 (g)
As written the reaction does not obey the law of conservation of matter – reaction needs to be balanced

19. Mg(s) + 2 HCl(aq)  MgCl2 (aq) + H2 (g)
Now the reaction is balanced!

20. Balance the Reactions N2 (g) + H2 (g)  NH3 (g)
Na(s) Cl2 (g)  NaCl(s)
Pb(NO3)2(aq) + NaCl(aq)  PbCl2(s) + NaNO3(aq)

21. Meaning of the Balanced Reaction
Atomic level
Molar level
Stoichiometry - relationship between moles, the balanced reaction and mass
Page 10? outlines the needed steps

22. 2 Na Cl2  NaCl
2 mol Na mol Cl2  2 mol NaCl

23. Cookie example! 2 eggs + 1 bag chips  50 cookies
How many cookies could you make if you had only one egg?
How many cookies could you make if you had 2 bags of chips?

24. Molar Ratios
Balanced reactions lead to molar ratios
N H  2 NH3

25. N2 (g) H2 (g)  NH3 (g)
If 3.5 grams of N2 to react, how many moles and how many grams of NH3 would be made?

26. N2 (g) H2 (g)  NH3 (g)
How many grams of H2 are needed to make 37.8 grams of NH3?

27. 2 LiOH + CO2  Li2CO3 + H2O
How many grams of LiOH are needed to react 750. grams of CO2?
How many grams of Li2CO3 will be made if 750. grams of CO2 react?

28. Limiting Reagent
Reactants are not always combined in stoichiometric quantities.
Often one reactant is used up before others.
This reactant is said to be the limiting reagent (or reactant.)
this reactant limits how much product can be made.

29. Limiting Reagent Calculations
When you are given masses for each reactant you must determine which reactant is limiting.
Convert grams of each reactant to moles.
Use the molar ratios to determine which reactant is limiting.
Base the amount of product that can be made on the limiting reagent.

30. Another Approach… Convert grams of each reactant to moles.
Calculate the moles (or grams) of a product that could be made from each reactant.
Whichever reactant results in the smaller quantity of product is the limiting reagent.
Base the amount of product made on the limiting reagent.

31. N2 (g) H2 (g)  2 NH3 (g)
12.5 grams of nitrogen is combined with 2.30 grams of hydrogen.
Which reactant is in excess and which is limiting?
How many grams of ammonia will be made?

32. Percent Yield
% Yield = actual yield x 100 %
theoretical yield