1. A MOLE IS JUST A NUMBER 6.02 X 10 23 Mole

2. Mole Map

3. Molar Density Density is Mass/Volume Molar density = Mass of one mole Volume of one mole = Molar Mass 22.4L Argon= 39.95 g = 1.78g/l 22.4 l

4. Gas Density http://www.youtube.com/watch?v=w7G4o2alLww& feature=related Mole Density and Molar Mass of a Gas Experiment http://www.youtube.com/watch?v=D0CzquuOrxM

5. Percent Composition When the grams are not given, use the molar mass Molar mass of each element X 100 Molar mass of compound

6. 1.) H—2(1.01)=2.02 S—1(32.06)=32.06 O—4(16.00)=64.00 2). Get total mass 2.02 + 32.06 + 64.00= 98.08 (this is bottom #) 3). H 2.02/98.08 X 100= 2.06% S 32.06/98.08 X 100= 32.65% O 64.00/98.08 X 100= 65.25% Example: H2SO4

7. Percent Comp by molar mass http://www.youtube.com/watch?v=JmDd_nJaP3o& feature=related

8. When mass is given, use mass as part over whole. Grams element/grams compound X 100 Example: if 64 g of Mg is combined with 32 g oxygen, what is the percent composition? 64 X 100= 66.7 % 64 + 32 32 X 100= 33.3% 64 + 32

9. % Comp by mass http://www.youtube.com/watch?v=DB2YCK2p56o

10. Empirical Formula Molecular Formula Consists of the symbols and the subscripts showing the smallest whole number ratio of atoms. Subscripts are reduced. May not be the actual formula. Examples: CO, CO 3, N 3 P The actual formula. You can reduce the subscripts. Examples: C 2 O 2, C 2 O 6, N 9 P 3 Empirical vs. Molecular Formulas

11. How do you calculate empirical formulas? 1. Change the % sign into a g. (g for grams) 2. Divide mass by molecular weight(convert grams into moles) 3. Divide by the smallest. 4. If necessary, multiply to make whole numbers. 5. These are your SUBSCRIPTS.

12. Example of empirical formulas. Find the empirical formula of a compound found to contain 63.52% Fe and 36.48% S. 63.52 g Fe= 36.48 g S = 55.85 g 32.07 g Fe 1 S 1

13. Example #2 Find the empirical formula of a compound found to contain 26.56% K, 35.41% Cr, and the remainder O. 26.56 g K 35.41 g Cr 38.03 g O

14. Empirical to Molecular X(empirical formula) = molecular formula X = molecular weight of molecular formula molecular weight of empirical formula Example: The empirical formula of a compound of P and O was found to be P2O5. The molar mass of the compound is 283.89 g/mol. What is the molecular formula? 1. Find the molecular weight of the empirical formula. 2. Divide molecular/empirical. 3. Multiply x by empirical formula.

15. Example http://www.youtube.com/watch?v=LPN-3d0FOMU Determine the molecular formula for a compound that is 40.0% C, 6.6% H, and 53.4 % O. The molar mass is 120 g. Determine the molecular formula of a compound with an empirical formula of CH and a formula mass of 78.110 amu.

16. Practice 1. Find the percent composition of Mg(OH) 2. 2. Find the percent composition of a compound that contains 1.94g C, 0.48g H, and 2.58g S in a 5.0g sample. 3.Determine the empirical formula of a compound containing 1.723gC, 0.289gH, and 0.459gO. 4. Find the molecular formula of a compound that contains 30.45gN and 69.55gO. The molar mass is 92.02g/mol.