in electrochemical cells two half cells are in contact with each other by
Answers
Answer:
a salt bridge or a electrolyte
Answer:
Salt bridge
An electrochemical cell can be constructed by joining two half-cells together. To maintain the current flow from one cell to the next, a salt bridge is employed to connect those two half-cells. There are numerous varieties of electrochemical cells, and the best option should be chosen based on the situation. When two half-cells are joined to one another, an electrochemical cell will produce a current.
Explanation:
Electrochemical cell:
A device that can either produce electrical energy from chemical reactions or use chemical reactions to generate electrical energy is called an electrochemical cell. Voltaic or galvanic cells are electrochemical devices that produce an electric current, and electrolytic cells are devices that produce chemical reactions, such as electrolysis. (Better source is required) A typical illustration of a galvanic cell is a 1.5-volt consumer-grade cell[3][better source needed]. One or more cells that are connected in parallel, series, or series-and-parallel make up a battery. An electrolytic cell is an electrochemical cell that uses electrical energy to drive a non-spontaneous redox reaction. They are frequently employed in a procedure called electrolysis, from the Greek word lysis, which means to break up, to disintegrate chemical compounds.
The breakdown of water into hydrogen and oxygen, as well as the conversion of bauxite into aluminum and other compounds, are both significant examples of electrolysis. An electrolytic cell is used to conduct electroplating (for instance, of copper, silver, nickel, or chromium). A direct electric current is used in the process known as electrolysis (DC). An electrolyte, two electrodes, and an electrolytic cell make up an electrolytic cell (a cathode and an anode). The electrolyte is often a mixture of ions that have been dissolved in water or another solvent. Electrolytes include molten salts like sodium chloride. The ions in the electrolyte are drawn to an electrode with the opposite charge when an external voltage is supplied to the electrodes, which can then drive charge-transferring (also known as faradaic or redox) reactions. A typically stable or inert chemical substance in the solution can only be broken down by an electrolytic cell with an external electrical potential (i.e. voltage) of the right polarity and sufficient magnitude. Chemical reactions that would not otherwise happen spontaneously can be produced by the electrical energy used.
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