Of The Rate Of Reaction Of Peroxydisulfate Ion With Iodide Ion

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 the experiment we used Turnip, Hydrogen Peroxide, Distilled Water, and Guaiacol as my substances. On the first activity, Effect of Enzyme concentration of Reaction Rate for low enzyme concentration, we tested three concentrations of the turnip extract, and hydrogen peroxide. For the Turnip Extract I used 0.5 ml, 1.0 ml, and 2.0 ml. For hydrogen peroxide we used 0.1 ml, 0.2 ml, and 0.4 ml. We used a control to see the standard, and used a control for each enzyme concentration used. The control contains turnip extract and the color reagent, Guaiacol. We prepared my substrate tubes separately from the enzyme tubes. My substrate tube

Students will place a potato cube into a test tube and add 3 ml of H202 into each tube. Then students will wait one minute and record the height in cm of the bubbles and rate how rapidly the solution bubbles on a scale of 0-5. (0=no reaction, 1=slow,……. 5= very fast.)

There are three stages of the overall reaction. Reaction 1 is the rate determining reaction whereby iodide ions from Potassium Iodide (KI) are oxidised by Hydrogen Peroxide (H₂O₂) in an acidic solution. This reaction utilises the Hydrogen ion from Sulfuric acid (H₂SO₄) to form triiodide ions and water as products (B Z. Shackhashiri, 1992).

The rate of a chemical reaction often depends on reactant concentrations, temperature, and if there’s presence of a catalyst. The rate of reaction for this experiment can be determined by analyzing the amount of iodine (I2) formed. Two chemical reactions are useful to determining

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

Lab six requires students to observe the effects of pH and enzyme concentration on catecholase activity. Enzymes are organic catalysts that can affect the rate of a chemical reaction depending on the pH level and the concentration of the enzyme. As pH comes closer to a neutral pH the enzyme is at its greatest effectiveness. Also at the absorbance of a slope of 0.0122 the enzyme is affected greatly. The pH effect on enzymes can be tested by trying each pH level with a pH buffer of the same pH as labeled as the test tube and 1mL of potato juice, water, and catechol. This is all mixed together and put in the spectrophotometer to test how much is being absorbed at 420nm. As the effect on enzyme concentration can be tested almost the same way. This part of the exercise uses different amounts of pH 7-phosphate buffer and potato juice, and 1mL of catechol mixed together in a test tube. Each substance is put in the spectrophotometer at a wavelength set tot 420nm. The results are put down for every minute up to six minutes to see how enzyme concentration affects reaction rate. The results show that the pH 8 (0.494) affects the enzyme more than a pH of 4 (0.249), 6 (0.371), 7 (0.456), and 10 (0.126). Also the absorbance is greatest at a slope of 0.0122 with test tube C that has more effect on the reaction rate, than test tube A, B, and D.

By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions, then the concentration of Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking place. From these results, I hope to draw conclusions as to the effects of these changes to the environment of the reaction on the rate and also determine the order of the reaction and the activation enthalpy.

The research question for the Alka Seltzer Lab is, “What is the effect of different surface areas of an Alka Seltzer tablets reaction time?’. Inside of an Alka Seltzer tablet there are two key ingredients; which are citric acid and baking soda. When a tablet is dropped into a liquid, the acid and baking soda show a physical reaction of fizzing and eventually dissolving. Materials needed for this lab was goggles, aprons, beakers, water of the same temperature, mortar pestle, and three alka seltzer tablets. In each beaker there was 150 mL of water. The first tablet was a full tablet, the second was broken into quarters, and the last tablet was crushed in a mortar pestle. The dependent variable of the lab was the rate of reaction, and the independent

In the Making Maalox Chemical Reaction Lab, the six main purposes of the lab are producing the solids magnesium hydroxide and aluminum hydroxide the active ingredient in Maalox, to be able to provide visual evidence of changes in properties, to be able to observe changes in energy, noting the type or classification of chemical reaction and use balanced equations, use pH indicators to identify products as acids or bases, and lastly to explore what happens when you add an acid to a base. The reactants that we will be using are alum, ammonia in a dropper bottle, epsom salt, cabbage juice, and water. The products that we will be getting are aluminum hydroxide, magnesium hydroxide, and a simple version

This experiment will measure the rate of oxidation of iodide ions by persulphate ions to derive the rate law for the reaction. Starch will be added to the reaction to facilitate the measure of time during the reaction. The reactant solutions will contain (NH4)2SO4 and KI, represented as:

By alternating between different mixtures and concentrations of the reactants and measuring the time it takes for the solution to turn blue-black, which comes as a result of the I2 interacting with the starch, the dependence of the reaction rate of the concentration can be shown. With a greater concentration of the reactants, H2O2, I-, and H+, in the reaction, the time needed for the color to change was less. The individual orders for H2O2, I-, and H+ are 1, 2, and 2 respectively. The overall order of this reaction is 5, and the average rate constant is (k = 0.0544).

Purpose: To investigate the kinetics of the reaction between persulfate and iodide ions, the effect of reactant concentration and temperature on the rate of the reaction, and to determine the effect of ionic strength of the solution. The activation energy (Ea) and rate constant, k are also determined. Introduction: The persulfate-iodide clock reaction is an experiment that is used to show chemical kinetics in action. In this reaction, ammonium persulfate was used to oxidize iodide ions to iodine, and sodium thiosulfate was used to reduce iodine back to iodide.

To vary the concentrations of each reactant along with the sulphuric acid in order to observe and measure its effect on the overall rate of reaction in absorbance using colourimetry.

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.