Le Chatelier's Principle

Le Chatelier’s Principle in iron Thiocyanate Equilibrium
Purpose
The general rule that is used to predict the direction in which the equilibrium will shift is known as Le Chatelier’s Principle. It is stated as if any external stress like changing concentration volume or temperature is applied to the equilibrium, than the system has the property to adjust itself to partially offset the stress.
Chemical equilibrium represents that the forward and reverse reaction are balanced to maintained this balance so as to keep the reaction at equilibrium state Le Chatelier’s principle play an important role. It shifts the equilibrium in such a way that according to the stress, products either increase or decrease. In this experiment, we are going to prepare an equilibrium system for the following reaction;
We are going to study the responses and changes that it have on application of any external stress and using Le Chatelier’s Principle, explaining the results.
Procedure
Into a clean 400 mL beaker add 125 mL of deionized water 10 drops of 1 M KSCN and 10 drops of 1 M F e (NO3) solution. This stock solution will have an intense red color due to the formation of the complex FeSCN2+. Obtain 10 clean medium sized test tubes and labeled them 1 through 10. Add 10 mL of this stock solution into each one of the test tubes. Keep test tube 1 as a control and add the following reagent into test tubes through 2 to 9.
Cover each test tube with parafilm and shake to mix. Heat test tube 10 in a hot water bath. Then compare the color intensity of watch of the test tubes with that of the control test tube 1. The test tube with the darkest color has the highest concentration of Fe SCN2+. In each test record your observations and explain the results in terms of Le Chatelier’s principle.
Table 14.1 Complexes and principle
Pre Lab
      Kc = [CoCl42-]     [Co2+] [Cl-]4
If concentration of Co2+ increases the equilibrium will shift toward Right.
  Increasing the...