Iodination of Acetone

In reference to the collision theory, molecules act as small spheres that collide and bounce off each other, transferring energy among themselves when the collide. In order for a reaction to occur, there must be collisions between molecules. Through experimentation, factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants, temperature, surface area, the physical state of reactants, and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and

Temperature is a measure of kinetic energy. As this movement increases, collision rate and intensity, and therefore reaction rates, increase. This experiment was conducted to determine if there is a minimum temperature that increase kinetic energy and denature enzymes to slow enzymatic reactions or fail to catalyze them. The experimental results indicate an increase in temperature will increase reaction rates until proteins denature.

Hypothesis: If the temperature of the sodium thiosulfate is increased, then the time it takes the precipitate to form will decrease therefore leading to the rate of reaction to increase as well. This can be explained as the temperature increases, the particles in the molecule will be moving more rapidly and hence as they move quicker, they will be colliding with other particles more frequently and with more energy. This energy will likely overcome the activation energy barrier and break the initial bonds and therefore produce a successful reaction and due to the increase in frequency of collisions, the time it takes the precipitate to form will decrease and since the product/precipitate is produced faster, therefore the rate of reaction will increase.

Temperature controls the speed the enzymes work at. Higher temperatures increase the kinetic energy which increases the chance of collision therefore speeding up the rate of

When the concentrations were changed so did the rate of reaction. When the concentration was changed to 0.265M the rate of reaction dropped by a factor of 0.5 (50%) below the control value. Furthermore when 60mL of water was added to the bleach dropping the concentration too 0.132M the rate dropped by a factor of 0.7 (70%).

Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60.62 KJ/mol.

Is this a linear relationship? What happens to the initial reaction rate as substrate concentration increases?

The hypothesis tested in this experiment was, if the temperature of enzyme catalysis were increased, then the reaction rate would increase, because enzyme-catalysis reacts by randomly colliding with substrate molecules, and the increase in temperature increases the speed of collision or reaction rate. The final data collected for the experiment was positive with my hypothesis. The coffee filter, covered in potato solution, sank and rose at a faster pace in the hydrogen peroxide when the temperatures were raised.

9. Does temperature have any effect on reaction rate? If so, why does it occur?

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

To vary the concentrations of each reactant along with the sulphuric acid in order to observe and measure its effect on the overall rate of reaction in absorbance using colourimetry.

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.

Martin Novick Group 14, Chemical Engineering Laboratory Submitted to Prof. David B. Henthorn September 25, 2012 Summary The goal of this project was to determine the pre-exponential factor, k o , the activation energy, E, and the reaction rate constants, k, of the saponification process of ethyl acetate using sodium hydroxide (NaOH) at 5 temperature between 15 and 25 degrees Celsius. Two trails were performed at temperatures 16, 18, 20, 22, and 24 degrees Celsius. The main equipment of the project were the jacketed beaker batch reactor and the LabPro conductivity probe. The solution’s conductivity throughout the reaction was collected and plotted in a linearized plot against time to

The key aim of this experiment was to determine the rate equation for the acid-catalysed iodination of acetone and to hence consider the insinuations of the mechanism of the rate equation obtained.