Lab Report On Kinetics Of Alcohol Oxidation

This website was used on October 3, 2014 to help develop a better understanding of collision theory in order to explain the various factors affecting the rate of reaction.

A reaction rate is the speed at which a chemical reaction occurs. The reaction rate is affected by surface area by increasing the more surface area there is, because there are more particles exposed to the other reactant. For example, if a solid is grinded into a powder, the reaction rate will be quicker as there is more surface area.

This would be a suitable independent variable as it would be easy to change ourselves. If the concentration of the substrate increases the faster the rate of reaction, as more hydrogen peroxide molecules can collide with catalase molecules, so more reactions will take place. As you increase the concentration of substrate this will continue to occur up to a point where all the active sites on the enzyme are being used.

Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction:

As the substrate in increased the initial reaction rate will increase until it is fully submerged and then will not increase any more. The relationship is linear. As the substrate concentration increases, the initial reaction rate increases.

To determine what factors influence the rate of a chemical reaction and to make predictions based on these

Introduction The reaction rates provide important information concerning the factors that control the speed of a chemical reaction or the steps that occur in complex mechanisms of a chemical reaction in a study called chemical kinetics. The most common factors that affect the reaction rate are concentration, temperature and actions of catalyst. The rate of reaction is ( Rate=k[A]n[B]m) which is written in rate law expression. Reaction rates may be determined by following the appearance of disappearance of chemical substance or the change in a characteristic property.

The purpose of the experiment is to oxidize a secondary alcohol (2-octanol) by using sodium hypochlorite (bleach) to produce 2-octanone. The starting material consisted of a sample of 2-octanol that was placed into a three-neck flask along with acetic acid and acetone creating an acidic solution. While monitoring temperature fluctuations to ensure a temperature of 400 Celsius was not reached, sodium hypochlorite slowly dripped from a separatory funnel into the acidic solution. Once this reaction reached its entirety, the solution was combined with sodium bisulfate to remove any of the remaining oxidizing agent. This solution was then tested and brought to a neutral pH using a sodium hydroxide solution. The reaction material was extracted using ether and was then washed with a saturated sodium chloride solution. The organic solution was then dried using magnesium sulfate and was then decanted and placed onto the rotovap. The produced weighed .599g and based on the infrared spectrum analysis (see Figure 1) preformed on the product it was determined to be 86.1% 2-octanol, which means .516g of 2-octanol was obtained in the final product.

The conditions for this type of reaction vary depending on what degree of alcohol you are trying to oxidize. In our case, we oxidized a secondary alcohol at room temperature. It was

The second rate is not used in this step since the volume of potassium iodide in the second solution is the same as the volume in the first solution. After simplifying, the ratio of the rate is equal to the ratio of the volume, therefore the coefficient and the order of the concentration equals one. By adding both value of the orders, the overall order equals

Chemical reactions take place in all living organism. All Most all chemical reactions require an enzyme. These enzymes act as a catalyst to help regulate the rate of a chemical reaction. Three small lab experiments were performed to find the optimum pH, temperature, and concentration of the enzyme and substrate. The lab used the reaction of Catalase converting H2O2 into H2O and O2. The reaction was measured by the production of oxygen, using quaiacol that turns brown when oxidized. A spectrophotometer set to an absorbance of 500 nm was also used to measure the reaction rate. The procedure can be found in the biology 1 lab manual on pages, 243,244,245. After preparing the tubes following the instruction in the procedure section, two test

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

2) Calculate the a mean rate constant using orders of reactions and the rate equation allowing for the overall order or reaction to be found.

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.

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.