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. Furthermore, two kinetic runs were setup; the first kinetic run had a solvent of 50% ethanol- 50% water, and the second run had a solvent of 40% ethanol- 60% ethanol. This caused the second solution to be more polar. A buret was filled with NaOH, and the initial volume …show more content…
These are both needed for the equation that will give the rate constant, k: ln([RCl]0 ÷ [RCl]t) = kt. The initial concentration was found with the formula [RCl]0 = (V ͚ - V0) , and the concentration at time t was found by [RCl]t = (V ͚ - Vt). These equations were derived after the reaction volume and NaOH concentration canceled out. Since the reaction was first order, plotting ln([RCl]0 ÷ [RCl]t) versus time, the slope will equal the specific rate constant, k. After plotting the data for both the kinetic runs, the second kinetic run had a greater rate constant of 0.0018 compared to 0.0007 in the first kinetic run. Therefore, the data reflected that the more polar solvent resulted in a faster reaction and a greater rate constant, which is characteristic of an SN1 reaction. The polar solvent solvates the carbocation, which lowers the energy and increases the stability of the carbocation. An increase in stability of the carbocation causes an increase in the rate of formation of the carbocation, therefore, increasing the rate of the reaction. Overall, the experiment was successful in testing the effects of solvent polarity, however some sources of error could have affected the data. For example, the recorded times of when the solution turned green or the amount of NaOH added could have been
That familiar fizzing you hear when you drop an Alka Seltzer tablet into a glass of water is the result of a chemical reaction, and chemical reactions are extremely prevalent when it comes to what living things do to carry out life processes. In addition, environmental conditions can alter the results of chemical reactions, and in this lab, we will be answering the
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 concentrations 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 reaction, there will be one reaction that is slower than the others.
Variables --------- During the experiments, the water will be heated using different spirit burners containing different alcohols. I will be able to change different parts of the experiment. These are the. Volume of water heated:
The goal of this experiment is to determine which products are formed from elimination reactions that occur in the dehydration of an alcohol under acidic and basic conditions. The process utilized is the acid-catalyzed dehydration of a secondary and primary alcohol, 1-butanol and 2-butanol, and the base-induced dehydrobromination of a secondary and primary bromide, 1-bromobutane and 2-bromobutane. The different products formed form each of these reactions will be analyzed using gas chromatography, which helps understand stereochemistry and regioselectivity of each product formed.
Anne Zhang 3/6/14 BSGE 7-1 Lab Report Problem Paragraph 1 Question: What is the effect of temperature on the dissolving time of an Alka-Seltzer? Alka-Seltzer is made up of baking soda, aspirin, and citric acid which gives the tablet the fizz when dropped in any temperature water. “Alka-Seltzer is a medication that works as a pain reliever and an antacid.
The rate equation is in terms of concentration over time and the reaction rate compares the increase/decrease
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
In this lab, it was determined how the rate of an enzyme-catalyzed reaction is affected by physical factors such as enzyme concentration, temperature, and substrate concentration affect. The question of what factors influence enzyme activity can be answered by the results of peroxidase activity and its relation to temperature and whether or not hydroxylamine causes a reaction change with enzyme activity. An enzyme is a protein produced by a living organism that serves as a biological catalyst. A catalyst is a substance that speeds up the rate of a chemical reaction and does so by lowering the activation energy of a reaction. With that energy reactants are brought together so that products can be formed.
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.
Almost every molecule in a solid moves, but it’s called a solid mainly because all of the molecules are very compacted and don’t have a lot of room to move.
The pH of the solution would alter the rate of the reaction if it was
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 temperature at which the reaction is carried out Use of a catalyst Reaction equation is mentioned above but rate equation can only be decided by doing experiments. So, the following procedure can be used to carry out the experiment. Plan Equipment 2 Measuring cylinders Beaker Stopwatch Paper with black cross on it Sodium Thiosulphate (different concentrations) Hydrochloric acid (same concentration each time) Water (different concentrations) Pipette. Prediction I predict that the greater the concentration of sodium thiosulphate solution, the faster the chemical reaction will take place.
In this experiment the Sodium Hydroxide solution went through three different phases where its quality and quantity changed. The first phase was called I. Preparing Approximately 0.1M NaOH, 1000mL of clear distilled water was boiled and then chilled to room temp.