Le Chatelier Principle

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Le Chatelier’s Principles
Henri Louis Chatelier, born on the 8th of October 1850 in Paris, France to Louis Le Chatelier and Louise Durand. He was the eldest son in a family of six kids and often times had to take on the responsibility of caring after them. As he was born into a middle class Roman Catholic family, he received the opportunity to attend a more privileged school compared to most other kids in his time. Therefore during his early years, Henri received the opportunity to attend the College Rollin in Paris, France from which he graduated in 1868 at the age of 18 with an undergraduate degree. His father being a very influential figure in the materials engineering world, having helped lay ground for the aluminum industry in France, as well as improve the processes of manufacturing and developing both iron and steel lead Henri to follow in his father’s footsteps. He enrolled into the Ecole Polytechnique on the 25th of October 1869, yet after only a year of schooling himself and his peers were recruited to the French army. Le Chatelier became a second lieutenant and not too long after took part in the Siege of Paris, fighting for the French. After his return he proceeded to move into L’Ecole des Mines in Paris, which he attended until his graduation in 1873. Three years later he married a friend of the family Geneviève Nicolas, with which he had seven children. Despite his teachings as an engineer and extensive background in the industrial sector, he chose to teach chemistry after finding that working as a mining engineer in the province was not all he thought it would be. In 1877 he returned to the Ecole des Mines so he may teach chemistry and in 1887 became appointed the head of general chemistry at the Ecole de...

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...d more nitric acid to fill what had been taken out.
If the pressure of the whole system is increased due to a deceased in the volume of the reaction vessel then the equilibrium of the reaction will shift towards the left. Because based on Le Chateliers principle if there is an increase in pressure then the equilibrium shifts towards the side which would produce a lower number of particles. In this case that side would be the left as the total number of moles for the reactants is six compared to ten on the product side.
If argon gas is added to the system without changing the volume of the reaction vessel then the equilibrium of the system will not be effected in any way. Because argon is a noble (Inert) gas it does not react with anything, so it will not change anything within the reaction itself. Allowing it to continue on as it was before the addition.

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