Lab Report Chemistry

However, the results of this experiment may not have been as accurate or precise as they

Title: The Effect Temperature of Sodium Thiosulfate Has On The Rate of Reaction with Hydrochloric Acid

3.What was your prediction about the results of each factor tested in your two lab procedures? Explain your predictions based on your knowledge of the dissolving process, collision theory, and reaction rates.

The lab was completed for two main reasons. The first reason was to determine the equilibrium constant for the

Analyze results – Assume that your experiment produces results identical to those seen in Table 4, what type of graph would be appropriate for displaying the data and why?

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples.

The problem with the experiment is regression to the mean. Regression is a threat that occurs when you have a nonrandom sample from a population and measures that are imperfectly correlated.

The chemical reactions that could be used to store energy are Decomposition Reaction (Invisible Ink) and Reversible Decomposition-- Combination Reaction (Dehydration of Blue Vitriol/ Rehydration of Copper (II) Sulfate). 2. The following reaction is exothermic, Heme-O2 +CO  Heme-CO+ O2 .

Evaluation. As I repeated the experiment 3 times and worked out the average rate of reaction in each test, I think my results are quite reliable. However, I could make further improvement by increasing the number of tests and taking the results with a smaller gap such as 10 seconds instead of 20.

Therefore, a direct linear trend in which the reaction time increased as the concentration of Na2S2O3 increased was anticipated. Instead, the data recorded for the volume of Na2S2O3 versus reaction time did not explicitly show a direct linear trend (Figure

When one looks back at the procedure of the experiment, trials 1, 2, 3, 4, 5, and 6 all use 6 M HCl for their reactions, and if this were to be substituted for 6 M HNO3, then these reactions would have still taken place, except in trial 2 because copper is less reactive than hydrogen in all cases, but their final observations may yield different colored solids and solutions (Beran,

During this experiment, 4 people participated to complete it. My partner and I did Part 2, while the other two did Part 1, then we all worked together in Part 3. I did not find interest in this assignment but it was extremely easy to complete. I was able to understand how to graph the analyzed data found by using the equations I determined. One flaw is that it took way too long to

There were some limitations that were encountered during the experiment, and the planning stages. Such as, the constant changes made to the method. The method had to be changed three times this was due to scaling back the measurements of the solutions. The solutions that were part of the original method would have resulted in 20 ml of the blue solution, which would waste the sodium bisulfite and potassium, every time a test was conducted.

Chemical kinetics involving reaction rates and mechanisms is an essential part of our daily life in the modern world. It helps us understand whether particular reactions are favorable and how to save time or prolong time during each reaction. Experiment demonstrated the how concentration, temperature and presence of a catalyst can change the rate of a reaction. 5 runs of dilution and reaction were made to show the effect of concentration on chemical reactions. A certain run from the previous task was twice duplicated to for a “hot and cold” test for reaction rate. The prior run was again duplicated for a test with

Two catalyst reactants are used in the experiment, thiosulfate and starch, to dictate the time of reactions.