Chemistry

Difference Between Galvanic Cells And Electrolytic Cells

A Galvanic cell is an electrochemical cell in which an electric current is generated from a spontaneous reaction. A galvanic cell is used to supply current by making transfers of electrons by a redox reaction. while an electrolytic cell is an electrochemical cell used to generate a non-spontaneous redox reaction. In electrolytic cells, electrical energy is converted to chemical energy or vice versa. the basic Difference Between Galvanic Cells And Electrolytic Cells is that galvanic cells do not require an external voltage source and it changes chemical energy into electrical energy. on the other hand, an electrolytic cell requires an external voltage source, and it changes electrical energy into chemical energy.

Difference Between Galvanic Cells And Electrolytic Cells in Tabular Form

Galvanic Cells Electrolytic Cells
Spontaneous redox reactions occur in these cells that convert chemical energy into electric energy. Non-spontaneous redox reactions occur in these cells that convert electric energy into chemical energy.
the redox reactions are produced electrical energy. electrical energy is produced through chemical reactions with the help of external resources.
two electrodes are usually used one positive electrode or anode and one negative electrode or cathode. there are also two electrodes that are usually used one positive electrode or anode and one negative electrode or cathode.
the anode is responsible for the oxidation process and the cathode is responsible for the reduction process. the anode is responsible for the oxidation process and the cathode is responsible for the reduction process.
these cells are divided into two parts i.e. half the cell is placed in a different container and the other half is directly connected in a salt bridge. the cell is worked and contained as a single unit in which molten or solution electrolyte is used as Electrodes.
these batteries are commonly used in carriage buses and heavy motor vehicles. purifying copper and electroplating are common applications of such types of cells.
both ends/electrodes discharge the ions. ions are discharged only at the cathode.
with the help of an external circuit, electrons flow through the positive to the negative electrodes. on contrary, electrons flow through the external sources from negative to the positive electrodes.

Galvanic cells

Galvanic cells consist of two half-cells that convert the chemical potential energy into electrical potential energy also known as voltaic cells. In galvanic cells, spontaneous oxidation-reduction reactions produce electrical energy. Each half-cell contains an electrode in an electrolyte.

To prevent a direct chemical contact of the reduction and oxidation reactions by creating a potential difference, separation is required to do so. In oxidation reaction electrons are produced that pass through an external circuit before it is being used by the reduction reaction.

During a redox reaction, a chemical reaction allows the electrical energy to use as an end product. Galvanic cells convert chemical energy into electrical energy. it has power that separate electrons flow through the cycle of oxidation and reduction, producing a half-reaction and connecting both to a wire then a path may be created for the electrons to flow across that wire. this type of electron flows is called a current.

It may be composed of any two metals i.e. cathode and anode. In galvanic cells, The cathode is an electrode in an electrochemical cell at which reduction occurs. while The anode is an electrode in an electrochemical cell at which oxidation occurs;

Electrolytic Cells

Electrolytic cells are similar to galvanic cells. it requires a salt bridge. Non-spontaneous redox reactions occur in these cells that convert electric energy into chemical energy. In electrolytic cells, electrical energy is produced through chemical reactions with the help of external resources.

Cathode and anode are two electrodes in addition to the flow of electrons. Electrolytic cells are important as they are the basis of batteries that are fuel modern society. The reverse reactions in each case are non-spontaneous and require electrical energy to occur.

The electrolysis process refers to the decomposition of an element that is provided under the influence of an electric current. Sir Humphrey Davey was the first who conducted electrolysis in 1808. In this process, electrical energy must be added to the redox reaction.

Electrolytic cells, unlike galvanic cells, need two metals to be positioned in the same container. the positive electrode is considered an anode in this case, and the cathode is considered a negative electrode. the anode is responsible for the oxidation process and the cathode is responsible for the reduction process.

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