Mole Calculations,Popcorn lab and % of water lab

With the begging of the year starting, we started talking about the mole. In a previous post about the mole we talked about the history of it and how it used. In this post it is a large post about the mole and ways we have used it in class.
MOLE CALCULATIONS 
We first started off with learning about mole calculations and how we use them in the real world. A mole is commonly abbreviated mol (short huh?) The mole is 6.02 X 10^23. The mole is the amount of something, like how a baker uses dozen, Chemists uses the mole to count something.
 So here is an example of how to use a mole correctly. This example is converting moles to particles and particles to moles.
Your equation looks like this # of moles X 6.02 X 10^23 representative particles      
                                                                                   1 mole = number of representative particles

Here is a real world problem : 2.5 mol Zn X 6.02 x 10^23 atoms  = 1.505 X 10^24  

                                                                                1 mol

What I did was I reduced the mol Zn and the bottom mol then multiplied across and divided by one to get 1.505 X 10^24 

HERE ARE SOME WORK SHEETS I DID TO SHOW THAT I KNOW HOW TO USE MOLES:) THESE ARE PAPERS FROM THE BOOK AND THE COVER ALL THE MOLE CALCULATIONS.

MASS AND THE MOLE
This is the also an easy mole equation. Molar mass is the mass in grams of one mole of any pure substance.
  This is the equation for molar mass # of moles X # of grams
                                                                                 1 mole       = mass

Here is an example 3.00 mol Mn X 54.9 g Mn
                                                          1 mol Mn  = 1.65 g Mn
Again you follow the simple math and reduce and balance the equation.

MOLES OF COMPOUNDS
Moles of compounds are a little harder than the others what you do is find a ratio so the formula CCl2F2 has a ratio of 1:2:2 because the formula has 1 carbon, and 2 chlorine and 2 fluorine.
 Here is an example: 1 mol C atoms         2 mol Cl atoms        2 mold F atoms        
                                 1 mold CCL2F2      1 mol CCl2F2           1 mol CCl2F2
moles CCl2F2 X moles F atoms   = moles F atoms
                             1 mole CCl2F2
*fluorine atoms = 5.50*

5.50 mole CCl2F2 X 2 mol Fatoms  = 11.0 mol Fatoms
                                    1 mol CCl2F2
And so 11.0 mol F atoms are in 5.50 moles of CCl2F2

EMPIRICAL AND MOLECULAR FORMULAS
First off we have percent composition all this is, is to find the percent by mass. This is so easy all you do is mass of element
        mass of compound x 100 = percent by mass

Empirical formula 
Empirical formula for a compound is the formula with the smallest whole number mole ratio of the elements. *the empirical formula may or may nor be the same as the actual molecular formula*
The empirical formula for hydrogen peroxide is HO the molecular formula is H2O2. Both have a 1:1 ratio.
An example is: 48.64 g C X 1 mol C
                                             12.01 g C  = 4.050 mol C
Same as before you reduce and divide. 

THIS IS A WORKSHEET COVERING EMPIRICAL AND MOLECULAR FORMULAS.

With this prezi below it will show how to use the hydrate formula in a popcorn lab and % of water lab: