Finding the formula of copper oxide
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Students heat copper(II) oxide in a glass tube while passing methane over it. The copper(II)
oxide is reduced to copper. If the reactants and products are weighed carefully the formula of
the copper oxide can be deduced. This could also be used simply as an example of reduction.
Lesson organisation
This experiment is likely to take up to an hour, perhaps more to analyse the results. Students
who have not carried out this type of reaction before may find it helpful to have the
techniques demonstrated first. It is not really suitable for a class practical for students under
the age of 14, but could be a useful demonstration.
Each pair or group of students will need access to 2 gas taps.
The students will need access to matches or lighters to light their Bunsen burners.
Alternatively, light a few around the room and students can light their own using a splint.
Apparatus and chemicals
Per pair or group of students:
Eye protection
•
Reaction tube, (hard glass test-tube with small hole near closed end: see note 2)
1-hole bung with glass tube to fit the reduction tube
Rubber tubing
Retort stand
Boss
Clamp
Bunsen burner
Heat resistant mat
Spatula
Copper(II) oxide (Harmful, Dangerous for the environment), 2 spatulas (see note 1)
Access to:
Balance – must be accurate to at least 0.01g
Technical notes
Copper(II) oxide (Harmful, Dangerous for the environment) Refer to CLEAPSS® Hazcard 26
1 For best results use wire form copper(II) oxide. Alternatively, use analytical grade
copper(II) oxide which has been dried by heating in an open dish at 300–400 °C for 10
min and then stored in a dessicator.
It is also worth referring to the CLEAPSS® Laboratory Handbook Section 13.2.3 for further
information about this experiment.
2Hard glass test-tube with small hole near closed end. See experiment 14: making a
reaction tube.
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Procedure
•
HEALTH & SAFETY: Wear eye protection.
a Weigh the test tube with the
bung in (mass 1). Put 2 spatulas
of copper oxide into the tube
and spread it out as much as
possible.
excess methane
burned off
copper (II) oxide
from
gas tap
b Weigh the tube again, with the
copper oxide in it (mass 2).
c Assemble the apparatus as
shown in the diagram, but do
not place the Bunsen burner
underneath yet. Clamp the test
tube as near to the bung as
possible.
reaction tube
Bunsen burner
d Turn on the gas tap attached to
the test tube about half way to
get a steady flow of gas. This will
pass methane through the apparatus.
e Wait for a few moments, until you think that all the air will have flushed out of the tube
and then light the gas coming out of the hole at the end of the tube. If this experiment
is a student activity, a teacher should supervise this step. Take care not to lean over the
tube as you light the gas. Adjust the gas tap so that the flame is about 3 cm high.
f Light the Bunsen burner and begin to heat the copper oxide in the tube. You will need
to use a roaring flame (air hole fully open). You will need to pick up the Bunsen burner
and move the flame around to heat every bit of the copper oxide. Ensure that the hottest
part of the Bunsen burner flame (the top of the inner cone) is being used for heating. If
there are parts which look unreacted, gently shake the tube – it will be very hot so do so
by gently shaking the clamp stand.
g When all the copper oxide looks like it has reacted (it will look like copper), keep heating
for a minute or two and then turn off the Bunsen burner.
h Keep the methane passing over the product as it cools down to prevent it from reacting
with any oxygen present and turning back into copper oxide. When the tube is cool,
switch off the gas.
i
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Weigh the test tube with the bung and the product (mass 3).
Teaching notes
Students should have recorded the following masses:
(mass 1) Test tube + bung
(mass 2) Test tube + bung + copper oxide
(mass 3) Test tube + bung + copper (product)
This should allow them to calculate the mass of the mass of the copper oxide (mass 2)
- (mass 1) and the mass of the copper (mass 3) - (mass 1). They should also calculate the
decrease in mass (mass 3) - (mass 2), which corresponds to the mass of oxygen.
With this information they can calculate the formula of the copper oxide.
Students will also need the relative atomic masses. Copper is 63.5 and oxygen is 16.
They should divide mass by the atomic mass for each element. This will give the number of
moles of each.
Having done this for both elements, they should find the ratio between the two by dividing
them both by the smallest number.
The ratio should be close to 1:1 as the formula of copper oxide is CuO.
Example calculation
Mass copper oxide = 1.76 g
Mass copper = 1.43 g
So mass oxygen = 0.33 g
Number moles Cu = 1.43/63.5 = 0.02251
Number moles O = 0.33/16 = 0.020625
Divide by the smallest to give the ratio aprox. 1 Cu: 1 O
This would suggest a formula of CuO, which is the correct formula.
Reference
This experiment has been adapted from Practical Chemistry:
http://www.practicalchemistry.org/experiments/intermediate/elements-compounds-andmixtures/finding-the-formula-of-copper-oxide,210,EX.html
Health & Safety checked, April 2008
Updated 29 Oct 2008
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