Investigating Chemical Equilibrium Essay

1. The first experiment is Preparation of a Cobalt Amine Bromide Product ; Synthesis #3 was used to create the compound. Added 5 grams of cobalt carbonate to 20 mL of hrdrobromic acid in a beaker. Noticied a slight color change to dark purple. Solution frothed after it settled I mixed in 15mL water and

When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.

The main objective of this experiment is to differentiate between a physical change and a chemical change.

The Vitamin C turned to a red/orange color with no physical/chemical reaction. For the salt the solution turned to an orange color with no physical/chemical reaction. With the Alka-Seltzer, the solution turned to a brown color with no reaction as well. Last but not least, the Baking soda turned to an orange/brown color with no reaction.

between the unknown cation and chlorine (Cl - ) was also formed from the addition of HCl. HCl was

Solub. Or Reaction w/ hot H20: no change observed from the cool water and is soluble

To conclude, the data we have collected from both experiments suggests that Le Chatelier’s principles are applicable and correct. When different substances were added to different solutions, the equilibrium shifted appropriately in order to gain a balance. The shifting of equilibrium resulted in different color changes in different mixtures. In part 2 of the experiment we the aforementioned changes were more easily spotted. We saw the relationship between forward and reverse reactions. When NaOH was added to tube #8 we saw that the color changed from orange into yellow, in order to gain balance but when we added HCl back, the color again changed to orange. Which clearly proved Le Chatelier’s

Endothermic reactions are accompanied by the absorption of heat. The dissolving of ammonium nitrate in water is an example of an endothermic reaction. The solution resulting from this mixture is colder than either the ammonium nitrate or the water. This is the simple explanation of what happens in an instant ice pack. The more detailed information will be discussed in the following paragraphs.

When the red Co(NO3)2*6H2O crystal was added to the white NH4 crystal, and water was added to dissolve, the solution turned blue in color. As the solution was nixed, the color changed to that of a blue-purple and a blue precipitate formed. When the 6 M NH3 began to be added, the color shifted to dark purple color after 15 mL of ammonia and the amount of the precipitate was less. After 20 mL of ammonia, the solution became a red brown with very little of the blue precipitate. After 30 mL of ammonia, the solution was similar in color to an iodine solution, a dark brown-red, almost black in color. At this point there was no visible precipitate on the surface of the solution. After 40 mL of the ammonia had been added, the solution was the same iodine like color as before. When closely examined, there was a black precipitate that had settled on the bottom of the beaker. At this point, hydrogen peroxide, 3% H2O2, was added to solution. After 4 mL of the H2O2 was added, the solution was the same color and the precipitate had not changes. After 8 mL of the H2O2, there was not noticeable change. After 12 mL of the H2O2, the solution was slightly redder in color but the precipitate had not changed. After 15 mL of H2O2, the solution was the same color and no changes had occurred to the precipitate. At 17 mL, the solution began to effervesce slightly, though there

17) Pour a small amount of the hot solvent into the flask containing the solid.

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

Write a balanced chemical equation for each reaction #1-8. Classify each reaction using the information provided in the

To begin figuring out if the reaction is orange or yellow after an ice bath you need to know LeChatlier's principle. LeChatlier's principle says that if anything gets added to the reaction will shift away. If something gets taken away from the reaction will shift toward. Chromate is a reactant so when it's added to trial one it shifted away to the products to keep up the ratio.

When we put the test tube 8, which had the 5 drops of water, into the ice cold water it also got a little darker. With all of these that turned darker, the equilibrium shift was on the product side. AgNO3 turned a white, NaOH turned a clear with a hint of yellow, the test tube with5 drops of water but in the boiling bath slightly turned a light red. The equilibrium shift was they went back to the reactant side. The only one that did not change was the HCl which had no

The results found from completing this experiment gave insight on how Le Châtelier’s principle reigns true. By viewing the color change of the different substances under temperature changes, and the physical properties change, it showed that predictions of the final equilibrium are accurate. For instance, viewing the clear NH4Cl crystalizing once HCl is added proved that this equilibrium of NH4+ and Cl- reach a state where there is enough aqueous solution and solid moving back and forth between forms and balance out. When viewing it settle into equilibrium, when it was heated in the hot water bath, the cloudy substance hardens on the bottom, with clear liquid floating on top of it. Viewing this in a broader perspective, this can be done for different types of reactions. But, things are subject to change if not only the temperature or concentration changes, but the pressure and volume. These three trials were done by changing concentrations, and then the temperature.