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Bunny Greenfelder
Bunny GreenfelderLv2
20 Oct 2019

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Related questions

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.

Write the balanced chemical equation for the reactions listed below. You will have to write the molecular and net ionic equation for each reaction.

1. a. copper (II) nitrate solution combined with a solution of sodium hydroxide

2. lead (II) nitrate solution combined with hydrochloric acid

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