Rates of reaction

Background: A clock reaction generally involves a mixture of solutions that, after a certain amount of time, displays a sudden colour change. This process demonstrates chemical kinetics in action, which is the study of chemical processes and rates of reaction where the reaction rate is the speed at which the chemical reaction proceeds. It is dependent on several factors that rely on one basic underlying principle called collision theory. In order for a reaction to occur, the reactant molecules

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). A clock reaction is characterised by an abrupt colour

Discussion The experiment investigated the relationship between temperature and the rate of reaction for the reaction of iron (III) nitrate with sodium thiosulfate. The results show that the rate of iron (III) reacting forming iron (II) increases as the temperature of the solutions increases. Table 1 shows that when the temperature of the reactants is 4℃, it takes 54.173 seconds for the reaction to occur to the stage that the cross to appears. The time taken for the solution to reach the same transparency

1. Experiment [tBuCl]0 (M) [OH-]0 (M) Time (s) Reaction rate (M/s) Rate constant (s-1) 1 0.03 0.003 38.78 7.74 x 10-5 2.72 x 10-3 2 0.03 0.006 73.295 8.18 x 10-5 3.04 x 10-3 3 0.03 0.009 156.78 5.74 x 10-5 2.28 x 10-3 Sample Calculation from Exp.1: Total Volume of Solution = 10mL*1L/1000mL= 0.01L [OH-] used = 0.1M, volume used = 0.3mL*1L/1000mL = 0.0003L [tBuCl] used = 0.1M, volume used = 3mL*1L/1000mL = 0.003L • [OH-]0 = ([OH-] used* Volume of [OH-] used)/ Total Volume of Solution =

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

Enzymes play a critical role in metabolic processes by speeding up chemical reactions. Enzymes lower energy barriers by acting as a catalyst for a reaction. An example is hydrolysis that occurs in glucose. Without enzymes glucose will still hydrolyze, but at a slow rate. With the right enzyme hydrolysis will occur even more rapidly than before. Enzymes work by having a substrates enter their active site. Induce fit (the substrates forms weak bonds with the enzyme causing the enzymes shape to enfold

Aim- To show the effect of the particle size of solids on rate of reaction. Hypothesis- If the size of the particles are smaller, there will be more collision between the particles as surface area will be more and therefore the rate of reaction will be more than if the size of the particle are larger. Precautions: 1. Wear safety glasses to prevent chemicals from going into your eyes. 2. You should wear a lab coat to make sure not to spill anything on your clothes. 3. Wear clothing that covers your

Investigate if changing the concentration of an acid will change the rate of the reaction when marble is dissolved in hydrochloric acid. Apparatus Marble Chips Conical Flask Hydrochloric Acid Gas Syringe Delivery Tube Stop Watch Fair Test To make the experiment a fair test I will use the same amount of acid for each concentration. I will do this by using a capillary tube because they are very accurate. I will use 3g of marble in each concentration of acid. I will clean everything out before I

the reaction to occur which means that an increased rate of reaction has been formed. 2b. As the surface area of the magnesium metal increases/the magnesium piece becomes smaller, it takes less time for the reaction to occur as more molecules are present which increases number of collisions and an increased rate of reaction has been formed. 2c. As the temperature of the acid increases or becomes hotter, it takes less time for the reaction to occur which means that an increased rate of reaction has

Following the calculation of the rate law, Rate = k[H+]2[C6H10O] it was found that the experimental order of the reaction was higher than the theoretical value, Rate = k[H+][C6H10O]. The reason for this value not being calculated correctly was most likely due to the performance of erroneous handling methods conducted during the experiment. From the calculations of rate law, it was observed that the measurements for Run 2 and 3 were not aligned with those of the other runs. The molar absorptivity’s