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साधारणतया तरल अम्ल जस्तै सल्फ्युरिक अम्लमा तामा धातु र जस्ता धातुका पाताहरूलाई डुबाएर तयार पारिएको एक प्रकारको सेललाई साधारण सेल भनिन्छ । यसबाट थोरै मात्रामा विद्युत उत्पादन गर्न सकिन्छ ।

साधारण ग्यालभानिक सेल

A manual of practical medical electricity - the Röntgen rays and Finsen light (1902) (14597134537)

रसायान-विज्ञान

Cross-section of a copper/zinc cell with a sulfuric acid electrolyte. The drawing illustrates the atomic model for the chemical reactions; lemon cells have essentially the same model. Zinc atoms enter the electrolyte as ions missing two electrons (Zn²⁺). Two negatively charged electrons from the dissolved zinc atom are left in the zinc metal. Two of the dissolved protons (H⁺) in the acidic electrolyte combine with each other and two electrons to form molecular hydrogen H₂, which bubbles off of the copper electrode. The electrons lost from the copper are made up by moving two electrons from the zinc through the external wire.

Most textbooks present the following model for the chemical reactions of a lemon battery. When the cell is providing an electric current through an external circuit, the metallic zinc at the surface of the zinc electrode is dissolving into the solution. Zinc atoms dissolve into the liquid electrolyte as electrically charged ions (Zn²⁺), leaving 2 negatively charged electrons (e⁻) behind in the metal:

Zn → Zn²⁺ + 2e⁻ .

This reaction is called oxidation. While zinc is entering the electrolyte, two positively charged hydrogen ions (H⁺) from the electrolyte combine with two electrons at the copper electrode's surface and form an uncharged hydrogen molecule (H₂):

2H⁺+ 2e⁻ → H₂ .

This reaction is called reduction. The electrons used in the copper to form the molecules of hydrogen are transferred from the zinc through an external wire connecting between the copper and the zinc. The hydrogen molecules formed on the surface of the copper by the reduction reaction ultimately bubble away as hydrogen gas.

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