Lab Repor Chemical Kinetics Essay

In this lab, the study of the kinetics of a chemical reaction will be investigated. One of these reactions involved the oxidation of iodide ions by bromate ions in the presence of an acid.

From the testing and results several major trends and relationships were discovered. The first observation, which supports the hypothesis, is the relationship between concentration of reactants and reaction rate. As concentration increased, the reaction rate also increased in direct proportion. This was shown by the results because when the concentrations doubled, from 0.1M and 0.125M to

They observed an increase in initial rate with increasing the concentration of substrate but after 40 minutes the degradation efficiency decreased with increasing initial concentration (figure7). A pseudo-first-order kinetic was assigned to the reaction and the initial rate of the reaction for different concentrations was measured. Using Langmuir rate model and the initial rates, rate constants in different pH values were calculated. Acidic pH (3.5) showed higher reaction rate due to favored interaction between positive surface of catalyst and oxygen atoms. pH 9.5 showed higher rate constant supposedly caused by substrate hydrolysis in basic solution

The data supports the hypothesis that an exponential relationship will be found between the change in temperature and the reaction rate, and that the highest temperature will have the fastest rate of reaction. The data also supports the hypothesis that as the concentration of Potassium Iodine increases so will the reaction rate, and vice versa for an increase in Sodium Thiosulphate concentration. The hypothesis that the Iron (II) ions will affect the reaction rate, and that the optimal amount will be about 0.1M of catalyst was partially supported.

This experiment runs many reactions varying the concentrations of the reactants in order to determine the order for each component and the rate constant.

Three experiments were carried out to identify the effects of temperature and substrate concentration on the rate of an enzyme-catalysed reaction, as well as the relationship between absorbance reading and concentration of the substrate solution based on Beer-Lambert law.

Each reaction would be carried out by mixing five different solutions four times separately and each reaction is consisted of KI solution, starch solution, Na2S2O3 solution, KNO3 solution and EDTA solution. The concentration of each solution varies because the first reaction include 25.0ml KI solution, 1.0ml starch solution, 1.0ml Na2S2O3 solution, 48.0ml KNO3, 1 drop EDTA solution and the total volume eqaul 75.0ml. The second reaction include 25.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1 drop EDTA solution and total volume equal 50.0ml. The third reaction include 50.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1 drop EDTA solution and the total volume equal 75.0 mL and the fouth reaction include 12.5 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 35.5 mL KNO3 solution 1 drop EDTA solution and total volume equal 50.0ml. After obtaining all of the solutions and seven different test tubes of 1.0ml Na2S2O3 solution which should be pour into the Erlenmeyer flask whenever the color of the solution changes. To calculate the reaction rate of each reaction the timer should start immediately when all of the solutions are mixed. Once all of the solutions have been mixed the students should observe as well as record the time of the reaction when the color change to dark blue and one of

By analysing the results of The Landolt clock reaction, and the outcomes that occur due to change in concentration and the addition of a catalyst, the data did partially support the hypothesis. That by changing the concentrations of potassium iodate and sodium bisulphite the rate of the reaction will increase. The rate gradually increased per every 10 seconds on the NaHSO3 graph. Whereas compared to the KIO3 graph the rate was more efficient, the reaction was achieved within 5 seconds. However, the second hypothesis regarding the addition of a catalyst, displayed acceptable results. The catalyst increased the speed of the reaction within 10 seconds, which was slightly faster than the reaction times gained from the

The study that focuses on chemical reaction rates is kinetics. Kinetics contributes to the understanding of the speed of chemical reactions and what determines if a reaction happens at all. A large factor in determining if a reaction occurs is if the activation energy can be achieved. Activation energy is the energy required to start a chemical reaction so that it will not need any additional energy to continue. The amount of energy absorbed or transmitted by a solution is proportional to the solution’s molar absorptivity and the concentration of the solute, this is known as Beer’s law.

The hypothesis of this experiment was that an increase in concentration will increase the rate of reaction by decreasing the time taken for the colour change to occur. Figure 1.1 shows time on the x axis and concentration on the y axis, it can be seen that as [reactant] decreases, time increases.Thus, the results correlate with the hypothesis that an increase in concentration will produce a faster reaction time and subsequently a larger reaction rate - regardless of change in [KIO3] or [Na2S2O5], both reactants produce the same result.

In the 90-minute reaction, the reaction was run to completion and TLC was conducted to analyze the final product. In the 50-minute reaction, aliquots of the of the reaction mixture was obtained every 15 minutes to analyze the reagents and induce the progress of the reaction.

Introduction: In this experiment we will be investigating how changing the temperature of the made up solution (copper chloride dihydrate and water) will impact the rate of a reaction when aluminium foil is dropped into it. We will determine this by selecting five different temperatures: 26 degrees, 36 degrees, 46 degrees, 56 degrees and 66 degrees and seeing at which temperature the reaction between the solution and aluminium foil produces the most heat. We will be recording the before and after temperatures after 2 minutes when the aluminium foil has been placed in the solution and also the average of the temperatures, this will help us determine if a hotter or colder

There are also some elements that are not a part of any type of family. These elements are mostly other metals that are located right after the transition metals. There are some nonmetals that are included in this group. Some of these nonmetals include silicon, nitrogen, carbon, and phosphorus. All elements in this group are some what reactive. Nitrogen is the most common element. Compounds using nitrogen consist of silver nitrate, potassium nitrate, and nitric oxide. Silver nitrate is used in many different chemistry labs.

First approximately 250mL of water was added to a 400mL beaker and heated on a hot plate to 20-25C. As the water was heating, two test tubes were then prepared, test tube A which contained 10mL of 0.0100 M KI, 10 mL of 0.0010 M Na2SO3, and 10 mL of deionized water, while test tube B included 10mL of 0.0400 M KBrO3, 10 mL of

The hypothesis that as (the first variable being tested), the concentration in the solution is changed and it becomes more dilute, this will result will be a slower rate of reaction. Therefore, it is also hypothesised that the addition of a catalyst will cause the rate of those reactions to speed up, was proven correct by the results of this experiment, in that the changing of the concentration and the addition of a catalyst changed the speed at which the reaction occurred. The results from both Part 1 and Part 2 conclusively showing that the have a direct effect on the rate at which the reaction occurs. In order to come to this conclusion, the data needs to be transformed into rate laws.