Le Châteliere’s principle report
Abstract
The principle of Le Châteliere is a qualitative principle which consists in the modification of variables such as the pressure, temperature, concentration and volume that is based on the modification of a system in equilibrium this will return to be adjusted so that this modification is canceled and returned again to theBalance. With the experiment of and demonstrated the principle Châteliere when performing the alterations of concentrations adding the drops and in which they will react and produce coloration changes.
Introduction
The chemical balance represents a balance between the reactions to the right and to the left. In most cases this balance is very delicate. Changes in experimental conditions can alter the balance and displace the equilibrium position so that greater or lesser amount of desired product is formed. The variables that can be controlled experimentally are concentration, pressure, volume and temperature. (Chang & Goldsby, 2013)
There is a general rule that helps to predict in which direction a reaction in balance will move when there is a change in concentration, pressure, volume or temperature. This rule, known as the Le Châtelier principle, establishes that if an external disturbance is presented on a equilibrium system, the system will be adjusted in such a way that such disturbance is partially canceled to the extent that the system reaches a new equilibrium position. The term "disturbance" means here a change in concentration, pressure, volume or temperature that alters the equilibrium status of a system. Le Châtelier’s principle is used to assess the effects of such changes. (Chang & Goldsby, 2013)
Materials and methods
Starting from a 50ml solution of potassium dichromate to a 0 dissolution.025 m with a concentration of 0.1 m of potassium chromate we proceed to calculate the volume to prepare the solution.
Once the volume we need to prepare, we begin to extract 12.5 ml with the help of the propipeta and the pipette, followed we place the solution in a precipitation vessel.
Therefore we transfer the 12.5 ml of the capacity ball, distilled water is added until the capacity of the capacity is reached, we cover the ball, stir it, and obtain the prepared solution.
Then, we pour 6ml of the prepared solution in 3 test tubes, numbered from 1 to 3, we proceed to place the tubes in the rack.
Therefore, we collect 6 ml of a prepared potassium chromate solution, numbered from 4 to 6, we traveled to 3 test tubes, and we place it in the rack.
Once the test tubes have already been listed, with the help of a laboratory dropper, we place 10 drops of 1m hydrochloric acid in test tubes 5 and 6.We observe the reaction that is generated.
With the help of a laboratory dropper, we place 10 drops of 1m in test tubes 2 and 3. We observe the reaction that is generated.
With the dropper help we place 10 drops of 1m in test tube 3, and observe the reaction that is generated.
With the dropper help we place 10 drops of 1m in tube 6, and observe the reaction that is generated.
Results and Discussion
Potassium chromate
In test tubes 5 and 6 containing the initial initial session was found with a yellowish coloration by adding the 10 drops of this began to become an orange color.
By adding 10 drops of naoh in tube 6 again becoming the color I had in the beginning in this yellow case.
Potassium dichromate
In test tubes 2 and 3 that contained the initially prepared solution, it was an orange coloration by adding the 10 drops of this began to become a yellow color.
After observing the reactions generated, we return to add 10 drops of in test tube 3.
By adding to the dissolution of this, it would cause the balance to go to the ion (which is what produces the change of orange color.
By adding a strong base as the ion is formed, which is what produces the yellow change.
With this, we verify the catelier’s click in this case the factor that alter was the condition of concentrations this evolved in the sense that it tends to oppose this modification as we observe it in practice.
Conclusions
Once the practice was completed, we could verify that the chemical balance is altered by variables such as the concentration in this case.The increase in concentrations of and in the solutions caused the formation of ions and respectively which causes the color changes in the solutions.
Bibliography
- CHANG, R., & Goldsby, K. (2013). Eleventh chemical edition . In chemistry (p. 646). China: Mc Graw Hill-65, 2013.
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