What is the relationship between the electrolytic cell and the galvanic cell? What are their common

First, the similarities.

Both involve the conversion of electrical and chemical energy; There is a transfer of electrons; There is a conductive solution in the device; Redox reactions occur.

Second, the differences.

1. The energy conversion is different.

A galvanic cell is a device that converts chemical energy into electrical energy, while an electrolytic cell is a device that converts electrical energy into chemical energy.

2. The principle is different.

The principle of galvanic cell reaction is that the reducing agent loses electrons on the negative electrode and undergoes oxidation reaction, and the electrons are transported to the positive electrode through the external circuit, and the electrons obtained by the oxidant on the positive electrode undergo a reduction reaction, so as to complete the transfer of electrons between the reducing agent and the oxidant, and generate an electric current.

The electrolytic cell is to pass an electric current through the electrolyte solution or molten electrolyte and cause a reduction oxidation reaction on the cathode and anode. The principle of reaction of the two is reversed.

3. The flow direction of electrons is different.

The electrons of the galvanic cell flow from the negative electrode to the positive electrode, and the electrons of the electrolytic cell flow from the negative electrode of the power supply to the cathode and from the anode to the positive electrode of the power supply.

4. The direction of the current is different.

The current direction of the galvanic cell is from the positive electrode to the negative electrode, and the current direction of the electrolytic cell is from the positive electrode of the power supply to the anode, and the cathode to the negative electrode of the power supply.

The fundamental difference between an electrolytic cell and a battery is the way they work. A battery is a device that converts chemical energy into electrical energy and consists of two or more battery cells (battery cells), usually constructed by placing metallic and non-metallic parts in electrolytes in different towns, which are isolated from each other but connected by conductive materials such as electrolytes. After a single use, the battery needs to be charged to regenerate the chemistry so that it can be used again.

A primary battery is a non-rechargeable battery that produces electricity from a chemical reaction between two or more different metals. It is usually disposable, i.e. it is used once and then loses its effectiveness. In contrast, a secondary battery is rechargeable and can undergo a chemical reaction to convert the stored energy into electricity, which can then be charged by the battery to regenerate the chemical reaction for reuse.

An electrochemical cell is a chemical device that converts chemicals into electrical energy and is often used in academic experiments for electrochemical or redox reactions. It consists of two or more electrode parts that pass through the electrolyte, connected by wires. In an electrolyte, substances of different potentials undergo a chemical reaction to produce electrical energy.

Remember a few words:

Galvanic battery: loss of high oxygen negative (loss of electrons, valency increases, oxidized, is the negative electrode) low and positive (electrons are obtained, valency is reduced, is reduced, is positive) electrons from the negative electrode through the external circuit to.

Cathode electrolytic cell: oxygen yang to yin (loss of electrons, oxidation, anode; Electrons are obtained, reduced, and made as cathodes) Due to the action of the applied electric field, the cations in the electrolytic cell move directionally, and the anode moves to the cathode to generate current.

Galvanic cell and electrolytic cell principle:

The working principle of galvanic batteries: chemical energy is converted into electrical energy through spontaneous redox reactions.

The working principle of the electrolytic cell: the power supply is linked, so that the current is forced to undergo a non-spontaneous redox reaction on the cathode and anode electrodes through the electrolyte solution, so as to convert the electrical energy into chemical energy.

Compare the galvanic cell and the electrolytic cell with **.

The principle is redox reaction. In the electrolytic cell, an external power supply is applied to force the redox reaction to occur, converting electrical energy into chemical energy. In galvanic batteries, chemical energy is converted into electrical energy by using a spontaneous redox reaction.

The galvanic battery can be discharged externally, and the electrode undergoes redox reaction, which consumes the electrode material and converts chemical energy into electrical energy; The electrolytic cell is an external power supply to supply power to the system, so that the electrodes undergo redox and the electrical energy is converted into chemical energy.