All throughout the lab the assumption that is made throughout the lab is that the bisulfate ion has a reaction order of zero. Thus, this light could have increased the energy of the particles participating in the reaction, and thus increase the inaccuracy because this is an external factor affecting the rate of reaction.
In conclusion, although there were some errors associated with this experiment, it was successful in determining the relationship between temperature and reaction rate.
This assumption will be further evaluated in the evaluation of the weaknesses and limitations. This could have been avoided by making a large amount of the HCl in the desired concentration at the beginning of the experiment.
The Kinetic Molecular Theory states that temperature is a measure of average kinetic energy of the particles Thus, Due to the increase in temperature the average kinetic energy of the particles increases proportionally thus resulting in higher overall entropy.
These two theories justify the corresponding increase of both factors.
Lastly a limitation in part B is that a final temperature for the solution could not be measured because of all of the surrounding influences such as holding the tube would have transferred heat to the solution.
Evaluation A limitation in part A would have been that the stirring would have affected the time it took for the solution to turn blue. Another factor that could have affected the accuracy is the fluctuation in room temperature during this experiment.
However, in regards to specific rates of reaction, they affect the accuracy. Although the experiment was successful in showing the relationship discussed above, there are a few errors associated with this experiment that could have hindered the accuracy of the results.
Furthermore, some reactions can be sped up depending on how much light they are exposed to. One factor that could have affected the accuracy of this experiment is the fact that each solution of HCl was diluted separately.
The experiment should have been done both ways to have the most accurate results. Also because the assumption was made that the reaction order of the bisulfate was zero because it was constant throughout may have affected the results as well.
This could have increased or decreased the temperature of the HCl during the reaction. As well another way that the procedure can be improved upon is to perform the lab like a titration lab using a burette, flask and the indicator.
This allows for greater error as each time something is measured there is an error associated with the piece of equipment used.
Rate of Reaction Graph 1 shows the relationship between change in temperature and the rate of reaction. Some of the tubes may have gotten more stirred than others and this would have caused an inaccuracy in the times that were collected.
The trend shows that the as the temperature of the HCl increases, so does the rate of reaction. Also, when the tube was taken out the bath tub the room temperature immediately affected it, constantly changing the final reaction.
It showed that temperature and rate of reaction increase proportionally due to a greater number of collisions. The final rate law determined was: In conclusion, this experiment was successful in determining the relationship between temperature and reaction rate.
Better collection techniques such as spectrometry should have been used because then when ion changed colour it would be detected right away. Another relationship that can be seen between the rate constant and the temperature is that as the temperature increased the rate constant increased as well.
Conclusions that can be drawn from the data is that when the concentration of the potassium iodate solution was increased the rate of reaction decreased. In order to avoid this problem, the reaction should be conducted in a closed room with a stable room temperature.
Instead of the iodate ion concentration being changed the concentration of the bisulfate could have been changed by making it the limiting reactant in the balanced equations.
This experiment was performed in an open classroom with bright lights and open windows.
Therefore due to increase in average kinetic energy of the particles, the collision rate increases proportionally resulting in a higher rate of reaction. Once again, this can be avoided by performing the experiment in a closed room. Also some solutions turned blue right away and others took a while so they could be seen by the human eye.
In part B the activation energy was found to be Conclusion and Evaluation As discussed in the introduction, the relationship between temperature and reaction rate is explained through the Collision Model and the Kinetic Molecular theory.
Temperature of HCl vs. This is a polynomial relationship, which implies that the rate of reaction increases exponentially in relation to the increase in temperature.Rate of Reaction of HCl & Mg Lab Answers.
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AP Chemistry Kinetics of a Reaction Lab by jonathanchen77 in Types > Research > Science Determining the Order of a Chemical Reaction Lab. o determine the reaction rate and the total rate law of a reaction involving the oxidation of iodide ions by bromate ions in the presence of acid o determine the order of each individual reactant 3/5(2).
AP Chem Lab Book (''11) of Brad Hekman. Search this site. Information & Links. Demonstrations. Underwater Fireworks. The Rate and Order of a Chemical Reaction.
Experiment The Determination of an Equilibrium Constant. Report Abuse | Print Page | Powered.
Rates of Chemical Reactions I: A Clock Reaction Lab 29 Objective To measure the effect of concentration upon the rate of reaction of peroxydisulfate ion with iodide ion; to determine the order of the reaction with respect to the reactant concentrations; and to obtain the rate law for the chemical reaction.
Iodine Clock Reaction Lab Answers Part A: Determining the complete rate law The order of reaction with respect to the iodate ion, m, must be determined for the following rate. Report abuse. Transcript of Chemical Kinetics Lab. The rate expression for this experiment was found to be L/mol s.
This low value indicates a slow reaction rate. The rate expression was found to be: and the overall order of the reaction is second order. The order of the reaction and the rate expression can only be determined.Download