1. The Mole Continued

2.  The mole is also defined as the number of protons in 1.00000 g of protons.

3.  The number of molecules in 12.00 grams of Carbon-12  6.022 x 10 23 molecules  Why?

4.  If you have 1.0000 moles of a material that has 50 protons and 60 neutrons, what is the mass of the material?  110 grams

5.  Atomic mass is the average mass of all isotopes of an element.

6.  Particles = Moles * Avogadro’s #

7.  8 moles of Carbon  How many particles?  8 moles * 6.022 x 10 23 molecules/mole  = 4.8176 x 10 24 molecules

8.  100 moles of Water  How many particles?  100 moles * 6.022 x 10 23 molecules/mole = * 6.022 x 10 25 molecules

9.  Moles = Particles / Avogadro’s #

10.  4.8176 x 10 24 particles of H Cl  How many Moles of H Cl  4.8176 x 10 24 particles / (6.022 x 10 23 particles/mole) = 8.0 moles 

11.  100 particles of Uranium?  How many moles of Uranium?  100 particles / (6.022 x 10 23 particles/mole) = 1.661 x 10 -22 moles

12.  Avogadro’s # = Particles / Moles

13.  Duh…  6.022 x 10 23 molecules / mole  It is always that!!!!!!

14.  Mass of an amount of a material is equal to the number of moles of the material times the molar mass of the material.

15.  Mass = Moles * Molar mass

16.  10 moles of Gold  What is the mass?  10 moles * 197.0 grams / mole = 1970.0 grams

17. .5 moles of Sodium  How many grams of Sodium? .5 moles * 22.990 grams / mole = 11.495 grams

18.  How many grams of H Cl are in 2.5 moles of H Cl?  2.5 moles * (1.008 g/mole +35.453 g/mole) = 91.1525 gram

19.  How much Ag 2 S in 3.5 moles?  3.5 moles * ((107.868 g/mole * 2) + 32.066 g/mole) =  867.307 grams Silver Sulfur

20.  323  1-3  324  5-6, 13