1. Conversion factors from chemical formula
Chemical formula contains information regarding the relationship between atoms(moles of atoms) or between molecules(moles of molecules)
Example: The formula of CCl2F2 tells us that there is 2 mole of Cl for every one mole of CCl2F2

2. Practice Problem
Calculate the number of moles of Chlorine in 38.5 mole of CCl2F2 ?

3. Practice Problem
Calculate the mass in grams of Cl contained in 25g of CCl2F2 ?

4. Obtaining an empirical formula from Experimental data
Steps
Write down the given masses of each element in the compound. If you are given mass percentage composition, assume a 100g sample and calculate the masses of each element from the given percentage

5. Steps
2.Convert each mass in to moles by using appropriate molar mass for each element as a conversion factor
3.Write down the pseudo formula for the compound using the number of moles of each element(from step 2) as a subscript

6. Steps
4. Divide all the subscripts in the formula by the smaller subscript
5. If the subscripts are not whole numbers, multiply all the subscripts with a whole number to get whole number subscript

7. Practice
A compound containing N and O is decomposed in the laboratory and produces24.5g N and 70.0g of Calculate the empirical formula of the compound

8. Practice
A laboratory analysis of Aspirin determined the following mass percent composition
C 60.0%
H 4.48%
O 35.52%
Find the empirical formula

9. Practice Problem
A Sample of Compound is decomposed in the laboratory and produces 165g of C, 27.8g of H and 220.2g of O calculate the empirical formula of the compound?

10. Practice Problem
Ibuprofen has the following mass percent composition
C – 75.69%
H – 8.80%
O – 15.51%
What is the empirical formula of Ibuprofen?

11. Calculating molecular formula from Empirical formula
Molecular formula of a compound = Empirical formula × n
Where n = 1,2,3 ….

12. Calculating the molecular formula
n can be obtained by -
Molar mass ÷ Empirical formula molar mass
Calculate the Molecular formula for fructose? Given that its empirical formula is CH2O and its molar mass is 180.2g/mol

13. Problem
A compound has the empirical formula CH and a molar mass of 78.11g/ mol. What is its molecular formula?

14. Determine the molecular formula
A compound with a percentage composition shown next has a molar mass of 60.1g/mol. Determine its molecular formula?
C – 39.97%
H – 13.41%
N – 46.62%

15. Combustion Analysis
Combustion analysis is another way to determine the empirical formula of an unknown compound.
Especially used to find the empirical formula of compounds containing C and H
When the sample is burned, all the C in the sample is converted to CO2 and all the H is converted to H2O
The CO2 and H2O produced are then weighed

16. Combustion Analysis
With the masses, we can use the numerical relationships between moles inherent in the formula for CO2 and H2O to determine the masses of C and H in the original sample
1mol of CO2 :1 mol of C
1 mol of H2O: 2mol of H
The amount of Other elements can be determined by subtracting the sum of the masses of C and H from the original mass of the sample.

18. Topics Remaining
Obtaining an empirical formula from combustion analysis
How to write balanced chemical equations
Balancing chemical equation containing ionic compounds with polyatomic ions