CHM2 LAB(TOTAL 2 LAB)

CHM2 Lab(total 2 lab) - Chemistry
PLACE ORDER
look at the files first(11 Rate Law..... and use_det_eq.....) Two labAP Inquiry Lab 11 What is the Rate Law of the Fading Crystal Violet Reaction Using Beer’s Law? In this experiment, you will observe the reaction between crystal violet and sodium hydroxide. One objective is to study the relationship between concentration of crystal violet and the time elapsed during the reaction. The equation for the reaction is shown here: A simplified (and less intimidating!) version of the equation is: CV+ + OH– CVOH (crystal violet) (hydroxide) The rate law for this reaction is in the form: rate = k[CV+]m[OH–]n, where k is the rate constant for the reaction, m is the order with respect to crystal violet (CV+), and n is the order with respect to the hydroxide ion. Since the hydroxide ion concentration is more than 1000 times as large as the concentration of crystal violet, [OH-] will not change appreciably during this experiment. Thus, you will find the order with respect to crystal violet (m), but not the order with respect to hydroxide (n). You will be using a colorimeter for this lab. A colorimeter shines a light through the solution and checks how much light is absorbed by the solution. As the reaction proceeds, a violet-colored reactant will be slowly changing to a colorless product. Using the green (565 nm) light source of a computer-interfaced Colorimeter, you will monitor the absorbance of the crystal violet solution with time. Absorbance is proportional to the concentration of crystal violet (Beer’s law). Absorbance will be used in place of concentration in plotting the graphs. Beer’s law is A = abc where A = absorbance, a = molar absorptivity constant, b = path length, and c = concetration Once the order with respect to crystal violet has been determined, you will also be finding the rate constant, k, and the half-life for this reaction. PreLab Add this lab to your table of contents Write a purpose for this lab Create a table of reagents Sketch a graph of concentration vs time, ln concentration vs. time, and 1/concentration vs. time for a zero, first and second order reaction. Sketch a graph of the [CV+] and the [CVOH] over time during this reaction, reaction and write what you should visually see due this change in concentrations. MATERIALS Power Macintosh or Windows PC 0.020 M NaOH Vernier computer interface 2.0 X 10–5 M crystal violet Logger Pro distilled water Vernier Colorimeter stirring rod one plastic cuvette two 10-mL graduated cylinders 250-mL beaker Write a PROCEDURE For Graphically determining the order of the reaction The following bits of information will avoid excess waste, and help you with your procedure. 