Experiment 2 Trial 1 a) Mass of CuSO 4 ·5H 2 O (g) 90.000g b) Moles of CuSO 4 ·5

Question

Experiment 2

Trial 1   

a) Mass of CuSO4·5H2O (g)                                              90.000g

b) Moles of CuSO4·5H2O (mol)                                       _______   

c) Moles of copper in CuSO4·5H2O (mol)                      _______   

d) Mass of copper in CuSO4·5H2O (g)                            _______   

e) Mass of copper oxide obtained                                    29.267g

f) Mass of oxygen in copper oxide                                   _______   

g) Moles of oxygen in the copper oxide (mol)               _______

h) Mole ratio, copper to oxygen (Cu:O)                          _______

i Average ratio, copper to oxygen    (Cu:O) _______

j) Formula of copper oxide _______

Mass of empty beaker 85.000g

Mass of beaker and Copper (II) sulfate pentahydrate 90.000g

Mass of empty test tube 27.400g

Mass of test tube after heating and cooling 29.306g

Using your data from Trial 1, show your work for each of the following:

Moles of CuSO4·5H2O

Moles of copper in CuSO4·5H2O

Mass of copper in CuSO4·5H2O

Mass of oxygen in copper oxide      

Moles of oxygen in the copper oxide

Mole ratio, copper to oxygen

Questions

1. How would each of the following affect your experimental determination of your copper/oxygen ratio (too high, too low, or no effect)? In each case, explain your answers.

a) You didn’t heat the solid long enough in Experiment 1.

b) The balance wasn’t properly calibrated in Experiment 1, causing all masses to be too 0.50 g too high.

c) Not all of the copper sulfate was converted to copper hydroxide in Experiment 2.

2. Write a balanced equation for the reaction occurring between copper and oxygen in Experiment 1.

3. Write a balanced equation for the reaction occurring between copper (II) sulfate and NaOH in Experiment 2.

4. Write a balanced equation for the reaction that occurred when the precipitate from Experiment 2 was heated.

Explanation / Answer

Q1 and 2 is not clear as Experiment 1 is not mentioned.

Q3. CuSO4+ 2NaOH Cu(OH)2+ Na2SO4

Here blue precipitate of copper hydroxide is formed.

Q4. On heating of opper hydroxide, copper oxide, CuO is formed which is a black solid.

Cu(OH)2 (s) --> CuO (s) + H2O (l)

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