Applications of Lechatelier’s Principle
Autor: Rachel • December 19, 2017 • 779 Words (4 Pages) • 626 Views
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reactants.
5. Adding the Fe3+ caused the color of the solution to become a darker red/burgundy and adding SCN- caused the color of the solution to become lighter and closer to clear. Thus, the amount of products increased. Both reactants are included because products were formed from both reactants.
6. When the solution was cooled or heated, the color change was barely noticeable. It was a clear color. However there were precipitates. This shows that the reaction can go forward or backward. The increase and decrease in product showed an increase in the forward/reverse reaction rate.
7. The reaction is exothermic.
Fe3+(aq) + SCN–(aq) ←→ FeSCN2+(aq) + Heat
Conclusion:
After analyzing the results of the experiment, it was concluded that Le Chatelier’s principle perfectly explains the observations of the shifts in equilibrium of the reaction as the system is subjected to various stresses. The lab was performed to observe the changes in the reaction at equilibrium as the concentration and temperature were taken into account. The observed change in color shows whether the reactants or products being favored. The potassium and nitrate ions did not have a role in the reaction at equilibrium. It showed no change in the color of the reaction. The SCN- and Fe3+ ions were part of the overall equilibrium equation because it changed the color of the solution to a darker red color. This shows the forward rate of the reaction. The H2PO4– ion lightened the color of the solution. This shows the reverse rate of the reaction in action. These shifts in equilibrium are explained in Le Chatelier’s principle, which states that a reaction will shift either right or left to address the stress and restore equilibrium. When the temperature was increased, the system shifted right to favor the products and when the temperature was decreased, it shifted left to favor the reactants. However, during the lab, the color change during equilibrium was barely noticeable. Only the precipitate was observed changing. The amount of time in the hot and ice bath could have been extended to show clearer results. The various stresses the system was subjected to resulted in shifts of equilibrium, which is stated in Le Chatelier’s principle.
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