Lab Report Kinetics of Chemical Reactions 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. Two catalyst reactants are used in the experiment, thiosulfate and starch, to dictate the time of reactions. The order with respect to Fe+3 and I- is also determined by graphing the slope of the log rate initial as a function of the log (Fe+3) or (I-). The activation energy is also graphed with the rate constant as a function of the inverse of the temperature. Procedure The volumes of solutions were obtained and placed into two separate beakers as shown in the tables below. Reagent Fe+3 HNO3 KI S2O3-2 Starch Volume needed 150 mL 150 mL 100 mL 100 mL 50 mL Beaker 1 Beaker 2 Combo .04 M Fe+3 .15 M HNO3 H2O .04 M KI .004 M S2O3-2 Starch H2O 1 10.00 20 20 10.00 10.00 5 25 2 20.00 10 20 10.00 10.00 5 25 3 30.00 0 20 10.00 10.00 5 25 4 10.00 20 20 5.00 10.00 5 30 5 10.00 20 20 15.00 10.00 5 20 Part A: The two beakers were allowed to chill for 15 minutes. Their contents were then mixed and put back on ice. Combination #1 was run at room temperature on a separate trial. The temperature was recorded at 23 0C. When the solution turned blue, the time was recorded. Finally, combination #1 was run at 45 0C and the solution was monitored until it became blue. Part B: Combinations #2 - #5 were all run at room temperature. The temperature varied slightly for each combination... ... middle of paper ... ...I- rate initial log I- initial Log rate initial 1. .004 2.03 x 10-6 -2.40 -5.69 4. .002 5.94 x 10-6 -2.70 -6.23 5. .006 4.01 x 10-6 -2.22 -5.40 A) Order of reaction with respect to [Fe+3] » 1 B) Order of reaction with respect to [I-] » 2 C) Rate law = K [Fe+3]1 [I-]2 2.03 x 10-6 = K [.004]1 [.004]2 K = 31.7 M-2s-1 D) ln K = ln 31.7 = 3.46 Rate initial for hot and cold: HOT: Rate initial = ½ (.0004) / 5.22s Rate initial = 3.83 x 10-5 3.83 x 10--5 = K [.004]1 [.004]2 K = 598 M-2s-1 COLD: Rate initial = ½ (.0004) / 2043.47s Rate initial = 9.79 x 10-8 9.79 x 10-8 = K [.004]1 [.004]2 K = 1.53 M-2s-1 1/T ln K Cold .00364 .425 Room .00338 3.46 Hot .00315 6.39 Ea M = - Ea/R M = -18001 -Ea = -18001 x .008314 -Ea = -149.7 Ea = 149.7 kJ
However, only experiments IV “Effect of Copper Metal” and V “Effect of Temperature” had reasonable results, so copper metal and temperature are the more effective factors. The less effective factors are the changes in concentrations of "H" ^"+" ions and "C" _"2" "O" _"4" "H" _"2" particles. This observation is represented in experiments II “Effect of "H" ^"+ " Ions” and III “Effect of "C" _"2" "O" _"4" "H" _"2" Concentration.” Both runs 2B and 2C had the fastest times of 25 seconds and 86 seconds
Abstract: This week we experimentally determined the rate constant k for the reaction 2HCl (aq) +Na2S2O3 (aq) → S (s) + SO2 (aq) + H2O (l) + 2NaCl (aq). In order to do this the average reaction time was recorded in seconds during two trials. The data from the experiment shows this reaction is in the first order overall: rate=.47s-1 [HCl]0 [Na2S2O3]1. These findings seem to be consistent with the expected results
*The left side of the equation will represent the data from the experiment, and the right side represents our hypothetical calculations. By plugging in either 65°C or 0°C (depending on if were solving for the hot or cold pack), and the...
The fifth experiment of the semester entails a synthesis reaction geared towards analyzing the structure of a product. The starting material is isopentyl alcohol. When reacted with acetic acid with sulfuric acid as a solvent, isopentyl alcohol produces isopentyl acetate, which is the goal product, as shown in the reaction below:
Obtain 200 mL of the sodium thiosulfate solution in a 250 mL beaker, 400 mL of the bleach solution in a 600 mL beaker, and prepare the solutions for the experiment. Using a graduated cylinder, measure 25 mL of the bleach into the beaker very precisely and pour it into a small Styrofoam cup. To help stabilize the cup, rest it inside of a beaker. Next, measure out 25 mL of the thiosulfate solution in a different or clean graduated cylinder.
Over the observed fifty seconds, there was a consistency among the temperatures. Without a calculated percent error, we are able to assume the average temperature was twenty-six degrees Celsius. There are factors that could have caused error to arise in our data collection. One factor could be that the temperature of the room was not consistent throughout the room. Another factor may have been the performance of the thermometer. The grasp in which the thermometer was held for procedure B may also be a factor.
...e will also become faster. In phase one, Nature of the Reactants five different metals were placed in the 2M HCl they all reacted differently with magnesium being the most reactive and copper being the least reactive. In phase two, Concentration, zinc was placed in different concentrations of 6M HCl. The higher the concentration was the more reactive the metal was. Next in phase three, Temperature, zinc was added to 6M HCl which was a different temperatures and the zinc was the most reactive with the HCl in the boiling water and least reactive with the HCl in the ice bath. Then in phase four, Surface Area, the powered zinc was more reactive then the piece of zinc in the 6M HCl because it had more surface area to be covered than the piece of zinc. Lastly in phase 5, Catalyst, the 3% H_2 O_2 was reactive with the 5 drops of 〖FeCl〗_3 but not with the 5 drops of water.
Put 300 grams of ice each into 4 different 1000mL beakers. Add 0 grams of salt into the first beaker. Add 30 grams of salt into the second beaker. Add 60 grams of salt into the third beaker. Add 90 grams of salt into the fourth beaker. Put a thermometer with starting temperature of 21°C into each beaker. Record the temperature every minute for 10 minutes. Repeat the trial 5 times.
The purpose of the experiment is to identify and understand reactions under kinetic and thermodynamic control. A reaction under kinetic and thermodynamic control can form two different types of products. A reaction under kinetic control is known to be irreversible and the product is formed quickly. A reaction under thermodynamic control is known to require rigorous conditions. It is also reversible. The final product is more stable than the product made by kinetic control. The chart below shows the two types of reaction coordinates:
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
The aim of this investigation is to: 1) find the rate equation for the reaction between hydrogen peroxide, potassium iodide and sulphuric acid by using the iodine stop clock method and plotting graphs of 1/time against concentration for each variable. Then to find the activation energy by carrying out the experiment at different temperatures using constant amounts of each reactant and then by plotting a graph of in 1/t against I/T, 3) to deduce as much information about the mechanism as possible from the rate equation.
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
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.
- Temperature was measured after and exact time i.e. 1 minute, 2 minutes, 3 minutes.
To control the rates of chemical reactions is imperative to the continued existence of our species. Controlled chemical reactions allow us to move forward in society, constantly. We find new ways to provide light and heat our homes, cook our food, and pursue in crafts that benefit our society. There are, however, just as there are advantages, disadvantages to the efficiency of controlling the rate of reactions, which in some cases can be fatal to our scientific development and progression. The growth of humankind necessitates that we must be able to control the rate of chemical reactions.