Joseph gay lussac timeline

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Joseph Louis Gay-Lussac December 6, — May 9, was a French chemist and physicist whose discovery of the law of combining volumes of gases in chemical reactions paved the way for our understanding of molecules and atoms. He also demonstrated that different gases expand at the same rate when subject to an increase in temperature at constant pressure. He was a co-discoverer of the element boron. His work demonstrated his talent for uncovering the principles that underlie outward phenomena, and it had a lasting effect on the history of chemistry and physics.
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Joseph Gay-Lussac

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Gay-Lussac, Joseph Louis | Article about Gay-Lussac, Joseph Louis by The Free Dictionary

Joseph Louis Gay-Lussac began his career in by very carefully showing the validity of Charles' law for a number of different gases. Gay-Lussac's most important contributions to the study of gases, however, were experiments he performed on the ratio of the volumes of gases involved in a chemical reaction. Gay-Lussac studied the volume of gases consumed or produced in a chemical reaction because he was interested in the reaction between hydrogen and oxygen to form water. He argued that measurements of the weights of hydrogen and oxygen consumed in this reaction could be influenced by the moisture present in the reaction flask, but this moisture would not affect the volumes of hydrogen and oxygen gases consumed in the reaction.
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Joseph-Louis Gay-Lussac: Ideal Gas Law

Gay-Lussac's law more correctly referred to as Amonton's law states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas when the volume is kept constant. It is a special case of the ideal gas law. Gay-Lussac is incorrectly recognized for the Pressure Law which established that the pressure of an enclosed gas is directly proportional to its temperature and which he was the first to formulate c. These laws are also known variously as the Pressure Law or Amontons's law and Dalton's law respectively.
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In Avogadro put forward a hypothesis that was neglected by his contemporaries for years. Avogadro, however, saw it as the key to a better understanding of molecular constituency. In Avogadro hypothesized that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. From this hypothesis it followed that relative molecular weights of any two gases are the same as the ratio of the densities of the two gases under the same conditions of temperature and pressure. Avogadro also astutely reasoned that simple gases were not formed of solitary atoms but were instead compound molecules of two or more atoms.
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