Lab Report On Kinetics Of Alcohol Oxidation

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:

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

This investigation will be carried out to investigate the rate of reaction of the enzyme catalase on the substrate hydrogen peroxide.

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.

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

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 sum of x and y will give the overall reaction order. The orders of reaction are based on the kinetics of the reactants and so can only be found after the experiments have been completed. The can be worked out using the initial rate method, in which experiments are repeated using different concentrations, then the initial rate of the reaction is calculated (using 1/time as shown above). The initial rate is then plotted against the concentration on a graph, showing the order of the reaction.

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

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.

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

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 kinetics is the study of how fast a chemical reaction occurs and the factors that affect the speed of reaction.1 Reaction rates are the measure of how much the concentration of reactants change during a given reaction.1 The rate of change of the reactants, Rate = - Δ [X]/Δt, is related to the slope of the concentration vs. time graph.1 From observing reaction rates, the overall order of the reaction and the rate constant can be calculated by using the integrated rate laws. For a zero-order reaction, the rate law can be written as [A]t = -kt + [A]0, where [A]t is the concentration at a given time, k is the negative slope, t is the time, and [A]0 is the initial concentration.2 Using the same variables, a first order reaction can be written as ln[A]t = -kt + ln[A]0 and a second order can be written as 1/[A]t = kt + 1/[A]0.2 On a graph, these concentrations are plotted vs. time, allowing the R2 value and equation of the line to be calculated. The R2 value is used in determining the order of the reaction. The closer the R2 value is to 1, the more likely that the graph displays the correct reaction order. The y=mx+b equation provides information about the slope and y-intercept, essential when determining the order and rate constant.

The rate of chemical reaction increases with the presence of a substance called as catalyst.

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.