Madison McVeyCHEM 237 – 549December 1, 2016Kinetic Study of Sn1 Solvolysis Lab ReportResults and Discussion:In this lab, students calculated the rate of reaction of two different kinetic runs using their concentrations. The first run was a 50% ethanol, 50% water solution and the second was a 40% ethanol, 60% water solution. The rate constant was found from the slope of the line formed when the natural log of concentration was plotted against time. The rate constant found for the first run was 0.0006 and the rate constant for the second run was found to be 0.0017. The graphs obtained are attached to this report. From the data above, it is obvious that the kinetic run involving the 40% ethanol, 60% water solution reacted faster than the solution that contained 50% ethanol and 50% water. This is because the water is more polar than ethanol and in an Sn1 reaction, a polar solvent aids in the dissociation of the alkyl chloride by stabilizing the carbon cation and lowering the energy of the transition state. Becausethe polarity of water is greater than that of ethanol, it is logical that the solution witha higher percentage of water had a faster reaction rate. Potential errors that occurred in this experiment include the quick reaction time, which could lead to incorrectly reported times, thus effecting the rate of reaction. Though the results of the experiment proved the experiment successful and supported known facts regarding the Sn1 reaction, the data and analysis could be slightly skewed because of this.0 100 200 300 400 500 60000.20.40.60.81f(x) = 0x − 0.04Kinetic Run #2: 40% Ethanol, 60% Waternatural log of con-centrationLinear (natural log of concentration)time in secondsln of concentration0 200 400 600 800 1000 120000.10.20.30.40.50.60.70.8f(x) = 0x − 0.03Kinetic Run #1: 50% Ethanol, 50% Waternatural log of con-centrationLinear (natural log of concentration)time in secondsln of