Essay on Computerized Data Acquisition of a Second Order Reaction

If the concentration of the solution is increased the particles have less room to move around which creates a greater chance of collisions. The surface area of the reactant greatly affects the speed of which it reacts because if the reactant is grinded up or cut up the solution has more room to get to it. The reaction rate can be calculated by the formulae; rate of reaction = total amount of reactant used or product made ÷ time taken. (Collision theory and rates of reaction, 2013)

A reaction rate is the speed at which a chemical reaction occurs. The reaction rate is affected by surface area by increasing the more surface area there is, because there are more particles exposed to the other reactant. For example, if a solid is grinded into a powder, the reaction rate will be quicker as there is more surface area.

When the concentrations were changed so did the rate of reaction. When the concentration was changed to 0.265M the rate of reaction dropped by a factor of 0.5 (50%) below the control value. Furthermore when 60mL of water was added to the bleach dropping the concentration too 0.132M the rate dropped by a factor of 0.7 (70%).

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.

Please complete the entire experiment as instructed in the lab manual except for any modifications noted below. Fill out the

It must be noted that only the absolute value of the slope matters in this situation. Third order reactions have somewhat a similar story except they require a plot of 1/concentration versus time to determine rate of reaction. When all three graphs are plotted, the graph with the line of best fit, or the one in which all point seem to be on a straight line is the correct one for the reaction. This is easily drawn using the LoggerPro software. When all three graphs are drawn, the graph with the best fit line and lowest root mean square error, or the lowest deviation from the best fit line, is the graph to be used to determine reaction kinematics. This knowledge is acquired from the equations of the integrated rate laws which are explained in the textbook.

Each solution contained different concentrations as follows: 0.005 mg/mL, 0.010 mg/mL, 0.015 mg/mL, 0.020 mg/mL, and 0.025 mg/mL. Each solution needed to have a volume of 10 mL. Before adding the different concentrations of Coomassie Blue into their separate tubes, the formula C1V1= C2V2 was used in order to determine how much stock solution is needed for the five dilute solutions. Once that number was calculated, a pipette was used to add the amount of stock solution needed for each tube. We then subtracted the amount of stock solution from 10 mL to determine the amount of H2O needed. The calculated amount of H2O was then added to each tube of solution. After doing that, a spectrophotometer was used to determine each solution’s relative absorbance. However, before that, we first had to calibrate the spectrophotometer before determining each solution’s relative absorbance. In order to calibrate the spectrophotometer, a disposable culture tube filled with distilled water was used. We then changed the data rate to 100 and removed the tube with water. In order to determine the relative absorbance, the relative absorbance had to be at 595 nm. Also, during this experiment, an unknown dilution was given to us by the lab instructor. We determined the relative absorbance by using the spectrophotometer and then recorded the results. The procedures for this experiment can be found on page 8 of

9. Does temperature have any effect on reaction rate? If so, why does it occur?

Abstract The purpose of these experiments is to find how the molecular components are affecting the macroscopic color of the solutions by recording the emission and absorbance spectrums for each solution. These experiments will help specify characteristics of the solution: its molecular and/or compounded configuration. Knowledge about the emission and absorbance information for the molecular composition allows for an identification to be made about the molecules or compounds within the solution, which then can be used to narrow down the possibilities for the solutions. The experiments will be conducted by observing the burning of the solutions to create emission spectrums and analyzing the solutions with a spectrophotometer to create the absorbance spectrums.

However, the rate of reaction only increases for a certain period of time until there is lesser substrate molecules than the enzyme molecules. The increase of enzyme concentration does not have effect if there are lesser substrate molecules than enzyme molecules initially.

1. The concentration within a reaction is determined by the rate of concentration fluctuations of both sides of the reaction. Increasing the quantity of the species, that is the molarity of the subject system, increases the rate of reaction. This happens by adding more of a species to a consistent volume increasing the probability of collisions. By Adding more of a constituent, you decrease the probability of both of the constituents not interacting. It could be the case that changing these concentrations, in comparison to others, could have a relatively more exponential amount of impact on the equilibrium. By either increasing the amount of either the products or reactants, you incite the system to proportion them to the previously consistent

Review 2: Text In chemical kinetics, the reaction rate law is calculated experimentally to find how change in concentration affects change in rate, and to find a proportionality constant k, known as the rate constant. Since the instantaneous initial rates at various concentrations of A and B are provided, we must find the orders m and n of each reagent to determine the rate law, Rate=k[A]m[B]n. When A is doubled and B is held constant, the instantaneous initial rate approximately quadruples.

Incorporation of assay controls included setting up a spectrophotomer and running the chart recorder with a full-scale deflection before the start of the assay. The set recorder had a corresponding value of 1 for the change in the absorbance. Therefore, prior testing was done to observe whether a change occurred in the readings. This helped to indicate that the results were valid, as they could have been affected by a fault during the setting up of the spectrophotometer. On the other hand this was considered as one of the controls for the experiment. Nevertheless, a new cuvette had to be used for each assay.

As this investigation intends to find a rate law that represents this chemical reaction, equilibria reactions must first be understood. Equilibrium reactions react stoichiometrically before reaching a point where the amount of product and the reactants being used/produces reaches a steady state. Where, the rate at which the products are being produced is the same as the rate at which the products are reverting back into the reactants. This is exemplified by the graph below, the point at which the lines have a gradient of 0 is the point of equilibria.

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.