Is there any example of an example of an electrochemical cell?
An electrolytic cell is an electrochemical cell that drives a non-spontaneous redox reaction through the application of electrical energy.They are often used to decompose chemical compounds, in a process called electrolysis—the Greek word lysis means to break up.Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminum and other chemicals. Electroplating (e.g. of copper, silver, nickel or chromium) is done using an electrolytic cell. Electrolysis is a technique that uses a direct electric current (DC).An electrolytic cell has three component parts:an electrolyte and two electrodes (a cathode and an anode).The electrolyte is usually a solution of water or other solvents in which ions are dissolved.Molten salts such as sodium chloride are also electrolytes.When driven by an external voltage applied to the electrodes, the ions in the electrolyte are attracted to an electrode with the opposite charge, where charge-transferring (also called faradaic or redox) reactions can take place.Only with an external electrical potential (i.e. voltage) of correct polarity and sufficient magnitude can an electrolytic cell decompose a normally stable, or inert chemical compound in the solution. The electrical energy provided can produce a chemical reaction which would not occur spontaneously otherwise.Examples-I. A galvanic cell, or voltaic cell, named after Luigi Galvani, or Alessandro Volta respectively, is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. It generally consists of two different metals connected by a salt bridge or individual half-cells separated by a porous membrane.II. A primary cell is a Galvanic battery that is designed to be used once and discarded, and not recharged with electricity and reused like a secondary cell (rechargeable battery).In general, the electrochemical reaction occurring in the cell is not reversible, rendering the cell un-rechargeable. As a primary cell is used, chemical reactions in the battery use up the chemicals that generate the power; when they are gone, the battery stops producing electricity and is useless.ref.-Electrochemical cell - Wikipedia
Examples of an electrochemical cell?
An electrochemical cell is a device capable of either deriving electrical energy from chemical reactions or facilitating chemical reactions through the introduction of electrical energy. A common example of an electrochemical cell is a standard 1.5-volt "battery".
Give an example of how electrolytic cells are used in industry?
Commercial production of chlorine uses an electrolytic cell and salt water. This is useful for industry because salt water is cheap, and you have to have a feed material that is cheaper than your product (otherwise you won't make money).
Example of how electrolytic cells are applied to life?
The recharging cycle of a battery, electroplating.
What are the effects of electrochemistry in life?
While the effect is hard to discern, electrochemistry plays a major role in many industrial processes that are central to modern life. A non-exhaustive list is given below:Industrial electrolysis (ex. Al, Zn, Ni, Cu, Mg, Cl2, H2 ++)Batteries both primary (single-use) and secondary (ex. rechargeable, Li-ion, Ni-MH, Ni-Cd, Lead-acid)Electroplating (ex. anodic corrosion protection, i.e., Zn sacrificial anode)Electrowinning (ex. purification of Cu)Fuel cells (ex. PEM fuel cell, SOFC, AFC)Electrochemical sensors (ex. penicillin, glucose, CO)Through these examples, it is clear that electrochemistry has a major effect on life.
In an electrochemical cell, why does the cathode gain mass?
The cathode(-) attracts cations(+) & anode(+) attracts anions(-). They are made of carbon.Metal ions are +ve so are attracted by cathode making its mass increase. Oxygen is -ve and is attracted by anode, reacting with the carbon to release carbon dioxide gas, thus decreasing in mass. For more details check electrolysis chapter in 'Federal Chemistry' book by Christopher N. Prescott or any other standard chemistry text books (there are many).