Reaction Of Ketone Lab Report

The objective of this experiment was to determine the rate law for a chemical reaction between crystal violet and hydroxide. A rate law is a part of kinetics, which is the study of how fast reactions occur and how to control the rate of a reaction (4). The rate law is be determined by measuring and graphing the absorbance of reactants during the reaction. The reaction was first order with respect to crystal violet (CV+) and hydroxide (OH-). Since crystal violet is in much smaller concentration than hydroxide, the experiment captured the reaction rate and order of crystal violet while the order of OH was calculated post-lab using the pseudo first order method (eqn 1,2,3). The rate law for CV++OH- CVOHis Rate = 0.1644m-1s-1[CV+][OH-].

First classical methods are described. The CHARMM force field, which we have used in this thesis is also briefly described. Then the quantum mechanical methods such as ab initio and semiempirical methods are briefly described. The SCC-DFTB method is described more elaborately since we have used SCC-DFTB as the quantum mechanical method to study the reaction mechanism in this thesis. Then QM/MM methods are described with available methods to study enzymatic reaction mechanisms.

Review 3: Text Chemical kinetics is the study of rates and mechanisms of chemical reactions. In our study of chemical kinetics, experimental data identifying the initial concentrations of reactants and the instantaneous initial rates of multiple trials is used to determine the rate law for the reaction, the order of the reactants, the overall reaction order, and the average rate constant. By comparing the instantaneous initial rates and the initial concentrations of the reactants for two trials, it is possible to deduce the order of each reactant. In order to determine the order of A, the two trials must be selected such that the concentration of A changes while the concentration of B is held constant.

For this experiment we determine the Michaelis constant (Km) and the maximum velocity (Vmax) and inhibition of alkaline phosphate. Using the different graph created and different methods of calculation I was able to determine the Km and Vmax for the different mixtures, and also what type of inhibitor it was. For mixtures 1-5, the Vmax was 4.04 and the Km was 0.019. For mixtures 6-10, the Vmax was 3.82 and the Km was 0.023. Using the slope from the graph of Lineweaver-Burk for reactions 6-10 I was able to determine Ki, which was 171.53, by calculating the [I] using C1V1=C2V2 scheme, which was 0.012. By plotting in the same graph the Lineweaver-Burk graph for reaction 1-5 and 6-10, I was able to determine that it was competitive inhibitor and

And the time for decay (t) from drug in the initial plasma, Cp1,to the drug in the final plasma, Cp2 is:

To verify our hypothesis, benzyl chloride 1a was initially chosen as a model substrate for an optimization of the various reaction parameters. In this optimization, we investigated the effect of parameters such as various oxidants additives, bases, solvent and various equivalents of the oxidant and additive. The results are shown in Table 2. The benzoic anhydride product 2a was produced in low yield 10% using 2 equiv. of TBHP as an oxidant, 4 mol% of NaI as an additive, 0.1 equiv of K2CO3 as the base in 0.75 mL of chlorobenzene at 120 °C for 3h (entry 1). Also, the increasing of reaction time for 5 of had no substantial effect on the yield of product 2a (entry 2). Therefore, in order to improve the yield of product, the effect of other additives

The purpose of these lab was to determine Michaelis constant (Km) and the maximal velocity (Vmax) and inhibition of alkaline phosphatase. The reason why we study enzyme kinetics in to be able to determine at what rate the enzyme catalyzed in a reaction. Michaelis constant equation measures how an enzyme converts a substrate into a product. Km in the require amount needed, and Vmax is the maximum velocity at which the reaction achieves the final product. For these experiment, with the graphs, I determine the value for Vmax, which equals to 4.04 and Km, which equals to 0.019, for reactions 1-5. For reactions 6-10, the value of Vmax equals 3.82, and the value for Km equals 0.023. Using the scheme of C1V1=C2V2 I was able to determine the value

Chemical kinetics is based on the use of an experimental rate law to determine the mechanism of a reaction. The experimental rate law for the given experiment can be found through the experimental instantaneous initial rate and the concentrations of each of the reactants present. First, using the equation rate = k[A]n[B]m, a ratio can be created of the rate equation of trial 1 to that of trial 2. These two trials are chosen because the concentration of reactant A is the same for both trials, so it can be simplified to one in the ratio. Since k is a constant and thus the same in both trials, it can be simplified to one in the ratio as well. After exchanging variables for the experimental data and simplifying, the resulting equation is 0.5 = 0.5m,

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.

A clock reaction is where the fusion of various reagents, with relation to time, cause a colour change in the solution. The end of the reaction rate is measured by the increase in the rate of concentration. There are two factors which contribute to the rate of the reaction, induction and inhibition. Induction is where the production rate of the clock chemical increases as the increases as the concentration of the solution increases. Whereas, Inhibition is where the chemical reacts with the clock chemical, increasing the concentration. The increase in the rate can only occur if all of the inhibitor chemical is consumed within the reaction (S.J Preece, 1999). Some examples of clock reactions are the arsenic (III) sulfide clock reaction, and Landolt iodine clock oxidation of bisulphite by iodate. This specific reaction is stated to be one of the most favourable clock reactions, showing a deep blue colour within a matter of seconds.

The two methods to determine the rate law of a kinetics experiment is by initial rates and by integrated rate law. To utilise the initial rates method, multiple experiments can be conducted with differing concentrations and measuring the initial rate for the reactions (Yamauchi, Nord and Schullery, 2016). From this, the reaction order for the corresponding substance can be calculated and the rate constant can be found. However, the method of initial rates requires the chemical reaction to be fairly slow and since several experiments need to be executed, it is not an ideal method.

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.

This investigation presents what would occur to the reaction rate of an enzyme if the temperature, pH level, concentration of a substrate and enzyme were changed. In this experiment, the enzyme catecholase, commonly found in plants, was tested and its product formation, benzoquinone was measured. When the concentration of the reactants such as the enzyme catecholase, and the substrate catechol were tested, the results of product formation increased greatly because the higher concentrations allowed the enzymes to increase their activity rates. When physical factors such as temperature and pH were tested the results fluctuated.

Investigations into the mechanics of chemical kinetics can reveal invaluable information relating to the rates of reaction. There are numerable applications of reaction rates, knowledge in this area is pivotal for industrial, commercial and research sectors. Thus, allowing them the ability to manipulate a variety of factors of chemical reactions with the use of reaction rates. In the scope of the kinetics of clock reactions, there is a range of information that can be obtained about reaction rates (Shakhashiri, 1992).

The purpose of this lab is to measure how an enzyme responds to the presence of an inhibitor in various concentrations, and identify what type of inhibitor that involved. In this lab, we used the Michaelis- Menten Kinetic, which proposed by two scientists Leonor Michael and Maud Leonora Menten for enzymatic dynamics. The model explains how reaction rate depends on the concentration of substrate and enzyme (chemwiki.ucdavis.edu). In the reaction of an enzyme catalyzed, the enzyme interacts with the substrate by binding to its active site to form the enzyme-substrate complex, ES. The reaction is