Moles of Iron and Copper

During class on October 27, 2009, the whole class participated in a lab. Through this experiment, it's main objectives were to:

Determine the number of moles of copper produced in the reaction of iron and copper(II) chloride

• Determine the number of moles of iron used up in the reaction of iron and copper(II) chloride
  

• Determine the ratio of moles of iron to moles of copper


• Determine the number of atoms and formula units involved in the reaction

The procedure of this particular lab consisted of:

1. Finding the mass of a clean, empty, dry 250 mL beaker. Record the mass to the nearest 0.01g.
2. Add aprrox. 8 grams of copper (II) cloride crystals to the beaker. Find the mass and record it in your notebook.
3. Add 50mL of distilled water to the beaker. Swirl th ebeaker around to dissolve all the copper(ii) chloride crystals.
4. Obtain two clean, dry nails. Find the mass of the nails and record it in your notebook.
5. Place the nails into the copper(II) chloride solution. Leave them undisturbed for approx. 20 minutes.
6. Use the tongs to carefully pick up the nails, one at a time. Use distilled water in a wash bottle to rinse off any remaining copper from the nails before removing them completely from the beaker.
7. After the nails are completely dry, find the mass of the nails and record it in your notebook.
8. Decan the liquid from the solid.
9. Rinse the solid again with about 25 mL of distilled water. Decant again. Repeat this step three or four times.
10. Wash the solid with about 25 mL of hydrochloric acid. Decant again; then, once more, clean the solid with 25 mL of distilled water.
11. After final washing, place the copper in a drying oven to dry.
12. Find the mass of the beaker plus the copper and record it in your notebook.
    

--Krizia Umali