Class practical or demonstration
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.
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.
Per pair of group of students:
Reduction tube, (hard glass test-tube with small hole near closed end)
1-hole bung with glass tube to fit the reduction tube
Clamp stand, boss and clamp
Heat resistant mat
Balance – must be accurate to at least 0.01g
Copper(II) oxide (HARMFUL, DANGEROUS FOR THE ENVIRONMENT), 2 spatulas
Methane (natural gas) (EXTREMELY FLAMMABLE)
Refer to Health & Safety and Technical notes section below for additional information
Health & Safety and Technical notes
Wear eye protection.
Copper(II) oxide, CuO(s), (HARMFUL, DANGEROUS FOR THE ENVIRONMENT) - see CLEAPSS Hazcard. For best results 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 desiccator.
Methane (natural gas), CH4(g), (EXTREMELY FLAMMABLE) - see CLEAPSS Hazcard. It is likely that most school will be using a class gas tap for this experiment. This gas forms explosive mixtures in the air
It is also worth referring to the CLEAPSS Laboratory Handbook Section 13.2.3 for further information about this experiment
a Weigh the test tube with the bung in (mass 1). Put 2 spatulas of copper(II) oxide into the tube and spread it out as much as possible.
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.
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 at least 10 seconds, to allow all the air to be 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 further 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 Weigh the test tube with the bung and the product (mass 3).
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.
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 approx. 1 Cu: 1 O
This would suggest a formula of CuO, which is the correct formula.
Health & Safety checked 2016
This Practical Chemistry resource was developed by the Nuffield Foundation and the Royal Society of Chemistry.
© Nuffield Foundation and the Royal Society of Chemistry
Page last updated October 2015
This is a resource from the Practical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany Practical Physics and Practical Biology.
The experiment is also part of the Royal Society of Chemistry’s Continuing Professional Development course: Chemistry for non-specialists