Kinetics

The Blue Dye #1 reaction can be determined by utilizing Beer’s Law, and First and Second order integration. Beer’s law is first used to calculate the molar absorptivity of the Blue #1 dye. Beer’s law states that the concentration of the Blue #1 Dye is directly proportional to the absorbance of the solution. The molar absorptivity, e was calculated to be 9.63x104 and will be used when calculating the activation energy of the reaction. First, the rate order for both the Blue #1 and Bleach needed to be determined. A known concentration of both Blue #1 dye and bleach are needed to conclude the rate order of the solutions because the rate order is dependent on the concentration of the solution used. The absorbance versus time is plotted and from

Purpose: The purpose of this experiment is to use kinetics to study a solvolyis reaction

Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction:

An experiment was done to determine the concentration of Allura Red in a commercially available beverage, Gatorade. This was done by using the colorimeter, the absorbance of five Allura Red solutions were measured. The graph obtained demonstrated a linear relationship and the equation obtained yielded a concentration of 1.9910-6M.

A = Absorbance difference  = Molar extinction coefficient C = Concentration L = Path length

The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.

Beer’s Law is a direct liner relationship between the absorbance of light are a selected wavelength and the concentration the absorbing species in the solution. (Sullivan 241). Beer’s Law shows a relationship between several concentrations. To determine if the determine our data consistent with Beer’s law, we will plot a graph of absorbance versus concentration with a linear regression

Kinetic Energy is the energy of movement, whether it is horizontal or vertical, it’s kinetic. There is many different types of kinetic energy. There is; vibrational, rotational and translational (the movement from one location to another. IN our experiment we also have kinetic energy. The particles that move around need kinetic energy to bond because if the particles wouldn’t have kinetic energy, they wouldn’t move, then they wouldn’t be able to collide and at last there would be no chemical reaction taking place. But for a reaction to take place there has to be enough kinetic energy to overcome the bonding forces of the reactants. The minimum amount of kinetic energy need to cause a chemical reaction is called activation energy (symbol: Ea

3 because this is the maximum absorbance for the iron (III) ion. The Beer's Law Plot that was graphed came out to be linear with an equation of:

From the graph, R2 can be extrapolated from the y-axis and the corresponding value on the x-axis (the point of intersection on the curve) gives the concentration of the unknown solution.

In this experiment, the purpose was to determine the rate law for the reaction of crystal violet and sodium hydroxide. By recording the absorbance in a calorimeter in increments of twenty seconds for twenty minutes, three graphs were constructed. From the ln(absorbance) vs. time plot, the reaction was determined to be first order with respect to crystal violet. Based on the data, the rate law for the reaction is concluded to be "rate= k [crystal violet]" .

Introduction: On the word of Shelton (2018) in the General Chemistry Ⅱ Lab Manual, “Kinetics is the study of the rates which chemical reactions occur at. The rate of reaction is dependent upon the change of concentration over the change in time” (p. 14). The objection of this lab was to establish the order of reaction with respect to persulfate ion and the overall rate constant. Experimental Procedure:

The same solution of 0.5 ml BSA was then added from test tube 1 to the test tube 2 after being properly mixed, and from test tube 2 the solution was being added to test tube 3, and so forth all the way up to test tube 5, with the same exact procedure. From the last tube, we then disposed the 0.5 ml solution. After above procedures, we now labeled another test tube “blank”; 0.5 ml blank distilled water was purred into the tube with the serial dilution of 1:10. We also had a tube C labeled “unknown” with the same 0.5 ml of solution. And after adding 5ml of Coomassie Blue to each tube (1-5) and to the blank, the result of absorbance was read at 595 nm.

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

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.