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1. Working Principle of Lead - acid Batteries

• When charging, the positive pole of the power supply is connected to the positive pole of the battery, and the negative pole of the power supply is connected to the negative pole of the battery. Under the action of an external power supply, lead sulfate (PbSO₄) on the positive plate is oxidized to regenerate lead dioxide (PbO₂). The reaction equation is: PbSO₄ - 2e⁻+ 2H₂O→PbO₂ + 4H⁺+SO₄²⁻. On the negative plate, lead sulfate (PbSO₄) is reduced to lead (Pb). The reaction equation is: PbSO₄+ 2e⁻→Pb + SO₄²⁻. As the charging progresses, the concentration of sulfuric acid (H₂SO₄) in the electrolyte gradually recovers, and the battery returns to its initial state.

• A lead - acid battery mainly consists of a positive plate (lead dioxide, PbO₂), a negative plate (spongy lead, Pb), and an electrolyte (sulfuric acid, H₂SO₄). During discharging, the lead (Pb) on the negative plate loses electrons to become lead ions (Pb²⁺), and the electrons flow to the positive plate through the external circuit. The chemical equation is: Pb - 2e⁻→Pb²⁺. At the same time, the lead ions (Pb²⁺) combine with sulfate ions (SO₄²⁻) in the electrolyte to form lead sulfate (PbSO₄) on the surface of the negative plate. The chemical equation is: Pb²⁺+SO₄²⁻→PbSO₄.

• On the positive plate side, lead dioxide (PbO₂) gains electrons and reacts with hydrogen ions (H⁺) and sulfate ions (SO₄²⁻) in the electrolyte. First, lead dioxide (PbO₂) gains electrons and reacts with hydrogen ions (H⁺) to form water (H₂O) and lead ions (Pb²⁺). The chemical equation is: PbO₂ + 2e⁻+ 4H⁺→Pb²⁺+ 2H₂O. Then, the generated lead ions (Pb²⁺) combine with sulfate ions (SO₄²⁻) to form lead sulfate (PbSO₄). The chemical equation is: Pb²⁺+SO₄²⁻→PbSO₄.

• Discharging Process

• Charging Process

2. Working Principle of Lithium Batteries

• When charging, the external power supply provides energy to make the lithium ions (Li⁺) be extracted from the negative electrode graphite (C) and move to the positive electrode through the electrolyte. The reaction of the negative electrode is: LiₓC - xe⁻→xLi⁺+ C. After the lithium ions (Li⁺) return to the positive electrode, they are re - inserted into lithium - iron - phosphate (LiFePO₄). The reaction of the positive electrode is: Li₁ - xFePO₄+ xLi⁺+ xe⁻→LiFePO₄. As the charging progresses, the battery's charge gradually increases until it is fully charged.

• The positive electrode of a lithium - iron - phosphate battery is lithium - iron - phosphate (LiFePO₄), the negative electrode is generally graphite (C), and the electrolyte is an organic solvent containing lithium salts. During discharging, lithium ions (Li⁺) are extracted from the positive electrode material lithium - iron - phosphate (LiFePO₄) and move to the negative electrode through the electrolyte. The reaction that occurs in the positive electrode material is: LiFePO₄ - xLi⁺- xe⁻→Li₁ - xFePO₄ (x represents the number of extracted lithium ions).

• After the lithium ions (Li⁺) reach the negative electrode, they are inserted into the layered structure of graphite (C), and at the same time, electrons flow from the positive electrode to the negative electrode through the external circuit and combine with the lithium ions. The reaction of the negative electrode is: xLi⁺+ xe⁻+ C→LiₓC. In this process, the battery releases electrical energy to the external circuit.

• Discharging Process of Lithium - iron - phosphate Batteries (LiFePO₄) as an Example

• Charging Process

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