how Zinc reacts with Copper

The reaction between zinc and copper oxide In this experiment copper(II) oxide and zinc metal are reacted together. The reaction isexothermic and the products can be clearly identified. The experiment illustrates the difference in reactivity between zinc and copper and hence the idea of competition reactions. Lesson organisation This is best done as a demonstration. The reaction itself takes only three or four minutes but the class will almost certainly want to see it a second time. The necessary preparation can usefully be accompanied by a question and answer session. The zinc and copper oxide can be weighed out beforehand but should be mixed in front of the class. If a video camera is available, linked to a TV screen, the ‘action’ can be made more dramatic. Apparatus and chemicals Eye protection Bunsen burner Heat resistant mat Tin lid  Beaker (100 cm3) Circuit tester (battery, bulb and leads) (Optional) Safety screens (Optional) Test-tubes, 2 (Optional – see Procedure g) Test-tube rack Access to a balance weighing to the nearest 0.1 g The quantities given are for one demonstration. Copper(II) oxide powder (Harmful, Dangerous for the environment), 4 g  Zinc powder (Highly flammable, Dangerous for the environment), 1.6 g Dilute hydrochloric acid, approx. 2 mol dm-3 (Irritant), 20 cm3  Zinc oxide (Dangerous for the environment), a few grams Copper powder (Low hazard), a few grams. Concentrated nitric acid (Corrosive, Oxidising), 5 cm3 (Optional – see Procedure g) Technical notes Copper(II) oxide (Harmful, Dangerous for the environment) Refer to CLEAPSS Hazcard 26. Zinc powder (Highly flammable, Dangerous for the environment) Refer to CLEAPSS Hazcard 107 Dilute hydrochloric acid (Irritant at concentration used) Refer to CLEAPSS Hazcard 47A and Recipe Card 31 Concentrated nitric acid (Corrosive, Oxidising) Refer to CLEAPSS Hazcard 67 Copper powder (Low hazard) Refer to CLEAPSS Hazcard 26 Zinc oxide (Dangerous for the environment) Refer to CLEAPSS Hazcard 108. Procedure HEALTH & SAFETY: Wear eye protection throughout. Consider placing safety screens around the experiment (Samples of zinc can vary considerably in reactivity, depending on particle size and the state of surface oxidation.) a Weigh out 2 g (0.025 mol) of copper oxide and 1.6 g (0.025 mol) of zinc powder. b Mix thoroughly to give a uniformly grey powder. c Pour the mixture in the shape of a ‘sausage’ about 5 cm long onto a heat resistant mat or clean tin lid. d Heat one end of the ‘sausage’ from above with a roaring Bunsen flame until it begins to glow, then remove the flame. A glow will spread along the ‘sausage’ until it has all reacted. A white/grey mixture will remain. e Heat this to show that the white powder (zinc oxide) is yellow when hot and white when cool. f Pour the cool residue into a 100 cm3 beaker and add a little dilute hydrochloric acid to dissolve the zinc oxide (and also any unreacted zinc and copper oxide), warming if necessary. Red-brown copper will be left. This can be rinsed with water and passed around the class for observation. Show that the powder conducts electricity using a circuit tester. g If further confirmation of identity is required, treat a small amount of the red-brown powder with a few drops of concentrated nitric acid in a test-tube in a fume cupboard. A brown gas (NO2, Very Toxic) is given off as the copper reacts and dissolves. After the reaction adding a little water makes the blue solution of copper(II) nitrate visible. Teaching notes The depth of discussion depends on the level of the students involved. Essentially it is a competition between metal(1) and metal(2) for oxygen in a reaction represented by: Metal(1) + Metal(2) oxide → Metal(1) oxide + Metal(2) The more reactive metal displaces the less reactive metal from its oxide, as in the case of zinc and copper(II) oxide, for example: Zn(s) + CuO(s) → ZnO(s) + Cu(s) Demonstrate that zinc oxide goes yellow when heated and returns to white when cool to help confirm the identity of this product. (This phenomenon is caused by a change in crystal structure - a genuine example of a 'physical change'.) Where appropriate, it could be pointed out that these reactions are redox reactions, the more reactive metal behaving as a reducing agent, and the metal oxide acting as an oxidising agent. This could be extended to consider these redox reactions in terms of the loss and gain of electrons by the metals. Other metals can be used, but take care to compare like with like. Coarse magnesium powder, for example, gives a less vigorous reaction than powdered zinc. Finely powdered magnesium gives a very vigorous reaction and should only be attempted with great care. The reaction between aluminium powder and copper oxide is almost explosive and must not be attempted. Health & Safety checked, March 2009