Zinc reacts with sulfuric acid to produce hydrogen. The reaction is catalysed by copper. The rate of reaction can be compared by means of the rate of production of hydrogen gas bubbles.
This is a quick and easy experiment that can be done individually or in pairs.
Each student or pair of students will require:
Measuring cylinder (10 cm3)
Granulated zinc, a few pieces
Copper turnings or powder, a few pieces / half a spatula
Dilute sulfuric acid, 1 M (IRRITANT), 15 cm3
Copper(II) sulfate(VI) solution, 0.5 M, a few cm3
Refer to Health & Safety and Technical notes section below for additional information.
Health & Safety and Technical notes
Dilute sulfuric acid, H2SO4(aq) (IRRITANT) - see CLEAPSS Hazcard, CLEAPSS Recipe Book and CLEAPSS L195 ‘Safer chemicals, safer reactions’.
Copper(II) sulfate(VI) solution, CuSO4(aq) - see CLEAPSS Hazcard and CLEAPSS Recipe Book.
a Put a few pieces of granulated zinc into each of the three test-tubes. Try to have approximately the same amount in each test-tube.
b Add 5 cm3 of dilute sulfuric acid to test-tube 1. Note the rate of production of gas bubbles.
c Add a few copper turnings to test-tube 2. Make sure they are in contact with the zinc. Add 5 cm3 of dilute sulfuric acid and note the rate of production of gas bubbles.
d Add 5 cm3 of dilute sulfuric acid to test-tube 3. Then add about 1 cm3 of the copper sulfate solution using a dropping pipette. Note the rate of production of gas bubbles. Note what happens to the colour of the copper sulfate solution. Note what happens to the surface of the pieces of zinc.
If the granulated zinc pieces are shiny then the reaction in test-tube 1 is slow. The reaction may be faster if the zinc is not very pure. Bubbles of hydrogen form on the surface of the zinc. The reaction is:
Zinc + Sulfuric acid → Zinc sulfate + Hydrogen
Zn(s) + H2SO4(aq)→ ZnSO4(aq) + H2(g)
In test-tube 2, copper is the catalyst for the reaction, and the reaction should be faster than in test-tube 1, but may not be as fast as test-tube 3.
In test-tube 3, zinc displaces copper from the copper sulfate solution and the surface of the zinc goes black. The displaced copper metal then acts as a catalyst for the reaction.
Zinc + Copper sulfate → Zinc sulfate + Copper
Zn(s) + CuSO4 (aq) → ZnSO4(aq) + Cu(s)
There may be enough hydrogen produced in test-tube 3 for students to test for using a lighted splint.
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.