Chemistry: Moles of Iron and Copper "Quick" Lab
Introduction:
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The mole is a convenient way to express the amount of substance. The mole is equal to 6.02 x 10 particles, or Avogadro' s
number of particles . More important, however, than the number of particles in a mole is the mass of a mole of an element. It is the mass
in grams corresponding to the atomic weight. Simply stated, the mass of one copper atom is 63.5 amu; the mass of one mole of copper
atoms is 63.5 grams.
In this experiment, you will observe a chemical reaction of iron with copper (II) chloride. You will determine the amount of iron
consumed in the reaction as well as the amount of copper produced.
Fe + CuCl2  Cu + FeCl2
Procedure:
Part One:
1.
Obtain a small plastic cup and write your names on it.
2.
Using an electronic balance, find the mass of the plastic cup. Record this value your data table.
3.
Add approximately 2 grams of copper (II) chloride to the plastic cup. Then, add 25 mL of distilled water.
4.
Using a stirring rod, make sure all of the copper (II) chloride has dissolved.
5.
Obtain two clean dry nails. Use a piece of sandpaper to make the surface of the nails shiny.
6.
Using an electronic balance, find the mass of the two nails. Be sure to record this value in your data table.
7.
Place the nails in the copper (II) chloride solution. Leave the nails undisturbed. During that time, you should see the
formation of copper in the plastic cup. At the same time, some of the iron will react.
Part Two:
1.
Use tongs to carefully pick up the nails, one at a time. Use a wash bottle to rinse any remaining copper from the nails
before removing them completely. If necessary, use a stirring rod to scrape any copper from the nails. Set the nails aside
to dry on a paper towel.
Use distilled water from
the bottle to wash any
copper remaining on the
nails into the beaker
2.
Decant means to pour off the liquid from a container that hold both a solid and liquid. Carefully decant the liquid from
the solid. Pour the liquid into a 400 mL beaker so that incase some of the solid is poured out, you can retrieve it.
When decanting, it ishelpful to
direct the liquid into the second beaker
along a stirring rod, as shown here.
3.
After decanting, rinse the solid with about 15 mL of distilled water. Decant again. Repeat this step 3 more times.
4.
After the final wash and decant, place the plastic cup with the copper in the class tray to dry overnight. Be sure your plastic
cup has some identification so you can retrieve it the following day.
5.
Find the mass of the two nails and record this inthe data table.
6.
Before leaving the laboratory, clean up all materials and wash your hands.
Part Three:
1.
Find your plastic cup containing the copper. Using an electronic balance, find the mass of the plastic cup and copper
produced. Record this value in the data table.
2.
Dispose of the plastic cup by placing it in the garbage can.
3.
Wash your hands.
DATA TABLE
1. Mass of plastic cup
2. Mass of two nails (before reaction)
3. Mass of two nails (after reaction)
4. Mass of plastic cup + copper produced
Calculations - SHOW WORK ON ALL CALCULATI ONS!
1.
Calculate the mass of iron consumed in the reaction.
2.
Determine the number of moles of iron consumed in the reaction.
3.
How many atoms of iron were consumed inthe reaction?
4.
Calculate the mass of copper produced inthe reaction.
5.
Determine the number of moles of copper produced in the reaction.
6.
How many atoms of copper were produced in the reaction?
Conclusions 1.
The equation for the reaction you performed in this experiment is listed inthe introduction, what other substance is
produced inthis reaction besides copper?
2.
How did the mass of the iron nails before the reaction compare to the mass of the nails after the reaction? How can you
account for this difference?