Labs / Chemistry
Galvanic Cell
Pick a metal for each half-cell and click the switch to close the circuit. The metal that gives up electrons more easily becomes the anode, electrons stream through the wire to the cathode, and ions drift across the salt bridge to keep each beaker neutral. The meter shows the voltage predicted by the standard reduction potentials.
E°cell 1.10 VEcell 1.10 Ve⁻ → Cu
What to try
- Which pairing gives the biggest voltage — and which metal always ends up as the anode no matter what it's paired with?
- Put the same metal on both sides. Why does the meter read 0 V and the electrons stop moving?
- Swap the two metals so the anode and cathode trade places. Which way do the electrons flow now?
- Dilute the cathode's ion solution. Why does a lower concentration pull the cell voltage down (the Nernst equation)?
- Open the switch while a reaction is running. Where does the voltage go, and why do the ions in the salt bridge stop drifting?