The purpose of this investigation was to test the hypothesis that if a solution is more concentrated, then the reaction time of a chemical reaction including that solution would decrease because there would be less water molecules in the way of the two combining solutions. The results of this investigation do support the hypothesis. There were three tests in this investigation. The first test or the control test consisted of combining 10 mL of KIO3 and 10 mL of NaHSO3, in which the KIO3 had a molarity of .02. The second test consisted of combining 5 mL of water and 5 mL of KIO3 to create a .01 M KIO3 solution, which then combined with 10 mL of NaHSO3 . Lastly, the third test consisted of combining 3 mL of KIO3 and 7 mL of water to create …show more content…
For example, the difference in average reaction rates of the highest concentration, 5 seconds, compared to the lowest concentration, 32.5 seconds, was 27.5 seconds. This means it took an average of 27.5 seconds more for the .0085 M KIO3 solution to react compared to the .02 M KIO3 solution, which suggests that as the concentration of the chemical increased the reaction rate of the chemical reaction including that chemical decreased. It is possible that as a chemical becomes less concentrated by dilution, the water molecules may get in the way of the two combining chemicals. As a result, the rate of the reaction would decrease. The results of this investigation showed a significant increase in the rate of the reaction as the concentration of the KIO3 solution decreases, this suggests that the more concentrated a solution is, the faster a chemical reaction will be if that reaction includes that solution. Therefore, the hypothesis that if a solution is more concentrated, then the reaction time of a chemical reaction including that solution would decrease was
The purpose for this experiment was to determine why it was not possible to obtain a high percent yield when Calcium Nitrate Ca(〖NO_3)〗_2 with a concentration of 0.101 M was mixed with Potassium Iodate KIO_3 with concentration of 0.100 M at varying volumes yielding Calcium Iodate precipitate and Potassium Nitrate. Filtration was used to filter the precipitates of the solutions. The percent yield for solution 1 was 87.7%, and the percent yield for solution 2 was 70.8%. It was not possible to obtain a high percent yield because Calcium Iodate is not completely soluble and some of the precipitates might have been rinsed back to the filtrates when ethanol was used to remove water molecules in the precipitate.
This experiment studied the kinetics and the effects of solvent polarity of a solvolysis reaction. This reaction is a SN1 reaction in which the solvent (water) is the nucleophile. The reaction begins with the removal of a chloride ion; this is the rate determining step (slow step). Water is then added to the carbocation, forming a protonated alcohol. Lastly, a proton is removed by the present base. Since the first step is the rate determining step, it is a first-order reaction.
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
2. In order to determine how fast a reaction is occurring there must be a basis for measurement. There must also be an indicator substances to determine the change that took place. Then there must be a tool to measure the change. In this lab a spectrophotometer was used. The ABS value is the actual value and it is used to determine the rate of change.
will result in an increase in the speed of the rate of reaction it has
Investigating the Factors Influencing the Rate of Reaction Between Sodium Thiosulphate and Dilute Hydrochloric Acid
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.
The concentration is the amount of particles in a certain amount of water. If a cross is placed under the beaker of the solution, the cross will eventually disappear because the high temperature of the water will make the particles move faster because they have more energy and they will move more quicker to give a bigger impact which will cause more frequent and violent collisions and the solution will disappear as the product forms to create a misty solution. The rate of reaction is normally recorded in tables and can then be defined onto graphs to show how the rate curves of different factors affect the speed of the reaction. A rate curve is the curve of a graph that shows how the reaction changes at different intervals.
The first experiments investigate the order of reaction with respect to the reactants; hydrogen peroxide, potassium iodide and sulphuric acid by varying the concentrations and plotting them against 1/time. An initial rate technique is used in this experiment so ‘the rate of reaction is inversely proportional to time.’ To find the order of reaction in respect to the reactants, 1/time is plotted against the concentration of Hydrogen Peroxide using the equation:
The pH of the solution would alter the rate of the reaction if it was
Investigating the Effects of Temperature on the Rate of Reaction between Magnesium and Hydrochloric Acid Introduction Chemical kinetics is the study and examination of chemical reactions regarding re-arrangement of atoms, reaction rates, effect of various variables, and more. Chemical reaction rates, are the rates of change in amounts or concentrations of either products or reactants. Concentration of solutions, surface area, catalysts, temperature and the nature of reactants are all factors that can influence the rate of reaction. Increasing the concentration of a solution allows the rate of reaction to increase because highly concentrated solutions have more molecules and as a result the molecules collide faster. Surface area also affects reaction rate because when the surface area of a reactant is increased, more particles are exposed to the other reactant.
One vital process in the human body observed in chemistry is the idea of chemical kinetics. Chemical kinetics is the study of the rate of reactions, or how fast reactions occur.1 Three factors that affect chemical kinetics are concentration, temperature, and catalysis. As the concentration of a substance increases, the rate of the reaction also increases.1 This relationship is valid because when more of a substance is added in a reaction, it increases the likelihood that the
acid and water to see how it affects the rate of reaction. I will use
In order for KNO3 to be dissolved, it must come into contact with
has on the rate of reaction. I will do this by recording the time it