Zinc / Copper cell

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LEFT ELECTRODEOxidation

RIGHT ELECTRODEReduction

Salt bridge: NO₃⁻ → anode·K⁺ → cathode

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MODEL READYAnimation accelerated · not to scale

HALF-EQUATIONS

OXIDATIONZn(s) → Zn²⁺(aq) + 2e⁻

REDUCTIONCu²⁺(aq) + 2e⁻ → Cu(s)

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

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MEASURED POTENTIAL

+1.10 V

Red probe: right · Black: left

ANODE −ZnOxidation

CATHODE +CuReduction

HALF-EQUATIONS

OXIDATION

Zn(s) → Zn²⁺(aq) + 2e⁻

REDUCTION

Cu²⁺(aq) + 2e⁻ → Cu(s)

OVERALL REACTION

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

CELL POTENTIAL STANDARD

E°cell = E°cathode − E°anode

(+0.34) − (−0.76) = +1.10 V

CELL NOTATIONZn(s) │ Zn²⁺(aq) ‖ Cu²⁺(aq) │ Cu(s)