Daniell, John Frederic

Holze R (2008) Daniell, John Frederic, Daniell cell. In Bard AJ, hizelt G, Scholz F (eds) Electrochmiical dictionary. Springer, Berlin, p 136... 

The Daniell cell is named after its inventor, the English chemist John Frederic Daniell (1790-1845). In the photograph shown here, the zinc sulfate solution is placed inside a porous cup, which is placed in a larger container of copper sulfate solution. The cup acts as the porous barrier. 

John Frederic Daniell started some experiments to improve the behavior of the voltaic pile. The use of the voltaic pile was limited because it was not able to sustain a constant current for a certain period of time. The problem was due to the polarization of the cell. In 1836, Daniell improved the voltaic cell by solving the polarization problem. He invented a cell in which hydrogen was eliminated through the generation... 

Write an article about the development and uses for the Daniell cell, an early battery made in 1836 by John Frederic Daniell of Great Britain. Find out how it improved on the Volta cell and whether or not this type of battery is used much today. 

A simple example of an electrochemical cell is the Daniell cell, named after the English chemist John Frederic Daniell (1790-1845). This apparatus, illustrated in Figure 8.1, consists of a zinc electrode immersed in a zinc sulfate solution and a copper electrode immersed in a cupric sulfate solution. The two solutions are separated by a porous partition which is of such a nature that it prevents the bulk mixing of the solutions but allows ions to pass through as the cell operates. The emf developed in the Daniell cell depends upon the concentrations of and Cu " ions in the two solutions. If the concentrations of the two solutions are both one mola (1 m), the cell is called a standard cell. 

The cell is named for the British chemist and meteorologist John Frederic Daniell (1790-1845). 

John Frederic Daniell (London 12 March 1790-13 March 1845) was at first engaged in a sugar refinery and in a resin factory. He heard Brande s lectures on chemistry and then took up research. He became F.R.S. in 1813, was Copley medallist in 1838, and in 1831 he was appointed professor of chemistry in King s College, London. He was a friend and admirer of Faraday. His book is dedicated to Faraday, in deference to whom Dalton s atomic theory is in both editions explained only at the end as best kept out of sight in the first... 

Take a look at Figure 9-1, which shows a Daniell cell that uses the Zn/Cu reaction to produce electricity. (This cell is named after John Frederic Daniell, the British chemist who invented it in 1836.)... 

John Frederic Daniell (1790-1845). English chemist and meteorologist. In addition to invention of the Daniell cell, an improvement over Volta s electric pile, Daniell made contributions to instrumental meteorology through his invention of a dew-point hygrometer that became a standard instrument for measuring relative humidity. 

Mertyns, Joost. From the Lecture Room to the Workshop John Frederic Daniell, the Constant Battery and Electrometallurgy Around 1840. Annals of Science 5b, no. 3 (July, 1998) 241-261. Early developments in batteries, electroplating, and electroforming are described. 

DanieU cell (John Frederic DanieU) Daniell invents the electric battery bearing his name, which is much improved over the voltaic pile. 

John Frederic Daniell (1790-1845) was an English scientist who is well known for his invention of the Daniell cell, which is one of the earliest prototypes of electric batteries. The Daniell cell consists of two metal, copper and zinc, electrodes and is a classical electrochemical system conunonly used in electrochemical education. 

In an electrochemical system with phases a and p, the criterion of equilibrium should be modified due to different electric potentials cp and respectively, in phases a and p. As an example, let us consider zinc electrode of the Daniell cell, which was introduced by John Frederic Daniell in 1836. Think of a piece of zinc metal being dipped into a dilute solution of ZnS04(aq). Between the solution and metal phases, aqueous zinc ions, Zn +(aq), can be transferred. If the initial solution is extremely dilute, then the rate of transfer of ions from the metal to the solution is faster than the transfer from the solution to the metal. When Ztf+(aq) leaves the metal surface, electrons are left behind because they cannot enter the solution. This builds up a negative electric potential in the metal phase. After some time, an equilibrium state is reached between the so-called electrochemical potential of Zn +(aq) within the metal and solution phases. The electrochemical potential of the species in each phase comprises two components (1) the chemical potential of the species p, and (2) the electric... 

John Frederic Daniell, British chemist and meteorologist the DanieU cell, which consisted of a copper pot filled with a copper sulfete solution, in which was immersed an unglazed earthenware container filled with sulfuric acid and a zinc electrode. 

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