Chemistry · Chapter 17

Build a Galvanic Cell

Drop any two half-cells into the two beakers. The model works out which one is the anode, points the electrons and the ions the right way, and reads out the cell potential. Try putting the stronger one on the left and watch everything turn around.

Your cell labels follow your choice

A galvanic cell built from the two half-cells you chose

The three equations

Both half-reactions scaled to the same electron count, and the overall reaction

Pick the half-cells

Classic pairs to try

Cell potential

1.10volts it runs
Arithmetic: 0.34 − (−0.76)
Electrons moved, n: 2
Free energy: −212 kJ/mol
Equilibrium constant: 1.6 × 1037
Anode on the left
Zinc is oxidized
Zinc sits lower on the table, so it gives up its electrons.

Cell notation

Zn(s) | Zn2+ || Cu2+ | Cu(s)

The anode always goes on the left. One bar marks a change of phase. The double bar is the salt bridge. An inert platinum strip appears whenever the half-cell has no solid of its own to use.