Data, Calculations and GraphsBy signing below, you certify that you have not falsified data, that you have not plagiarized any part of this lab report, and that all calculations and responses other than the reporting of raw data are your own independent work. Failure to sign this declaration will cost you 5 points.Signature: Purpose and MethodPart I: Clock Reaction (3 pts) (purpose, reactions/rate law, method)The purpose of the first section is to determine the rate of the reaction: BrO3(a) + 6I(aq) + 6H(aq) --> Br(aq) + 3I(aq) + 3H2O(aq). We want to determine the order of the reaction with respect to each reagent, e want to determine the rate constant (k) at room temperature (about 25 degress celcius) and at 0 degress celcius, determine the activation energy (Ea), and determine the effect of a specific catalyst on (k) and (Ea). There will be reactions in test tubes with the following species: H2O + Na2S2O3 + KI, KrBrO3 + HCl + starch, and color comparison solution. This will run for fifteen runs (varying the amount of each species) and then for the 13th, 14th, and 15th run, they will be kept in an ice bath. The reaction for this part of the lab is BrO3-(aq) + gI-(aq) + 6H3O+(aq)-->Br-(aq) + 3I2(aq) + 9H2O(l) with another reaction of I2 + 2S2O3 2-(aq)--> 2I-(aq) + S4O6 2-(aq). We will determine the rate law using the equation rate=k[BrO3-]b[I-]i[H3O+]h to determine the value of k. After we calculate kwe can use the Arrhenius equation k=Ae^(Ea/RT) to find Ea using a form of the equation ln(k2/k1)=(Ea/R)((1/T1)-(1/T12)) to find the activation energy.Part II: Crystal Violet-Hydroxide Reaction (3 pts) (purpose, reactions/rate law, method)The purpose for the second part of the lab is to use the reaction CV(+) + OH(-) --> CVOH to find the order of the reaction with respect to CV(+), determine the order of the reaction with respect to OH(-), and to find the rate constant (k) at room temperature. We set up an instrument to measure absoorptivity of CV(+) with variations of concentrations of OH(-). A 9x10^-6 M solution is made by diluting a 7.5x10^-5 M CV+ solution with DI water. This was repeated for 2, 3, 4, and 5 ml of CV+ solution. We then figured out the max wavelength. For the next part, i used 2.5 ml of 3x10^-5 M CV+ solution and I recorded the absorbance at 10-20 second intervals. The absorbance value divided by the molar absorbance gave the CV+ concentration at the time, and the natural log of the value is plotted versus time to determine the k(prime) values. The equation is CV(+)(aq) + OH(-)(aq) --> CVOH.Type a sample calculation for the "Rate" here: (2 pts)[S2O3 2-] : M1V1=M2V2(0.0005M)(0.0005L)=(0.0025L)(M2)M2= 1.0e-4 MRate= (1/6)d[S2O3 2-]/dt (0.0001M)/(6*168s) = 9.921e-8Place your plot of 1/[CV+] vs time here (cover this instruction box so that your graph is an appropriate size).Properly label your graph (labels for axes, including units, and a title).Include a trendline and its equation and Rvalue on your graph. This is done by right-clicking on one of the data points on your graph and choosing "Add Trendline" from the drop down menu. The first tab asks what type of trendline you wish to use, and the Options tab allows you to include the trendline equation and Rvalue.
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