Iodine Clock Reaction

Many factors effect reaction rates, two shown above include temperature and concentration. Concentration affects the rate of reactions because the more concentrated a solution the more likely collisions between particles will be. This is simply because there are more particles present to collide with each other. When the temperature is higher, particles will

After concluding our investigation of luminol reactions with the different variables of cold water, hot water, bleach, and hydrogen peroxide, our hypothesis was supported by the results. The purpose of our experiment was to discover which certain variables would result in a longer duration of a glow. Our hypothesis stated that the higher temperature of the water (therefore, the variable hot water) the glow caused from the reaction would last longer due to the rapid thermal energy leading it to have a more vibrant and longer-lasting luminescence. As displayed in our data table, and delineated into a bar graph, where hot water lasted for the highest number of seconds when tested in three separate reactions. Cold water came in as the second longest, while

According to the collision theory, the rate of a reaction depends on the frequency of collisions between reacting particles. The more frequent the collisions, the faster the rate of the reaction. However, in order for the collisions to be effective, the particles must collide with sufficient energy (activation energy). Furthermore, the particles must collide with the proper orientation.

By heating to refluxing, the temperature and thermal energy were controlled during the experiment. Heating the reaction is important because it is required in order for the bonds to break to cause a chemical reaction. Breaking bonds also means requiring energy and that is where activation energy comes into play. All chemical reactions has to overcome an energy barrier to generate the product from the reactant.

Introduction: First discovered by Hans Heinrich Landolt in the 19th century, the Iodine Clock reaction is what is described as a chemical clock reaction, and today is one of only few known to science. It is useful as a tool in determining the rate of a chemical reaction due to a marked change in the color of the reacting solution when a particular reaction has been completed. The process is also practical as an introduction to reaction rates and kinetics. A solution of hydrogen peroxide is mixed with one containing potassium iodide, starch and sodium thiosulfate. After a varying amount of time the colorless mixture suddenly turns dark blue which is one of a number of reactions related to the iodine clock.

Then, a fixed amount of sodium bisulfite/sulfuric acid/starch solution was added to each iodate solution, and the time needed to turn the mixed solution blue was recorded. Based on the measured time, reaction rate was calculated. It was found that the higher the concentration of iodate ions, the faster the reaction time. It was also found that the order of reaction was approximately 1. The result matched my prediction.

Temperature: Temperature is an extremely important variable to consider, as it can affect the rate of reaction in a number of ways. If the temperature of a system is increased, more molecules will reach the activation energy and the rate of reaction will increase. The number of collisions will also increase. As enzymes must collide with substrates, an increase in temperature and thus kinetic energy will result in more collisions occurring in a given time. Increasing the temperature will also increase the heat of the molecules.

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.

Reactions are defined as having three states, reactants, transition state, and products. The transition state is the highest energy state of the system, essentially acting as the activation energy. If the molecules collide with more kinetic energy than the transition state energy, then the reaction will transpire, and products will be produced.4 The experimentally determined activation energy for the bleaching reaction between green dye #3 and bleach was 12328 J/mol, as compared to the activation energy of 7580 J/mol for the reaction between green dye and cetylpyridinum chloride, the experimental was larger.3 This means it takes far more energy to cause the bleach to react with green dye #3 than it does for green dye to react with cetylpyridinum chloride. Moreover, the reactions are not the same, so the activation energies will be dissimilar, nonetheless, both reactions cause the decolorization of green dye.

Procedure A was an experiment on observing how different effects of extreme temperatures have on enzyme catalysis. There are three parts in this experiment. In part 1, we took a syringe labeled “H2O2” and used it

In the results we can see that the purple pink solution of potassium permanganate (MnO4-) was reduced to a colourless solution of manganese ions (Mn2+).

In the Iodine Clock reaction experiment, we stall a reaction by having Iodine changed rapidly by two chemicals between it’s two forms. These two forms have slightly different properties. The first form of iodine is I⁻. This is not an indicator of starch. The second form of iodine is I₂. This type is an indicator of starch(a chemical that changes color in the presence of a starch).

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

| Measure the time taken for the potassium permanganate solution to decolourise from purple to colourless by using stopwatch

Activation energy is the minimum amount of energy for a reaction to undergo. Only a small amount of collisions between