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Copper (II) oxide and zinc metal react together in an exothermic reaction to produce zinc oxide and copper. By observing this reaction and its products, and noting the difference in reactivity between zinc and copper, students can familiarise themselves with the idea of competition reactions.
In this practical, students add powdered or finely-divided metals to a copper (II) sulfate solution and measure the temperature rises. The experiment reinforces ideas about energy changes during reactions, the reactivity series of the metals and the chemical behaviour of metals.
A temperature correction graph for a metal displacement reaction between zinc and copper sulfate solution. The zinc is added after 4 minutes. The steps to make a temperature correction graph are: Take a temperature reading before adding the reactants for a few minutes to get a steady value
Teaching notes. epends on the level of the students involved. Essentially it is a competition between metal(1) and met. 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)
5 sty 2022 · The circuit is a loop through the zinc, the wire, the copper, and the electrolyte, back to the zinc. Zinc dissolves in lemon juice, leaving zinc ions (Zn 2+ ) in the juice, while the two electrons per atom move through the wire toward the copper.
Zinc sulfate (or nitrate (V)) Five samples, approximately 1 cm lengths or squares, of each the following metals (note 2): Copper foil. Lead foil (TOXIC, DANGEROUS FOR THE ENVIRONMENT) Magnesium ribbon.
Zinc is more reactive than copper, so when zinc is added to copper (II) sulfate solution, copper is displaced. This reaction is associated with an enthalpy change and enthalpy is converted into heat energy. The heat energy warms up the surroundings (which in this case is the waste in which the reaction takes place. Materials:
