The Concentration Of Reactants During The Fastest Rate Of Reaction

Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60.62 KJ/mol.

The results for the rate of reaction, as seen in Table 2, suggest that as the temperature increases, the rate of reaction increases at a progressively greater rate. When the temperature increases 21℃ from 4℃ to 25℃, the rate of reaction increases from 1.846 s-1 to 6.1100 s-1 while a similar increase in temperature from 25℃ to 65℃ has a much more significant difference in the rate of reaction: 47.85s-1 at 65℃.

This image explains that the higher the temperature, the concentration, and the pressure the faster the rate of the reaction is.

The work resulting from this branch of science has led to the conclusions that some chemical reactions proceed in a single step while others such as the Landolt Iodine Clock undergo multiple phases. By measuring the rate of a reaction it can be determined whether the reaction occurs in one or more steps (Laidler, 2008). Specifically, the rate of a reaction is the speed at which the reactants become products, and is affected by multiple factors including temperature, surface area, catalysts and concentrations; the higher the concentration of a substance, the faster the rate of the reaction (Science Buddies, 2018). The relationship between the rate of a reaction and the concentration of the reactants is demonstrated through a rate law.

In this experiment we tested the effects that enzymes and substrate have on chemical reaction rates, which is the rate at which chemical reactions occur.. This experiment tested how different concentrations of enzyme and substrate affected the light absorption measurements on a spectrophotometer. The experiment also tested how temperature affected the light absorption, and in a separate test, the effect of the enzyme inhibitor hydroxylamine was also tested. In the first test conducted, 3 different concentrations of enzyme, and three different concentrations of substrate were measured in a spectrophotometer. For the enzyme and the substrate, the measurements got higher as the concentrations were higher, but the over measurements of the substrate were smaller than those of the enzyme. In the second test conducted, the medium concentration enzyme was tested under the temperatures; 4°C, 23°C, 37°C, and 60°C. The measurements in this test got higher as the temperature got higher, but did the measurements under 4°C were overall significantly higher than the other temperature measurements. Lastly, the last test conducted showed that the measurements of the substance with 0 and 1 drop of hydroxylamine inhibitor went up, but the measurements of the enzyme with 5 drops of hydroxylamine inhibitor stayed rather low and did not change much. In conclusion, these experiments showed that chemical reaction rates are sped up with higher concentrations of enzyme, substrate,

The purpose of this lab is to calculate the overall order of an unknown rate law equation. The lab is also performed to create the rate law of the equation. This is done through varying the amount and concentration of the reactants in the equation. These two variables can have a drastic impact on the speed that the reaction develops at It also does this by varying the dependence of the reactants throughout the trials. The order of the equation is found by finding the correlation between the concentration of the reactants and the reaction rate. Determining this makes it clear which reactants affect the speed at which the reaction develops: whether they have no effect, slow the reaction down, or speed it up. From this experimental data

Temperature, a solution’s concentration, reactant’s surface area and whether a catalyst is in effect, all affect reaction rate. When the temperature is increased increases the speed of the molecules, which will speed up the reaction rate, as the molecules will collide more often. When concentration is increased, molecules have restricted room to roam which brings about a greater chance of collisions. The reaction rate is also greatly affected by the surface area, as the

This transformation relies on the amount of activation energy for the particle to form a new product, and the orientation at which the particles collide. There are several factors that can affect reaction rates within aqueous solutions including temperature, concentration, particle size and catalysts. Temperature affects the rate of reaction of a solution by adding heat which speeds up the particles within the solution or by slowing the particles down through the cooling of the reaction. Concentration also has a large impact on the rate at which a reaction occurs because of the change in the number of particles in the solution. By increasing the concentration of the reactants the collision frequency also increases which escalates the rate at which products are being formed. Decreasing the number of particles in the solution also will decrease the speed with which products are created. Once a reaction between substances has fully occurred, a dynamic equilibrium is established. Although in a dynamic equilibrium the concentration of the reactants appears to be unchanged, a reaction still occurs with the forward reaction rate being equal to that

According to the collision theory, the rate of a reaction depends on the frequency of collisions between reacting particles. The more frequent the collisions, the faster the rate of the reaction. However, in order for the collisions to be effective, the particles must collide with sufficient energy (activation energy). Furthermore, the particles must collide with the proper orientation.

The effects temperature ,we all the basic as temperature increases so does the movement in the molecules which means as you increase the temperature the rate of reaction increase as well. For most reactions that happen around room temperature which is about 70 degrees Fahrenheit ,for every approx.10 degrees Celsius the rate of reaction doubles. The rate of reaction is calculated using the the Arrhenius rate equation . The Arrhenius rate law is “an equation describing the mathematical relationship between temperature and the rate of reaction ” ."K=A*exp(-Ea/R*The equation relates k, the rate constant for a given chemical reaction, with the temperature, T, the activation energy for the reaction, Ea , the pre-exponential factor A, and the universal gas constant, R. High temperature and low activation energy favor larger rate constants, and therefore speed up the reaction". Source: Boundless. “The Arrhenius Equation.” Boundless Chemistry. Boundless, 20 Sep. 2016. Retrieved 04 Nov. 2016 from

The reaction rate is defined as, the speed at which a chemical reaction proceeds. It is often expressed in terms of either the concentration (amount per unit volume) of a product that is formed in a unit of time or the concentration of a reactant that is consumed in a unit of time (according to Britannica Online Encyclopedia). But not only concentration affects the reaction rate, temperature also affects the rate. The Kinetic Molecular Theory is described as a gas that has a large number of submicroscopic particles (atoms or molecules), all of which are in constant rapid motion that has randomness raising the collisions with each other and with the walls of the container. All chemical reactions proceed in different ways according to their reacting substances, types of chemical transformation, and temperature. In this lab, we tested the effects of

Increasing enzyme concentration increases reaction speed. This is due to the maximum velocity level in which the enzyme is able to be active. As the enzyme concentration increases it compensates for the amount of restriction factors such as temperature, pH and substrate levels; all of which increases their effectiveness due to an imbalance in substrate (Eed, 2013). This was shown using an increased Pyrosphosphatase concentration throughout the experiments. As shown in figure 1, the enzyme hydrolysis rate increased in accordancce to increased concentration level(Chou, 1974). Throughout the experiments, the volume solution was the same ,while increasing the enzyme amount (Pyrosphosphatase).

The data supports the hypothesis that an exponential relationship will be found between the change in temperature and the reaction rate, and that the highest temperature will have the fastest rate of reaction. The data also supports the hypothesis that as the concentration of Potassium Iodine increases so will the reaction rate, and vice versa for an increase in Sodium Thiosulphate concentration. The hypothesis that the Iron (II) ions will affect the reaction rate, and that the optimal amount will be about 0.1M of catalyst was partially supported.

The purpose of this experiment was to measure and interpret the effect of a chemical concentration on a reaction rate. A collision theory is a theory proposed by Max Trautz and William Lewis that states: qualitatively explains how chemical reactions occur and why reaction rates differ for different chemical reactions (Wikipedia, 2015). An example of collision theory is when two motor vehicles collide with one another creating a large impact as the particles combine with one another due to the large impact created. A chemical reaction is a process that involves the rearrangement of the molecular and ionic structure of a substance when the interaction of two or more chemicals is compounded to create a new substance (Middle School Chemistry, 2015). An example of a chemical reaction is when a bike begins to rust or when photosynthesis takes place (Uen.org, 2015). The different types of Molars used in the experiment affected the speed of the reactions of the acid. These times varied on the amount of concentration used in the molars. This was shown in the results of the experiment as the 2Molar gave an average time of 23.88 seconds, for the water to decrease to 30 ml in the test tube. The 1Molar gave an average 54.94 seconds to reach 30 ml of water in the test tube, and the 0.5Molar displayed an average time of 3 minutes 13 seconds to reach 30 mL.

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.