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EXPERIMENT
6
OBJECTIVE
APPARATUS
AND
CHEMICALS
Elemental Mass Percent and
Empirical Formula From
Decomposition of a Copper Oxide
Prepared by Edward L. Brown, Lee University and
Verrill M. Norwood, Cleveland State Community College
The student will heat copper oxide in a methane atmosphere forming elemental
copper. The masses of the original CuO and the resulting Cu will be used to
arrive at the mass percent and empirical formula of the copper oxide.
Elemental Mass Percent
In today’s lab, the decomposition of copper oxide (CuxOy) provides the mass data needed
to determine the mass percent of both elements.
Empirical Formulas
The empirical formula of a compound is the simplest whole number ratio of its elements.
This ratio can be either an atomic ratio or a molar ratio. The experimental determination
of a compound’s empirical formula occurs in three steps:
AA PP PP AA RR AA TT UU SS
Ring Stand 15 cm Pyrex test tube
Bunsen Burner Glass tubing (bent)
Rubber tubing
CC HH EE MM II CC AA LL SS
Copper oxide (CuxOy)
Elemental Mass Percent and Empirical Formula From Decomposition
of a Copper Oxide
CHEM 1001 - Experiment 6 6-2
Step 1: Determine the mass of each element present.
Step 2: Convert the individual elemental masses into the number of moles of
each element.
Step 3: Express the molar ratio of the two elements by dividing the number of
moles of each element by the smaller of the two numbers. This will
assign “1 mole” to the element with the smallest number of moles and
the other element will be assigned a number greater than or equal to “1
mole”.
Sample Problem 1: The electrolysis (decomposition) of water produces hydrogen and
oxygen gases. From the mass of the elements given in step 1, what is the empirical
formula of water?
Step 1: Mass of the Elements 0.002085 g H 0.01715 g O
Step 2: Moles of the Elements 2.085E-3 g ÷ 1.0079 g/mol 1.715E-2g ÷ 16 g/mol
2.0686E-3 mol H 1.072E-3 mol O
Step 3: Divide by smallest moles 1.93 mol H 1.00 mol O
Step 4: Write the empirical formula H2O1 or simply H2O
Decomposition of CuxOy
Copper oxide exists as either Copper I (cuprous) or Copper II (cupric) oxide. Heating
either of these compounds with methane (CH4) gas will produce copper metal. Your
unknown could be copper I oxide or copper II oxide.
1. Flame dry a Pyrex test tube (15 cm or longer) by holding it vertically (mouth upward)
with tongs in the flame of a Bunsen burner for 3 – 4 minutes. Rest the hot test tube on
a clean dry surface until it has cooled to room temperature (about 5 minutes).
Determine the mass of the test tube [Data Sheet Q1] by taring a small beaker on the
balance and then placing your test tube in the beaker.
2. After recording the mass of the test tube, add 1.000 g 0.200 g of copper oxide.
PROCEDURE
Elemental Mass Percent and Empirical Formula From Decomposition
of a Copper Oxide
CHEM 1001 - Experiment 6 6-3
hold the test tube over the copper
oxide container and add a little
copper oxide.
gently place the test tube in the
beaker and note the mass.
if the mass is 1.000 g 0.200 g
greater than the mass of the empty
test tube, record the exact mass
[Data Sheet Q2], if not, add more
copper oxide.
Record the 4 digit Unknown
Number of the Copper Oxide you
used [Data Sheet Q3].
3. Clamp the test tube to a ring stand with a
bare metal test tube clamp.
4. Assemble the remaining apparatus as shown in Figure 1 but DO NOT TURN ON
THE GAS.
5. Next, light only the Bunsen burner – THIS SHOULD NOT BE AN EXTREMELY HOT
FLAME.
6. HAVE YOUR INSTRUCTOR ASSIST YOU WITH THE
LIGHTING OF THE GAS THAT EXITS THE TEST TUBE.
7. Heat the copper oxide with a cool flame for 5 minutes.
8. Then, adjust the Bunsen burner to produce a hot flame. Heat the test tube with this hot
flame for 10 – 40 minutes (depending on the type of copper oxide used). You will see
a copper colored compound form during this heating process. Periodically ask your
Instructor if your experiment is finished or not.
9. If your Instructor says that your experiment is finished, turn off the gas to the Bunsen
burner, but allow the flame to keep burning at the mouth of the test tube while the rest
of the test tube cools down.
10. After 5 minutes, turn off the gas to the test tube and carefully remove the glass tubing
(Caution: HOT!). Allow the test tube to cool to room temperature.
11. Record the mass of the test tube and copper metal [Data Sheet Q4].
Figure 1
Rubber tubingto gas outlet
Elemental Mass Percent and Empirical Formula From Decomposition
of a Copper Oxide
CHEM 1001 - Experiment 6 6-4
12. Remove the copper from the test tube and rub it gently on a hard surface (i.e. the
bottom of a porcelain well plate) to produce the familiar shiny look and color of
copper. You may dispose of this copper metal in the trash OR keep it as a lab
souvenir.
Waste Disposal: If you don’t keep it as a souvenir, the elemental copper can be
placed in the regular trash container.
Lab Report: Once you have turned in your Instructor Data Sheet, lab attendance will
be entered and you will be permitted to access the online data submission / calculation
part of the lab report (click on Lab 6 – Empirical Formula of Copper Oxide). Enter
your data accurately to avoid penalty. The lab program will take you in order to each
calculation. If there is an error, you will be given additional submissions (the number and
penalty to be determined by your instructor) to correct your calculation.
CHEM 1001 - Experiment 6 6-5
CHEM 1010 - Lab 6 Student Data Sheet
1. Mass of the test tube g
2. Mass of the test tube + Copper Oxide g
3. Unknown Number of the Copper Oxide (4 digits)
4. Mass of the test tube + Copper metal g
CHEM 1010 - Lab 6 Instructor Data Sheet
1. Mass of the test tube g
2. Mass of the test tube + Copper Oxide g
3. Unknown Number of the Copper Oxide (4 digits)
4. Mass of the test tube + Copper metal g
Name:
Section: