Mole Ratio Lab (November 30, 2011)

In this lab, we were to determine the ratio btwn. the moles of iron → moles of copper. (Copper II Chloride)

1) Weigh both nails and filter paper
2) Collect copper (II) chloride w/ scoopula
3) Place the 8g of weighed copper (II) chloride on top of filter paper
4) Add 8g of copper (II) chloride to beaker, then fill w/ 50mL of water
5) Stir the copper (II) chloride & water
6) Determine the mass of nails
7) Place the 2 nails into the solution for 10 mins
8) Place funnel in clamp
9) Fold filter paper into 4 divisions & put in funnel in the shape of a cone
10) Use the tongs to pick up the 2 nails from the beaker & scoop the copper (II) chloride off the nails into the solution
11)Put stirring rod in center of funnel & pour solution into funnel
12) After all the solution is in the beaker, pick the filter paper w/ the tongs
13) Place filter paper in oven for about 30 mins
14) Take paper & weigh on scale
15) Clean up everything

-Paulo Santillan

Molar Volume Lab (November 22, 2011)

In this lab we followed the steps to determine the molar volume of a gas (Butane = C4H10)

1) Fill the sink about 3/4 w/ water
2) Weigh your butane lighter on the scale
3) Place the graduated cylinder in water (base facing upwards)
4) Fill the whole graduated cylinder w/ water
5) Hold the butane lighter under the cylinder (water)
6) Click the butane lighter to release butane in cylinder
7) Make a measurement of the amount of butane filling the test tube
8) Dry the butane lighter in oven for about 10-15 min
9) Weigh the butane lighter again
10) Make calculations
11) Clean up

-Paulo Santillan

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