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SUBSTITUTE THESE VALUES TO COMPLETE YOUR CALCULATIONS
CHM-201 General Chemistry and Laboratory I
Laboratory 2 – Empirical Formula of an Oxide
Fall 2020
Section H1
Group A Name PATRICK ALMEIDA (Substitute Data)
Mass of the crucible and cover
Mass Difference from previous
After 1st heating
After 2nd heating 32.9865g
After 3rd heating (if necessary)
After 4th heating (if necessary)
(use the final value in your report)
Mass of crucible, cover and magnesium before heating 33.2251g
Obsevations after adding water to the crucible (after heating and reacting the magnesium):
Mass of the crucible, cover and magnesium oxide
Mass Difference from previous
After 1st heating
After 2nd heating 33.3667g
After 3rd heating (if necessary)
After 4th heating (if necessary)
(use the final value in your report)
Almeida
Lab_2_Group_A-H1_Data
Image_00001
Image_00002
Image_00003
Image_00004
Image_00005
Image_00006
Image_00007
Image_00008
Laboratory_2_Report-CHM201-H1-Group_A
Name
Section H1
Group A
PLEASE ENABLE EDITING BEFORE FILLING OUT THIS REPORT!
This report form is complete. There is no need to add additional information,
such as conclusions.
Report Due on or before November 1, 2020
I will accept no reports after November 15, 2020
Please save this file as a pdf and submit it on Moodle.
Individual Results
1. Mass of Empty Crucible and Magnesium (10 points)
2. Mass of Crucible containing Oxide (10 points)
3. Calculation of empirical formula using data from your group only (30 points)
1. Mass of crucible and lid with magnesium
2. Mass of empty crucible and lid (from your group’s data)
3. Mass of magnesium only
1. Mass of crucible and lid containing magnesium oxide
2. Mass of empty crucible and lid (from your group’s data)
3. Mass of oxide only
1. Total mass of oxide formed
2. Total mass of magnesium
3. Total mass of oxygen in the oxide
4. Total moles of magnesium
5. Total moles of oxygen present in the oxide
6. Ratio of moles of oxygen to moles of magnesium
4. Group results – compute this information from the class data below (calculate the sums of the
group’s results)
This table is a worksheet. You may show the results of each calculation here if you wish, but it is not
equired.
Section H1
Group A
Mass of
C+C
Mass of
Mg+C+C
Mass of
MgO+C+C
Mass of
MgO
Mass of
Mg
Mass of
O
XXXXXXXXXX3667
Masses are
all in grams
(g)
XXXXXXXXXX1814
XXXXXXXXXX4505
XXXXXXXXXX1802
XXXXXXXXXX3633
XXXXXXXXXX6843
XXXXXXXXXX8895
XXXXXXXXXX8467
Totals
5. Calculation of empirical formula using data from all data in your group (above) (20 points)
Questions
1. This experiment depends on how accurately you measured the masses. (10 points)
a) Give at least one reason why the mass could be lower than expected and one reason why the
mass could be higher than expected. Which of these cases do you think best represents your
esults? Explain.
) If you computed the average masses of magnesium and magnesium oxide rather than the total
mass, would it make any difference in the result? Explain.
1. Total mass of oxide formed (group data)
2. Total mass of magnesium (group data)
3. Total mass of oxygen in the oxide
4. Total moles of magnesium
5. Total moles of oxygen present in the oxide
6. Ratio of moles of oxygen to moles of magnesium
7. Empirical formula for the magnesium oxide
2. Write balanced chemical equations for the following reactions (you will need to review the
information provided in the introduction to this laboratory for the formulas involved. Remember that
oxygen and nitrogen are diatomic. (20 points)
a) The reaction of magnesium with oxygen
) The reaction of magnesium with nitrogen
c) The reaction of magnesium nitride with water
d) The reaction of magnesium hydroxide when heated
Name
Individual Results
Questions