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The Chemical History of a Candle was the title of a series of six lectures on the chemistry and physics of flames given by Michael Faraday at the Royal Institution in 1848, as part of the series of Christmas lectures for young people founded by Faraday in 1825 and still given there every year.
A close-up image of a candle showing the wick and the various parts of the flame; Michael Faraday lectured on "The Chemical History of a Candle".The Royal Institution's Christmas Lectures were first held in 1825, [2] and have continued on an annual basis since then except for four years during the Second World War. [3]
Michael Faraday (/ ˈ f ær ə d eɪ,-d i /; 22 September 1791 – 25 August 1867) was an English physicist and chemist who contributed to the study of electromagnetism and electrochemistry.
The Faraday Lectureship Prize, previously known simply as the Faraday Lectureship, is awarded once every two years (approximately) by the Royal Society of Chemistry for "exceptional contributions to physical or theoretical chemistry". [1] Named after Michael Faraday, the first Faraday Lecture was given in 1869, two years after Faraday's death ...
Michael Faraday was another early worker, whose major contribution to chemistry was electrochemistry, in which (among other things) a certain quantity of electricity during electrolysis or electrodeposition of metals was shown to be associated with certain quantities of chemical elements, and fixed quantities of the elements therefore with each ...
In the early 1830s, Michael Faraday laid the foundations of electrochemistry and solid-state ionics by discovering the motion of ions in liquid and solid electrolytes. Earlier, around 1800, Alessandro Volta used a liquid electrolyte in his voltaic pile , the first electrochemical battery, but failed to realize that ions are involved in the process.
Michael Faraday Announced his important law of electrochemical equivalents, viz.: "The same quantity of electricity—that is, the same electric current—decomposes chemically equivalent quantities of all the bodies which it traverses; hence the weights of elements separated in these electrolytes are to each other as their chemical equivalents."
For Faraday's first law, M, F, v are constants; thus, the larger the value of Q, the larger m will be. For Faraday's second law, Q, F, v are constants; thus, the larger the value of (equivalent weight), the larger m will be. In the simple case of constant-current electrolysis, Q = It, leading to