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 didnât heat the solid long enough in Experiment 1.
b) The balance wasnât 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.
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 didnât heat the solid long enough in Experiment 1.
b) The balance wasnât 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.
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