Equilibrium Reactions and Le Chatelier's Principle
Lab: 5
Experiment:13
Pre-Lab The purpose of this experiment is to observe an equilibrium reaction counteracting changes to it’s system all in accordance to Le Chatelier’s principle. An equilibrium reaction can be pushed toward products or reactant based on changes in temperature or concentration. The reversibility of reaction will also be looked at.
Pre-Lab questions
1. The concentrations of products and concentrations of reactants remain constant but both reactions are still going on, just at the same rate.
2. Le Chatelier’s principle when an equilibrium has been established in a system and is altered, the systems will counteract the change.
3. a) it will go to the left b) to the left c) to the right
4. Remove the CO2 gas being produced
5. concentrations and totals in equilibrium change over time.
6.
a) The solution will be yellow. K2CrO4 ( K2+(aq) + CrO42-(aq) b) The solution will be orange. The hydrogen ion will react with chromate to form an equilibrium and produce some dichromate and water. This reaction will cause the amount of chromate to decrease in order to form more products and the equilibrium will shift to the right. c) The NaOH, specifically the hydroxide, would react with the dichromate and push the equilibrium toward reactants. This would increase the amount of reactants and decrease the amount of dichromate being formed in the equilibrium. The solution would be yellow because there would be more chromate.
7. The common ion effect is the amount of dissociation a weak electrolyte undergoes with a common ion is reduced.
Review Questions Complete questions # 1 - #4 1. The equilibrium would shift towards the right and the color of the solution would be orange. 2. The equilibrium would shift to the left. More acetate ion has been added to the equilibrium already containing this ion
Experiment:13
Pre-Lab The purpose of this experiment is to observe an equilibrium reaction counteracting changes to it’s system all in accordance to Le Chatelier’s principle. An equilibrium reaction can be pushed toward products or reactant based on changes in temperature or concentration. The reversibility of reaction will also be looked at.
Pre-Lab questions
1. The concentrations of products and concentrations of reactants remain constant but both reactions are still going on, just at the same rate.
2. Le Chatelier’s principle when an equilibrium has been established in a system and is altered, the systems will counteract the change.
3. a) it will go to the left b) to the left c) to the right
4. Remove the CO2 gas being produced
5. concentrations and totals in equilibrium change over time.
6.
a) The solution will be yellow. K2CrO4 ( K2+(aq) + CrO42-(aq) b) The solution will be orange. The hydrogen ion will react with chromate to form an equilibrium and produce some dichromate and water. This reaction will cause the amount of chromate to decrease in order to form more products and the equilibrium will shift to the right. c) The NaOH, specifically the hydroxide, would react with the dichromate and push the equilibrium toward reactants. This would increase the amount of reactants and decrease the amount of dichromate being formed in the equilibrium. The solution would be yellow because there would be more chromate.
7. The common ion effect is the amount of dissociation a weak electrolyte undergoes with a common ion is reduced.
Review Questions Complete questions # 1 - #4 1. The equilibrium would shift towards the right and the color of the solution would be orange. 2. The equilibrium would shift to the left. More acetate ion has been added to the equilibrium already containing this ion