Essay on Determination of the Rate Constant

And finally into test tube 3, I pipetted 1.0 ml turnip extract and 4.0 ml of water. The contents of test tube 1 was poured into a spectrometer tube and labeled it “B” for blank. “B” tube was now inserted it into the spectrometer. An adjustment to the control knob was made to zero the absorbance reading on the spectrometer since one cannot continue the experiment if the spectrometer is not zeroed. A combination of two people and a stop watch was now needed to not only record the time of the reaction, but to mix the reagents in a precise and accurate manner. As my partner recorded the time, I quickly poured tube 3 into tube 2. I then poured tube 2 into the experiment spectrometer tube labeled “E” and inserted it into the spectrometer. A partner then recorded the absorbance reading for every 20 seconds for a total of 120 seconds. After the experiment, a brown color in the tube should be observed to indicate the reaction was carried out. Using sterile techniques, any excess liquid left was disposed

In reference to the collision theory, molecules act as small spheres that collide and bounce off each other, transferring energy among themselves when the collide. In order for a reaction to occur, there must be collisions between molecules. Through experimentation, factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants, temperature, surface area, the physical state of reactants, and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and

The Hydroxyl group on alcohols relates to their reactivity. This concept was explored by answering the question “Does each alcohol undergo halogenation and controlled oxidation?” . Using three isomers of butanol; the primary 1-butanol, the secondary 2-butanol and the tertiary 2-methyl-2-propanol, also referred to as T-butanol, two experiments were performed to test the capabilities of the alcohols. When mixed with hydrochloric acid in a glass test tube, the primary alcohol and secondary alcohols were expected to halogenate, however the secondary and tertiary ended up doing so. This may have been because of the orientation of the Hydroxyl group when butanol is in a different

Kinetics is the study of the rate of chemical processes. The kinetics of the reaction between crystal violet and NaOH was studied. In order to monitor crystal violet concentration as a function of time, a spectroscopic colorimeter was used. What is the rate law for decolorization of crystal violet? In order to figure this out, the rate of the reaction of crystal violet and sodium hydroxide must be found. In this experiment, the initial goals were to determine the overall rate law for the rate of decolorization of crystal violet in basic solutions as a function of time and to determine the rate law for the reaction including the actual value of k; Rate = k[A]x[B]y. The rate of a reaction was expected to depend on the concentrations

Introduction: The purpose of this experiment is to understand the kinetics of the hydrolysis of t-butyl chloride.The kinetic order of reaction was studied under the effects of variations in temperature, solvent polarity, and structure. It is particularly observed in tertiarhalides i.e. in SN1mechanism, Nucleophilic Substitution which is in 1storder. It is basically a reaction that involves substitution by a solvent that pretendslikea nucleophile i.e. it donates electrons. The reaction being in firstorder means

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

Upon the addition of water, it was noted that a layer separation occurred and the water layer remained on top, with the 2-methylphenol layer on the bottom layer. Then, conversion calculations were performed to determine the appropriate amount of 3M NaOH to be added to the 2-methylphenol solution. From the calculations, it was determined that 1.08 mL were to be added. 3M NaOH itself was a cloudy solution in appearance and upon the addition of 3M NaOH to the 2-methylphenol solution, it was noted a color change occurred and it became a yellow-green solution. Following this, the same calculations used previously, were used to determine the appropriate amount of sodium chloroacetate, which was found to be 0.38 g (3.26 mmol). Sodium choloroacetate was a white, crushed solid that was then combined with 1 mL of water and was swirled until the sodium chloroacetate completely dissolved. This sodium choloracetate solution was then transferred to the 2-methylphenol solution by the use of a medicine

The purpose of this experiment is to determine the nucleophilic strength of chloride and bromide ions as it reacts with 1-butanol (n-butyl) and 2-methyl-2-propanol (t-butyl alcohol) under SN1 and SN2 conditions.

In this experiment, two reactions were run to determine the molar absorptivity and the equilibrium constant of FeSCN2+. The main principles used in this lab are equilibrium, LeChatlier’s Principle, Beer’s Law and Spectrocopy. The first reaction was run to completion using LeChatier’s Principle and the second reaction was run to equilibrium. A spectrophotometer was used to measure absorbances. Using a graph of absorbance versus concentration of FeSCN2+ was used to determine that the molar absorptivity constant was 3670. Beer’s Law was used to determine that the average equilibrium constant was 33.1793.

The absorbance was then calculated, which was then used to calculate the concentration of the blue dye. The average concentration of blue dye was found to be 1.0 × 〖10〗^(-5) M. The initial concentration of 5.0 mL NaOCl solution was 1.34 M. The molarity of the diluted 50 mL sample of NaOCl was then found using the proportionality between the molarity and volume, equaling a molarity of 0.193 M. The ratio of blue dye to NaOCl was varied to examine the time in which the solution took to go from blue to colorless.

In day 2 of the experiment in step 1, two millitliters of 2% silver nitrate solution in ethanol were placed insix test tubes. Two drops of the six alkyl halides were added to the test tubes. The alkyl halides included, n-butyl chloride, sec-butyl chloride, t-butyl chloride, n-butyl bromide, allyl chloride, and chlorobenzene. Once the alkyl halides were added, the contents were swirled, and left alone to react. The t-butyl chloride, n-butyl bromide, allyl chloride, and chlorobenzene all reacted and precipitate was formed. It was observed that it took the t-butyl chloride 30 seconds to react and form a precipitate. It was observed that it took the n-butyl bromide four minutes to react, the allyl chloride 1 minute to react, and the chlorobenzene

As an enzyme-catalyzed reaction may be the main reason for a reaction to occur faster, many factors can

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

Determination of a Rate Equation Rate equation has the form rate = k [A]x[B]y which shows how the rate of a chemical reaction depends on the concentration of the reactants (A&B) and the rate constant k. The rate equation normally indicates what species are involved in the rate-determining step and how many species are involved. A rate equation is used to describe how the concentration of a product increases or the concentration of the reactants decreases with time, the equation also indicates how the concentration of one or more reactants directly affects the rate. Occasionally it can even be the concentration of a product that affects the rate.

In this lab a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.