The kinetics of the acid catalyzed hydrolysis reaction of five Fe(II) Schiff base amino acid complexes were followed spectrophotometrically at 298 K. The used ONO donor ligands were derived from the condensation of salicylaldehyde with different five amino acids. The acid catalyzed hydrolysis reaction was studied in different ratios (v/v) of aqua – organic mixtures and in the presence of different concentrations of surfactants (CTAB and SDS). The increase in organic solvent ratio enhances the reactivity of the reaction. Moreover the addition of CTAB or SDS to the reaction mixture accelerates the reaction reactivity. The obtained kinetic data were used to determine the values of mG (the change in the activation barrier) for the studied …show more content…
The decrease in CMC value of the surfactant in presence of the complexes suggesting the interaction between the surfactant and the chelates which bring the reactants together through electrostatic interactions[31]. As the ionic micelles enhance the rate of reactions by increasing the concentration of the reactants within the small volume of its Stern layer[45]. Micelles can affect the reaction rates by including the reactants into the micellar aggregate. It was observed that the reaction rate increases with increasing both [CTAB] and [SDS] (Figs. 8 & 9), which clearly showing the catalytic effect of both CTAB and SDS below and above their CMC values[37, 46, 47]. It is can be demonstrated that the addition of CTAB and SDS to the reaction mixture, affected the hydrophobicity of the studied complexes leading to the acceleration in the reaction rate. The interaction between the surfactants and the complexes decreases the surface area of the reactants and increases the reaction rates, as the presence of the micelles leads to change in the mutual attraction and repletion force in the reaction medium. Therefore, the collision rate between the reactants will increase because of their nearby distance at the micellar boundary[37], this trend may considered as surface catalysis. Thus the attraction of the reactants species on the micellar surface enhances the reaction rate. On increasing [surfactant], the total area available for reaction will be more[30], consequently the observed rate constant (kobs.) values increase with increasing [surfactant] (cf. Tables.4 & 5). The plots of kobs against [surfactant] (Figs. 8 & 9) show a gradual increase in rates with [surfactant]. Such a type of behavior of the studied surfactants may be due to
Tyler White CHEM151LL 32658 04/01/2018 Different Types Chemical Reaction Types and Equations Purpose: The purpose of this lab experiment is to examine different types of chemical reactions such as Decomposition reaction, Synthesis reactions, Combustion reactions, and different Chemical equations. The experiments were conducted online using Late Nite Labs. Materials: Because the experiments were conducted online there wasn’t any physical use of materials, only digital ones, for these labs to be performed. Only the registration for the website was needed to perform these online labs, as well as a desktop computer.
Introduction Alka-Seltzer has been on the market since 1931 and has helped to relieve indigestion and upset stomach. The tablets began to fizz and bubble when dropped into water. “The fizziness happens when baking soda (sodium bicarbonate) and citric acid react chemically in water. They yield sodium citrate, water and carbon dioxide gas, which causes bubbles.” Based on this information, we will measure the reaction time of AlKa- Seltzer dissolved in 200 ml of water at 3 different tempertures in the first portion of this experiment.
(1 point) What is the desired catalytic reaction and the primary undesired reactions and explain the enthalpy terms? The chemical equation representing the desired catalytic reaction is the selective hydrogenation of CO2 to produce methanol, which can be written as follows: CO_2 + 3H_2 → CH_3 OH + H_2 O In this equation, carbon dioxide (CO2) and hydrogen gas (H2) react in the presence of a catalyst to produce methanol (CH3OH) and water (H2O).
ABSTRACT To catalyze a reaction, an enzyme will grab on (bind) to one or more reactant molecules. In this experiment we examined how increasing the volume of the extract added to the reaction would affect the rate of the reaction. The enzyme used was horseradish peroxidase which helps catalyze hydrogen peroxide. Using different pH levels, the absorbance rate of the reaction was measured to see at which condition the enzyme worked best. The rates of absorption were calculated using a spectrophotometer in 20 second intervals up to 120 seconds.
Abstract In this experiment, the reaction kinetics of the hydrolysis of t-butyl chloride, (CH3)3CCl, was studied. The experiment was to determine the rate constant of the reaction, as well as the effects of solvent composition on the rate of reaction. A 50/50 V/V isopropanol/water solvent mixture was prepared and 1cm3 of (CH3)3CCl was added. At specific instances, aliquots of the reaction mixture were withdrawn and quenched with acetone.
Lab Report 5: Acetylsalicylic Acid (Aspirin) Synthesis Name: Divya Mehta Student #: 139006548 Date Conducted: November 19th 2014 Date Submitted: November 26th 2014 Partner’s Name: Kirsten Matthews Lab Section: Wednesday 2:30 L9 IAs Name: Brittany Doerr Procedure: For the procedure, see lab manual (CH110 Lab Manual, Fall 2014) pages 96-98. Wilfrid Laurier University Chemistry Department. Fall 2014. Acetylsalicylic Acid (Aspirin) Synthesis.
Our class went to the Conodoguinet creek and we tested the creek for signs of acid rain pollution, phosphates and nitrates, and dissolved oxygen levels. My hypothesis is that the creek would end up being polluted. But after the testing we did our results showed that the creek was not polluted. some of the tests we completed were water alkalinity tests, critter count tests and rocks that neutralized the acidity of acid rain. We also calculated the velocity of the water.
What type of chemical reaction will a balloon receive when filled with an acid and base? Acids and bases are around us everywhere in various types of liquids. They are in the foods we eat and the things we use on a daily basis, for example liquid dishwashing soap. Acids are usually sour and bases are silky, giving it a bitter taste. Water can act like both, depending on the situation.
Conclusion: In Station 1- reaction 2, Station 3- reaction 1, Station 4-reaction 1, Station 5 reaction 1, Station 6-reaction 1 and 2, and Station 7- 1 and 2 there was chemical reaction because all of those mixed ionic compounds created a precipitate. However some solutions did not become insoluble and produce precipitates such as: Station 1- BaCl2 (aq) + KNO3 (aq) , Station 2- KNO3(aq) + AgNO3(aq) and KNO3(aq) + CaSO4(aq), Station 3- Na2CO3(aq) + KNO3(aq) , Station 4- NaPO4(aq) + KNO3(aq)
Wilfrid Laurier University, ON, Canada. Observation Results: Table 1: Qualitative Observations of all reactants and products in experiment Reactant/ Product Before During
Aim The aim of this investigation was to experimentally determine the order and rate law expression of the reaction between sodium iodide and iron (III) nitrate 9-hydrate. Introduction The most interesting topic in grade twelve chemistry was the unit on kinetics, therefore after brainstorming a mind map on the stimulus that I chose, I was interested in creating an experiment to determine the order and rate law expression between two reactions myself. The original idea for this project came from a lesson on the order of reactions and rate law expressions.
Aim: To find out the relationship between the greater concentration of sodium thiosulfate when mixed with hydrochloric acid and the time it takes for the reaction (the time it takes for the solution to turn cloudy) to take place and to show the effect on the rate of reaction when the concentration of one of the reactants change. Introduction: The theory of this experiment is that sodium thiosulfate and hydrochloric acid reach together to produce sulfur as one of its products. Sulfur is a yellow precipitate so, the solution will turn to yellow color while the reaction is occurring and it will continue until it will slowly turn completely opaque. The reaction of the experiment happens with this formula: “Na2 S2 O3 + HCL =
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.