.  . .
Me06 Zinc and copper in a Galvanic Cell made of two Half Cells

In the following experiment the metals from the Cola cans are replaced by zinc (Zn) and copper (Cu).
Weigh the electrodes at the beginning and in the end of the experiment to measure what happens with their masses during the flow of electricity.
What you need: Scale, weights, Zn and of Cu sheets, 2 insulated copper wires with 4 crocodile clips, digital multimeter, 2 vials with copper and zinc salt solutions, wick from tissue paper.
Experiment: * Left: Weigh the metal sheets: Zn = 1.0 g,  Cu 1.1 g.
* Photo 2: Dip these electrodes into the solutions of their salts.
* Connect them to the multimeter like in the previous experiment. * Dip the wick into the two solutions.
Observations: The voltage reads 0.9 Volt. Photo 2: The current is 0.3 µA.
* Photo 3: Leave the device for some days, while zinc and copper directly connected by a wire.
Observations Photo 3 and right: The size (and mass) of the Cu electode has increased, the blue colour fades, the mass of the Zn electrode decreased.
Explanations: As an electron donor zinc pushed electrons through the wire to the copper electrode.
Thes copper ions are reduced:   Zn(s) + Cu²⁺(aq) ----indirect redox reaction---> Zn²⁺(aq) + Cu(s)
Negative sulfate ions are flowing to the zinc half cell via wick.