The Effect Of Concentration On The Rate Of Reaction By Decreasing The Time

The importance of conducting this experiment is to discover the rate reaction of the Landolt Iodine Clock. This reaction is used to display the chemical kinetics in action, it was discovered by Hans Heinrich Landolt in 1886. It is where two colourless solutions are combined and no instant change appears but over a certain time delay depending on the factors it will instantly change to a dark blue. The Chemical kinetics of the reaction refers to the rate of the reaction. Different reactions occur at different rates, for example if it is a proton transfer reaction which is an acid-base reaction it will often occur at a faster rate. When the molecules collide in the reaction they must have a sufficient amount of kinetic energy so that the reaction can be initiated. The amount of kinetic energy is generally dependant on the temperature of the reaction, at higher temperatures there is a higher rate of reaction because of the increase of kinetic energy in the reactant molecules.

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

The purpose of this experiment was studying the reaction rate of crystal violet with NaOH by observing the concentration using the MicroLAB colorimeter, monitoring how the reactant concentration affects reaction rate constant, determining the reaction order, and to calculate the reaction pseudo rate constants and the true value rate constant. The rate of the reaction of crystal violet with NaOH is given by the generalized rate law, rate = k [OH-]x [CV]y where k is the rate constant for crystal violet and CV is crystal violet, C25H30N3+. Where x and y are the reaction orders. The equation can be rewritten as:

Abstract: This experiment helps determine the rate of reaction of crystal violet while it reacts with sodium hydroxide with respect to crystal violet. The amount of sodium hydroxide is varied in this experiment while crystal violet is kept at a constant. The transmittance of crystal violet is observed and recorded using a colorimeter and the data obtained is used to plot graphs which are manipulated using LoggerPro software to produce the desired outcome; rate of reaction of crystal violet. Upon completion of the experiment it was seen that the rate of reaction of crystal violet turned out to be 1

3. Please refer to the graphs at the beginning of the post-lab and question 2a. The effect of magnesium on a reaction rate depends on the magnesium’s shape and surface area, greater the surface area, the faster the reaction rate.

Enzyme concentration has a direct impact on the rate of reaction. When looking at graph 1 it is easy to see a linear relationship between the rate of formation of NADH and the concentration of the enzyme. As enzyme concentration increases the rate of reaction increases because substrates are more likely to collide with available enzymes. Le Chatelier's principle supports this as adding more enzyme will cause the reaction to shift more towards the enzyme substrate complex which will result in the rate of the reaction increasing. Based on this data we were able to choose the best enzyme dilution factor for the remaining experiments.

From the testing and results several major trends and relationships were discovered. The first observation, which supports the hypothesis, is the relationship between concentration of reactants and reaction rate. As concentration increased, the reaction rate also increased in direct proportion. This was shown by the results because when the concentrations doubled, from 0.1M and 0.125M to

In an unused well, place 8 drops of KI. Add 2 drops of HCl and 4 drops of starch to the KI solution. Add the standard number of drops of Na2S2O3 for this experiment. Swirl the solution by moving the well plate in a small circle. Draw up 0.4 mL of H2O2 and add to the solution. Swirl the solution and monitor the color while timing. Record the amount of time it takes for the entire solution to turn a dark blue-black color. Repeat this trial 3 more times while decreasing the concentration of the reactant KI. For the 2nd, 3rd, and 4th trials, use 6 drops of KI with 2 drops of distilled water, 4 drops of KI with 4 drops of distilled water, and 2 drops of KI with 6 drops of distilled water

The objective of this experiment was to determine the role of various chemicals in a reaction, to determine how concentration affects the rate of the reaction, and to determine how temperature affects the rate of the reaction.  Both concentration and temperature greatly affect the rate at which the reaction occurred, and changing the concentrations of the reactants or the temperature at which the reaction occurred changed how quickly the reaction took place.

Over the course of the second week of April, we have been trying to answer the question, “How much KIO3 do we need to use in order to make the reaction we have been producing occur within 25 seconds?” The reason we are determining this outcome, is partially because this experiment is included in our grade, but another reason to do this is because chemistry is all about numbers and mathematical formulas, which this covers. Plus if we ever want a job in kinetics we’ll have basic knowledge about how to go about it.

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

The experiment was carried out to investigate the effects of the increase in the enzyme concentration on the rate of reaction. By using self investigative and experimental skills, the experiment was done in order to determine how the rate of reaction will be altered, whether it will increase, decrease or remain constant when the different concentration of enzymes added.

To keep this a fair test I have made sure that the acid used is the

consumed. They have the ability to increase the rate of reaction in a chemical reaction. Catalysts achieve this by lowering the amount of energy required for a reaction to take place, which means that it occurs at a quicker rate. Potentially, molecules that would once have taken years to interact, can take seconds with the addition of a catalyst. The overall purpose of a catalyst is to ensure that reactions proceed effectively which is why a range of catalysts are commonly used in many elements of society. Common examples of where catalysts are used include; plastics, clean energy, converting energy sources to fuels, digestion and pharmaceuticals (Hamers, 2017).

On the first part, 2 beakers with different contents were prepared. 5 runs were prepared, and each run had different volumes of the substances. The different runs for the effect of Peroxodisulfate (VI) and iodide ion concentrations on reaction rate were presented on Appendix A. Each run had different concentrations of substances to test the effect of the change in amount of concentration to the rate of the reaction. Contents of beaker A and B were mixed; the timer was started immediately, and was stopped once a blue color appeared in the mixture. [7] Once Peroxodisulfate (VI) ions and iodide ions combine they produce I2 molecules which in turn reacted with the starch added to form a blue color. I2 reacted with the starch as fast as it was produced. Hence, it was very difficult to measure the rate of its reaction. So as to address the problem, S2O3 2- ion was added. This ion destroyed the I2 by reducing it back to I- as fast as it was produced. The amount of S2O32- ion added was just small so that it would not consume so much time. If the initial concentration of S2O32- ion was kept very small, Δ[S2O32-] would be small and Δ[S2O82-] would be even smaller. Consequently, there would be little change in the concentration of the reactants during the elapsed time Δt. This was a necessary condition for the initial rates method. The rate of the reaction was