1. Avogadro’s and the Mole

2. Moles a mole is the number of carbon atoms in exactly 12g of carbon. a mole is a unit of measurement, just like grams…

3. Grams  Moles the use of molar mass allows the calculation of the mass of a given number of moles (or vice versa)

4. Example What is the mass of 3.25mol of CO 2 ?

5. Example 2 How many moles of N2 are there in 50.0g of N2? #mol =

6. g/mol remember the units of molar mass are g/mol and can be calculated using a given mass divided by a given number of moles

7. Example If 0.140mol of acetylene gas has a mass of 3.64g, what is the molar mass of acetylene? g/mol =

8. Molecules  Moles Avogadro learned that there are 6.02x10 23 molecules in every mole! We can use that now to convert molecules first to moles and then change it up!

9. Example How many moles are there in 6.489 x 10 25 molecules of copper(II)sulfate?

10. Example 2 How many molecules are contained in 45.8 grams of NaOH?