Chemical Equilibrium
Abstract
Chemical equilibrium occurs when a reversible reaction is happening forward and backward, at the same time by the same amount, is equal. Two procedures were made. First is the Effect of Concentration on Equilibrium. The solution became orange when it was diluted with ammonium hydroxide and the solution became yellow when water was added to the solution. In the second, Effect of Temperature on Equilibrium, the solution turned into a light brown gas when it was placed in the refrigerator and turned dark brown when it was warmed.
Introduction Sodium chromate, Na2CrO4, is a crystallized powder or yellow crystals. It is soluble to water. It is toxic by inhalation, ingestion and/or skin contact. It is a strong oxidizer and absorbs moisture from the atmosphere. Sodium chromate can easily convert to sodium dichromate by treating it with an acid [1]. Copper is a soft, orange-brown metal that has been used by humans for years. Copper does not react with most acids. It does react with hot, concentrated sulfuric acid and with nitric acid [1]. Chemical Equilibrium happens when the reactants first comes together, their rate of reaction is determined by their initial concentrations [2]. Even though the reactants are constantly forming products and vice versa, the amount of the reactant and products does become steady. When the net charge is zero, the reaction has reached its equilibrium. When the concentration decreases, so does the reaction rate. But, sometimes there is a reversible reaction which re-forms the reactants. The rates of the forward reaction and reverse reaction become equal, so that the concentration stops changing.
Le Chatelier’s Principle states that a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change [3]. The system adjusts in such a way that the “stress” is partially relieved as it reaches to a new equilibrium. There are three ways that Le Chatelier’s Principle
Chemical equilibrium occurs when a reversible reaction is happening forward and backward, at the same time by the same amount, is equal. Two procedures were made. First is the Effect of Concentration on Equilibrium. The solution became orange when it was diluted with ammonium hydroxide and the solution became yellow when water was added to the solution. In the second, Effect of Temperature on Equilibrium, the solution turned into a light brown gas when it was placed in the refrigerator and turned dark brown when it was warmed.
Introduction Sodium chromate, Na2CrO4, is a crystallized powder or yellow crystals. It is soluble to water. It is toxic by inhalation, ingestion and/or skin contact. It is a strong oxidizer and absorbs moisture from the atmosphere. Sodium chromate can easily convert to sodium dichromate by treating it with an acid [1]. Copper is a soft, orange-brown metal that has been used by humans for years. Copper does not react with most acids. It does react with hot, concentrated sulfuric acid and with nitric acid [1]. Chemical Equilibrium happens when the reactants first comes together, their rate of reaction is determined by their initial concentrations [2]. Even though the reactants are constantly forming products and vice versa, the amount of the reactant and products does become steady. When the net charge is zero, the reaction has reached its equilibrium. When the concentration decreases, so does the reaction rate. But, sometimes there is a reversible reaction which re-forms the reactants. The rates of the forward reaction and reverse reaction become equal, so that the concentration stops changing.
Le Chatelier’s Principle states that a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change [3]. The system adjusts in such a way that the “stress” is partially relieved as it reaches to a new equilibrium. There are three ways that Le Chatelier’s Principle
References: [1] Ebing, Gammon. General Chemistry. 9th Ed. Charles Hartford. 2007 [2] Lodish H, Berk A, Zipursky SL. et. al. Molecular Cell Biology. 4th Ed. NY. W.H.Freeman. 2000 [3]http://www.chm.davidson.edu/vce/equilibria/temperature.html [4]http://www.chemguide.co.uk/physical/equilibria/lechatelier.html