Amedeo Avogadro Contribution To Chemistry



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Not much is known about the infamous Avogadro besides his contributions to Chemistry and Physics. Avogadro was born on August 9th, 1776 as the son of the Count of Quaregna (a title he later inherited). Avogadro spent most of his life in his hometown of Turin, Italy. He later became a professor at the Turin University. Avogadro had six children with a loving wife, and was a strong religious man. He was said to be liked by his students because of his sense of humor also. Avogadro started college when he was only 13, and graduated when he was 16. Avogadro received his doctorates in ecclesiastical law (law pertaining to the church) at the ripe age of 20. Following that, he began to practice law. Although Amedeo Avogadro was destined to become a lawyer, his main interests changed to chemistry, mathematics, and physics.

In the year 1800, Avogadro began his private studies in Physics and Mathematics. In his free time he did a lot of reading and had a complete set of the current scientific journals in his library printed in four

different languages. In one of these journals he read in 1808 that Joseph Louis Gay-Lussac, “Had found that when two gasses react together to form different products, the volumes of the reactants and the products (if they are all still gasses) are all whole numbers.” This accepted belief was called the Law of Combining Volumes. Avogadro then thought, hey, this must mean that equal amounts of gas at the same temperature and pressure must contain the same amount of molecules. He knew that when two volumes of Hydrogen and one volume of oxygen were reacted it formed two volumes of water vapor. Why two and not one? Avogadro’s answer was that it must mean that sets of two oxygen atoms were used to create the one volume of oxygen he used. After noticing this, Avogadro was able to see that, “Molecular weights of any set of gasses are the same as the ratio of the densities to those gasses under the same conditions of temperature and pressure.” His conclusion was that, “All gasses, simple or complex, contain the same number of molecules under the same conditions of temperature and pressure.” This idea is one of the main points in Chemistry. Although Avogadro did not literally find the unit of Moles (6.02 x 10^23 molecules), the number is called Avogadro’s Number in honor of his theories that led future scientists to be able to calculate this number.

The impact of this amazing realization is still spreading today. Avogadro’s law is used in thousands of different applications each and every day; from a high school chemistry I class, to scientists trying to figure out the cure to cancer. This number, and law is used to find the outcome of a reaction before it is even attempted, and is the basis of many theoretical chemistry and physics ideas. Although the applications for this are limited to chemical equations and the such, the combinations are endless, straying into the realm of the chemistry of DNA and other complicated molecular structures. We are only beginning to use this law to its full extent, and we will continue to broaden its impact by using it more.

Amedeo Avogadro. If you were to sit in a chemistry class you wouldn't get very far without using Avogadro's number. Avogadro's number equals 6.02 x 10^23. Lorenzo Romano Amedeo Carlo Avogadro, Count of Quaregna and Cerreto was an Italian sciNew content will be added above the current area of focus upon selectionLorenzo Romano Amedeo Carlo Avogadro, Count of Quaregna and Cerreto was an Italian scientist, most noted for his contribution to molecular theory now known as Avogadro's law, which states that equal volumes of gases under the.

The name of Italian scientist Amedeo Avogadro (1776–1856) is associated with two fundamental laws in chemistry. The first states that 1 mol of every gas occupies 22.4 l at standard temperature and pressure; the second affirms that 1 mol of every substance has the same number of molecules (6.02 × 10 23), a value referred to as Avogadro's number.We examine how these principles came to be. Physical science: Chemistry as 1811 the Italian physicist Amedeo Avogadro was able to reconcile Dalton’s atomic theory with Gay-Lussac’s volumetric law by postulating that Dalton’s atoms were indeed compound atoms, or polyatomic. Footnote: Avogadro's name is best known to today's students of chemistry because of the Avogadro constant, also known as Avogadro's number. Jean Perrin named the number of molecules in a mole (or gram-mole as it was called at the time)in honor of Avogadro early in the 20thcentury. Avogadro did not determine this number.

Amedeo Avogadro was a bright man who stumbled upon a question chemists had encountered for years and somehow, with some great brain power, found the answer. The only dilemma with this historic find was that Avogadro’s life was, for the most part, isolated from other scientists. This was one of the main reasons why his theory did not catch on quickly. In fact, it was not until 1858 when the significance of Avogadro’s work was realized. When Italian chemist Stanislao Cannizzaro explained why Avogadro’s law did not always hold true in some rare instances, Avogadro’s hypothesis finally became the accepted theory at the time.

