Moles to Volume Conversion

- At a specific pressure and temperature one more of every gas has the same volume
- At 0 degrees celsius and 101.3kPa 1mol = 22.4L
- This Temperature and pressure is called STP
- 22.4L/mol is the molar volume at STP
ex
2.5mol x 22.4L = 56L
               1 mol

11.6L x 1 mol = 0.518mol
             22.4L

11.5mol x 22.4L = 258L
                1 mol

1cc = 1mL
1cm^3 = 1mL

- JanCarlo Paysan

converting from moles to molecules

converting 2 moles of Au

like converting distance:
  
2 mol x 6.02x10^23 
                  1 mol

the mole's cancel each other out so you get  

2      x 6.02x10^23      = 12.01x10^23    = 12.0x10^23
                   1


you multiply and then convert to significant digits.

-Paul Dinh

Molar Mass (Mass of Atoms)

•The mass (in grams) of 1 mole of a substance is called the molar mass.
•It can be determined from the atomic mass on the periodic table
•Measured in g/mol
*Molar Mass* -The atomic weight of an element expressed in grams is the mass of one mole of the element. 

Molar Mass of Compounds

•To determine the molar mass of a compound add the mass of all the atoms together.

-Paulo Santillan

Avrogado's Number (How we count atoms)

•Atoms & molecules are extremely small
•Macroscopic objects contain too many to count or weigh individually
•Amedeo Avrogado proposed that the # of atoms 12.00000g of Carbon be equal to a constant (This is equal to 1 mol of Carbon)
•This value is now called Avrogado's Number & froms the basis of all quantitative chemistry.
• Avrogado's Number → 1mol = 6.02x10^23
•One mole is simply a multiple of things, such as:
∟1 pair = 2
∟1 dozen = 12
∟1 century = 100
∟1 mol = 6.02x10^23
•One mole represents a huge # of particles:
Particle                                                                                                                         
•Atoms                       Element                             6.02x10^23             Fe
                                                                                1 mol                                                             
•Molecules                 Covalent Compound            6.02x10^23             CO2     
                                                                                1 mol                                                                 
•Formula Unit             Ionic Compound                 6.02x10^23              NaCl
                                                                                1 mol
_____________________________________________________________________________
                     

 

                              

-Paulo Santillan  

Chem Lab

in lab we did we had to pick a hydrate and follow the steps
1) we had to weight the empty dry test tube
2) we had to weight the test tube with the hydrate in it
3) we had to light the bunsen burner
4) we had to boil all the water out of the hydrate
5) once we boiled all the water out we had to weigh the hydrate again
6) we calculated how much grams of water was boiled off and how much percent of water the hydrate was
7) we had to calculate our percent error for the percentage of water boiled off

- JanCarlo Paysan