Copper Nails Moles

Lab 4B

Objectives: Objectives of this lab include determining the number of moles of copper produced in the reaction of copper (II) chloride, determining the number of moles of iron used up in the reaction of iron and copper (II) chloride, to determine the ratio of iron to copper, and to determine the number of atoms and formula units involved in the reaction.

Materials: As found in “Heath Chemistry” Experiment 4B p. 55

Procedure: As found in “Heath Chemistry” Experiment 4B p. 55 – 56

Observations: The copper (II) Chloride and water turned a ocean blue color. After the nails were cleaned with sandpaper, the nails were submerged with the copper (II) chloride. The nails at this point turned a brown murky color. The nail also had some copper on it, which was then scraped off. After the reaction, the weights of the iron nails were 1.72 grams, whist the beaker with the copper is approx. 49.43

Questions and Calculations:

1. a) Mass of iron used in reaction: 2.21g - `1.72 g = 0.49g

b) Mass of copper (II) Chloride used 55.75g – 49.43g = 6.1g

c) Mass of copper produced: 49.43 – 48.93 = 0.6g

1. a) Iron mm = 55.8

     0.49/55.8 = 6.6 * 10^-3 moles

b)  Copper mm = 63.5

         0.6g/63.5 =  9.2 * 10^-3 moles

1. a) 6.6 * 10^-3 moles * 6.02 * 10^23 = 5.3 * 10^21

b) 9.2 * 10^-3 moles * 6.02 * 10^23 =  5.7 * 10^21

   4.    9.2 * 10^-3 : 6.6 * 10^-3

              0.0092 : 0.0066 = 1.37

1. Yes there was. The aqua blue colors on the dried pieces of copper is the evidence. This is because in this experiment, it was impossible to get all of the copper (II0 chloride out.

Follow up Questions

1. 34.0g / 55.8 = 0.61 moles * 1.37 = 0.84 mols of copper
2. 45.0/63.5 = 0.71 moles / 1.37 = 0.51 mols of iron
3. 0.71 moles * 6.02 * 10^23 = 4.3 * 10^23 (atoms)
4. 0.61 moles * 6.02 * 10^23 = 3.7 ~ 10^23 (atoms)
5. 456 g of iron * 1.37 (ratio) = 624.7g of copper

  Conclusion

   In conclusion, the lab objectives have been completed. The ratio of iron to copper (1.37) has been determined, the number of atoms in the reaction has been determined, as well as the amount of moles. The weights of the equipment and chemicals has been determined. In the actual experiment, there was a blue color left in the beaker with the dried copper. This was determined to be Copper (II) Chloride. There potentially could have been less if the beaker was washed with distilled water more than once.