Galvanic Cell Simulator

Pick two half-cells. The simulator identifies the anode and cathode, shows electron flow, and calculates E°cell, ΔG°, K, and the Nernst potential at 25 °C.

Want the concepts first? Read the galvanic-cells lesson or review standard reduction potentials.

Left half-cell[Zn²⁺] = 1.000 M

Right half-cell[Cu²⁺] = 1.000 M

Results

Anode (oxidation)Zn(s) → Zn²⁺ + 2e⁻

Cathode (reduction)Cu²⁺ + 2e⁻ → Cu(s)

Net reactionZn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

Electrons transferred (n)2

E°cell = E°cathode − E°anode+0.34 V − (−0.76 V) = +1.10 V

ΔG° = −nFE°-212 kJ/mol

K10^37.2

Q1.000

Ecell = E° − (0.05916/n) log Q+1.10 V

Ecell > 0: the reaction is spontaneous as written. Salt-bridge anions migrate toward the anode; cations migrate toward the cathode.

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