How chemical reactions can be harnessed to generate electrical power
In short: At its core, electrochemistry explores the profound connection between electricity and chemical change. While some chemical reactions occur spontaneously, releasing energy, others can be driven by electricity. This fundamental relationship is what allows us to power everything from portable batteries to complex industrial processes.
Electrochemistry is the branch of chemistry dedicated to the relationship between electricity and chemical change. Many chemical reactions occur spontaneously, liberating electrical energy in the process. These specific reactions are the driving force behind the operation of batteries and fuel cells, which convert chemical energy into usable electric power.
To measure the tendency of different chemical species to gain or lose electrons—a process known as reduction or oxidation—scientists use the electromotive series. This series ranks atoms, molecules, and ions based on their reduction potential, expressed in volts. This measurement is standardized by using a hydrogen electrode as a reference point, which is arbitrarily assigned a voltage of zero.
Under standard conditions, this hydrogen electrode maintains a concentration of one mole per litre of hydrogen ions (H+) in equilibrium with hydrogen gas (H2) at a pressure of one atmosphere and a temperature of 25°C (77°F). By combining half-reactions, chemists can determine the potential of a complete reaction. For instance, the reaction between copper and zinc can be expressed as Cu2+ + Zn ⇌ Cu + Zn2+, which has a potential of -1.10 volts.
According to the 1953 convention, a negative voltage value indicates that a reaction proceeds spontaneously from left to right. Regarding the copper-zinc case, this implies that zinc metal reacts naturally within copper(II) ion solutions, producing copper metal alongside zinc(II) ions. This field also encompasses electrolysis, where electricity is used to drive non-spontaneous reactions, and electroplating.
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Sources
- Summary by Intellect · source: Electrochemistry: Crash Course Chemistry #36
- Also: Electrochemistry | Electrolysis, Redox Reactions & Corrosion | Britannica
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