Lorenzo Romano Amedeo Carlo Avogadro di Quaregna e di Cerreto,[1] Count of Quaregna and Cerreto (9 August 1776, Turin, Piedmont – 9 July 1856) was an Italian savant. He is most noted for his contributions to molecular theory, including what is known as Avogadro's law. In tribute to him, the number of elementary entities (atoms, molecules, ions or other particles) in 1 mole of a substance, 6.02214179(30)×1023, is known as the Avogadro constant.

Amedeo Avogadro

Biography

Amedeo Carlo Avogadro was born in Turin, Italy in 1776 to a noble family of Piedmont, Italy.

He graduated in ecclesiastical law at the early age of 20 and began to practice. Soon after, he dedicated himself to physics and mathematics (then called positive philosophy), and in 1809 started teaching them at a liceo (high school) in Vercelli, where his family had property.

Amedeo avogadro atomic theory

In 1811, he published an article with the title Essai d'une manière de déterminer les masses relatives des molécules élémentaires des corps, et les proportions selon lesquelles elles entrent dans ces combinaisons ('Essay on Determining the Relative Masses of the Elementary Molecules of Bodies and the Proportions by Which They Enter These Combinations'), which contains Avogadro's hypothesis. Avogadro submitted this essay to a French journal, De Lamétherie's Journal de Physique, de Chimie et d'Histoire naturelle (Journal of Physics, Chemistry and Natural History) so it was written in French, not Italian. (Note: In 1811, northern Italy was under the rule of the French Emperor Napoléon Bonaparte.)

In 1820, he became professor of physics at the University of Turin. After the downfall of Napoléon in 1815, northern Italy came under control of this kingdom.

He was active in the revolutionary movements of 1821 against the king of Sardinia (who became ruler of Piedmont with Turin as his capital). As a result, he lost his chair in 1823 (or the university officially declared, it was 'very glad to allow this interesting scientist to take a rest from heavy teaching duties, in order to be able to give better attention to his researches').[2]

Eventually, Charles Albert granted a Constitution (Statuto Albertino) in 1848. Well before this, Avogadro had been recalled to the university in Turin in 1833, where he taught for another twenty years.

Little is known about Avogadro's private life, which appears to have been sober and religious. He married Felicita Mazzé and had six children.

Amedeo Avogadro Contribution To Chemistry Pdf

Some historians suggest that he sponsored some Sardinian revolutionaries, who were stopped by the announcement of Charles Albert's constitution.

Avogadro held posts dealing with statistics, meteorology, and weights and measures (he introduced the metric system into Piedmont) and was a member of the Royal Superior Council on Public Instruction.

In honor of Avogadro's contributions to molecular theory, the number of molecules in one mole was named Avogadro's number, NA or 'Avogadro's constant'. It is approximately 6.0221415 × 1023. Avogadro's number is used to compute the results of chemical reactions. It allows chemists to determine amounts of substances produced in a given reaction to a great degree of accuracy.

Amedeo Avogadro Contribution To Chemistry Journal

Johann Josef Loschmidt first calculated the value of Avogadro's number, often referred to as the Loschmidt number in German-speaking countries (Loschmidt constant now has another meaning).
Accomplishments

Avogadro's Law states that the relationship between the masses of the same volume of different gases (at the same temperature and pressure) corresponds to the relationship between their respective molecular weights. Hence, the relative molecular mass of a gas can be calculated from the mass of sample of known volume.

Books Amedeo Avogadro

Avogadro developed this hypothesis after Joseph Louis Gay-Lussac had published in 1808 his law on volumes (and combining gases). The greatest problem Avogadro had to resolve was the confusion at that time regarding atoms and molecules. One of his most important contributions was clearly distinguishing one from the other, stating that gases are composed of molecules, and these molecules are composed of atoms. For instance, John Dalton did not consider this possibility. Avogadro did not actually use the word 'atom' as the words 'atom' and 'molecule' were used almost without difference. He believed that there were three kinds of 'molecules,' including an 'elementary molecule' (our 'atom'). Also, more attention was given to the definition of mass, as distinguished from weight.

