Jacobus Henricus van 't Hoff in the context of "Arrhenius equation"


Jacobus Henricus van 't Hoff in the context of "Arrhenius equation"

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⭐ Core Definition: Jacobus Henricus van 't Hoff

Jacobus Henricus van 't Hoff Jr. (Dutch: [vɑn (ə)t ˈɦɔf]; 30 August 1852 – 1 March 1911) was a Dutch physical chemist. A highly influential theoretical chemist of his time, Van 't Hoff was the first winner of the Nobel Prize in Chemistry. His pioneering work helped found the modern theory of chemical affinity, chemical equilibrium, chemical kinetics, and chemical thermodynamics. In his 1874 pamphlet, Van 't Hoff formulated the theory of the tetrahedral carbon atom and laid the foundations of stereochemistry. In 1875, he predicted the correct structures of allenes and cumulenes as well as their axial chirality. He is also widely considered one of the founders of physical chemistry as the discipline is known today.

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👉 Jacobus Henricus van 't Hoff in the context of Arrhenius equation

In physical chemistry, the Arrhenius equation is a formula for the temperature dependence of reaction rates. The equation was proposed by Svante Arrhenius in 1889 on the basis of the work of Dutch chemist Jacobus Henricus van 't Hoff, who had noted in 1884 that the Van 't Hoff equation for the temperature dependence of equilibrium constants suggests such a formula for the rates of both forward and reverse reactions. This equation has a vast and important application in determining the rate of chemical reactions and for calculation of energy of activation. Arrhenius provided a physical justification and interpretation for the formula. Currently, it is best seen as an empirical relationship. It can be used to model the temperature variation of diffusion coefficients, population of crystal vacancies, creep rates, and many other thermally induced processes and reactions. The Eyring equation, developed in 1935, also expresses the relationship between rate and energy.

The temperature dependence arises because a greater fraction of molecular collisions have sufficient energy to exceed the activation barrier as temperature increases.

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