![]() Before adding heat we observed that the color given off from the solution was light blue while heating the solution it was turn a darker blue. The Le Principle (LCP) was observed through adding more concentration to a solution which determined the establishment of the shift and even with part four we used heat to shift the equilibriums. Data: seen in in lab report data collecting Conclusion: In conclusion the equilibrium shifts we observed through color change and precipitation. Carefully add concentrated HCl (aq) to the solution in the test tube until a distinct change occurs. Place 3 mL of saturated NaCl (aq) into a small test tube. Procedure: PART 1: SATURATED SODIUM CHLORIDE SOLUTION 1. The shifts can only be explained examining effects of the applied stress from Le Principle. Thiocyanate Solution (aq) (aq) (aq) Yellow Colorless Deep Red observing their color changes and precipitation formation, we were able to determine the direction of the shift. Cobalt(II) Chloride Solution (aq) 4 (aq) CoCl42 (aq) 6 H2O (l) Pink Blue 5. Aqueous Ammonia Solution (with phenolphthalein) NH3 (aq) H2O (l) (aq) (aq) Colorless Pink 4. Acidified Chromate Solution 2 (aq) 2 (aq) Cr2O7 (aq) H2O (l) Yellow Orange 3. Saturated Sodium Chloride Solution NaCl (s) (aq) (aq) 2. Their equilibrium systems can observed below. The systems studied are known as saturated Sodium Chloride solution, acidified Chromate solution, aqueous Ammonia solution (with phenolphthalein), Cobalt (II) Chloride solution, and Iron solution. Exothermic: A B C D heat Endothermic: A B heat C D In this lab we studied the effect of applying stresses to five equilibrium systems. An exothermic and endothermic reaction can be seen below. In an exothermic reaction, heat energy is released and can be considered a product, while in endothermic reactions, heat energy is absorbed and is considered a reactant. ![]() ![]() The direction of the shift largely depends whether the reaction is exothermic and endothermic. Another factor that affects the reversible reaction at equilibrium and acts upon the Le Principle is a change in temperature. Decreasing the concentration of C or D can cause a shift to the right. Decreasing the concentration of A or B can cause a shift to the left. Increasing the concentration of C or D can cause a shift to the left. For example: Increasing the concentration of A or B can cause a shift to the right. Considering the reversible reaction at equilibrium: A B C D, changing the concentration for any of these lettered solutions can change the system to no longer be at equilibrium. When a stress like this is applied, the reversible reaction will shift to reestablish the equilibrium known as Le Principle. A stress in a reversible reaction can be known as increasing or decreasing a chemical concentration or a temperature change. Reversible reaction: A reversible equation at equilibrium can be disturbed if a stress was applied. A reversible reaction is known when the of products to reactants and reactants to products, occur simultaneously. Introduction: In this lab we performed five different experiments that involved a reversible reaction. ![]() Preview text Veena Aruldhas CHEM 132 Professor Teklai Lab Partner: Jason Marlin Le Principle Objective: To observe the effect of an applied stress on chemical system at equilibrium.
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