In 1815, he published Mémoire sur les masses relatives des molécules des corps simples, ou densités présumées de leur gaz, et sur la constitution de quelques-uns de leur composés, pour servir de suite à l'Essai sur le même sujet, publié dans le Journal de Physique, juillet 1811 ('Note on the Relative Masses of Elementary Molecules, or Suggested Densities of Their Gases, and on the Constituents of Some of Their Compounds, As a Follow-up to the Essay on the Same Subject, Published in the Journal of Physics, July 1811') ([1]), about gas densities.

In 1821 he published another paper, Nouvelles considérations sur la théorie des proportions déterminées dans les combinaisons, et sur la détermination des masses des molécules des corps (New Considerations on the Theory of Proportions Determined in Combinations, and on Determination of the Masses of Atoms) and shortly afterwards, Mémoire sur la manière de ramener les composès organiques aux lois ordinaires des proportions déterminées (Note on the Manner of Finding the Organic Composition by the Ordinary Laws of Determined Proportions).

In 1841, he published his work in Fisica dei corpi ponderabili, ossia Trattato della costituzione materiale de' corpi, 4 volumes.
Response to the theory

The scientific community did not give great attention to his theory, so Avogadro's hypothesis was not immediately accepted. André-Marie Ampère achieved the same results three years later by another method (in his Sur la détermination des proportions dans lesquelles les corps se combinent d'après le nombre et la disposition respective des molécules dont leurs particules intégrantes sont composées -- On the Determination of Proportions in which Bodies Combine According to the Number and the Respective Disposition of the Molecules by Which Their Integral Particles Are Made), but the same indifference was shown to his theory as well.

Only through studies by Charles Frédéric Gerhardt and Auguste Laurent on organic chemistry was it possible to demonstrate that Avogadro's law explained why the same quantities of molecules in a gas have the same volume.

Unfortunately, related experiments with some inorganic substances showed seeming exceptions to the law. This was finally resolved by Stanislao Cannizzaro, as announced at Karlsruhe Congress in 1860, four years after Avogadro's death. He explained that these exceptions were due to molecular dissociations at certain temperatures, and that Avogadro's law determined not only molecular masses, but atomic masses as well.

In 1911, a meeting in Turin commemorated the hundredth anniversary of the publication of Avogadro's classic 1811 paper. King Victor Emmanuel III attended. Thus, Avogadro's great contribution to chemistry was recognized.

Rudolf Clausius, with his kinetic theory on gases, gave another confirmation of Avogadro's Law. Jacobus Henricus van 't Hoff showed that Avogadro's theory also held in dilute solutions.

Avogadro is hailed as a founder of the atomic-molecular theory.
See also
Wikisource has the text of the 1911 Encyclopædia Britannica article Avogadro, Amedeo, Conte di Quaregna.

Avogadro (lunar crater)
Avogadro's constant

References

Electrax crack mac. ^ Guareschi, Icilio (1911), 'Amedeo Avogadro e la sua opera scientifica', Opere scelte di Amedeo Avogadro, Turin: Accademia delle scienze, pp. i–cxl.
^ Link to page at the University of Piedmont in Italy

Further reading

What Did Amedeo Avogadro Discover

Hinshelwood, C. N.; Pauling, L. (1956), 'Amedeo Avogadro', Science 124 (3225): 708–713, 1956 Oct 19, doi:10.1126/science.124.3225.708, PMID 17757602
Cavanna, D. (1956), 'Centenary of the death of Amedeo Avogadro', Minerva farmaceutica 5 (6): 134–7, 1956 Jun, PMID 13369233
Crosland, M. P. (1970), Avogadro, Amedeo, 1, New York: Charles Scribner's Sons, pp. 343–350, ISBN 0-684-10114-9.
Morselli, Mario. (1984). Amedeo Avogadro, a Scientific Biography. Kluwer. ISBN 90-277-1624-2.

Amedeo Avogadro Invention

Review of Morselli's book: Pierson, S. (1984), 'Avogadro and His Work: Amedeo Avogadro', Science 226 (4673): 432–433, 1984 Oct 26, doi:10.1126/science.226.4673.432, PMID 17799933

Amedeo Avogadro's Contribution To Chemistry

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