1. To set up the program, Click or tap Mode to open Data Collection Settings. Change Rate to 1 samples/s and End Collection to 200 s. Click or tap Done. 2. Use 10.0 mL of 0.020 M NaOH solution. Use 10.0 mL of 2.0 X 10–5 M crystal violet solution. CAUTION: Sodium hydroxide solution is caustic. Crystal violet is Sheet1 0 0.62 0.5 0.609 1 0.597 1.5 0.576 2 0.552 2.5 0.544 3 0.539 3.5 0.541 4 0.526 4.5 0.514 5 0.506 5.5 0.495 6 0.486 6.5 0.478 7 0.465 7.5 0.457 8 0.446 8.5 0.435 9 0.425 9.5 0.413 10 0.405 10.5 0.393 11 0.382 11.5 0.372 12 0.361 12.5 0.353 13 0.34 13.5 0.334 14 0.326 14.5 0.313 15 0.307 15.5 0.297 16 0.291 16.5 0.288 17 0.28 17.5 0.271 T vs A 0 0.5 1 1.5 2 2.5 3 3.5 4 4.5 5 5.5 6 6.5 7 7.5 8 8.5 9 9.5 10 10.5 11 11.5 12 12.5 13 13.5 14 14.5 15 15.5 16 16.5 17 17.5 0.62 0.60899999999999999 0.59699999999999998 0.57599999999999996 0.55200000000000005 0.54400000000000004 0.53900000000000003 0.54100000000000004 0.52600000000000002 0.51400000000000001 0.50600000000000001 0.495 0.48599999999999999 0.47799999999999998 0.46500000000000002 0.45700000000000002 0.44600000000000001 0.435 0.42499999999999999 0.41299999999999998 0.40500000000000003 0.39300000000000002 0.38200000000000001 0.372 0.36099999999999999 0.35299999999999998 0.34 0.33400000000000002 0.32600000000000001 0.313 0.307 0.29699999999999999 0.29099999999999998 0.28799999999999998 0.28000000000000003 0.27100000000000002 T ASheet1 0 0 0.2 0.582 0.5 0.554 0.8 0.549 1 0.543 1.2 0.549 1.5 0.551 1.8 0.559 2 0.552 2.2 0.535 2.5 0.527 2.8 0.508 3 0.503 3.2 0.504 3.5 0.501 3.8 0.497 4 0.489 4.2 0.477 4.5 0.477 4.8 0.471 5 0.459 5.2 0.458 5.5 0.443 5.8 0.441 6 0.429 6.2 0.426 6.5 0.421 6.8 0.41 7 0.404 7.2 0.394 7.5 0.391 7.8 0.392 8 0.381 8.2 0.374 8.5 0.366 8.8 0.37 9 0.362 9.2 0.357 9.5 0.351 9.8 0.345 10 0.34 10.2 0.335 10.5 0.326 10.8 0.324 11 0.32 11.2 0.307 11.5 0.314 11.8 0.301 12 0.295 12.2 0.292 12.5 0.293 12.8 0.28 13 0.282 13.2 0.283 13.5 0.276 13.8 0.264 14 0.259 14.2 0.258 14.5 0.257 14.8 0.248 15 0.244 15.2 0.241 15.5 0.243 15.8 0.237 16 0.233 16.2 0.231 16.5 0.225 16.8 0.234 17 0.221 17.2 0.222 17.5 0.222 17.8 0.215 18 0.213 18.2 0.211 18.5 0.223 18.8 0.205 19 0.205 19.2 0.203 19.5 0.196 19.8 0.198 20 0.188 T vs A 0 0.2 0.5 0.8 1 1.2 1.5 1.8 2 2.2000000000000002 2.5 2.8 3 3.2 3.5 3.8 4 4.2 4.5 4.8 5 5.2 5.5 5.8 6 6.2 6.5 6.8 7 7.2 7.5 7.8 8 8.1999999999999993 8.5 8.8000000000000007 9 9.1999999999999993 9.5 9.8000000000000007 10 10.199999999999999 10.5 10.8 11 11.2 11.5 11.8 12 12.2 12.5 12.8 13 13.2 13.5 13.8 14 14.2 14.5 14.8 15 15.2 15.5 15.8 16 16.2 16.5 16.8 17 17.2 17.5 17.8 18 18.2 18.5 18.8 19 19.2 19.5 19.8 20 0 0.58199999999999996 0.55400000000000005 0.54900000000000004 0.54300000000000004 0.54900000000000004 0.55100000000000005 0.55900000000000005 0.55200000000000005 0.53500000000000003 0.52700000000000002 0.50800000000000001 0.503 0.504 0.501 0.497 0.48899999999999999 0.47699999999999998 0.47699999999999998 0.47099999999999997 0.45900000000000002 0.45800000000000002 0.443 0.441 0.42899999999999999 0.42599999999999999 0.42099999999999999 0.41 0.40400000000000003 0.39400000000000002 0.39100000000000001 0.39200000000000002 0.38100000000000001 0.374 0.36599999999999999 0.37 0.36199999999999999 0.35699999999999998 0.35099999999999998 0.34499999999999997 0.34 0.33500000000000002 0.32600000000000001 0.32400000000000001 0.32 0.307 0.314 0.30099999999999999 0.29499999999999998 0.29199999999999998 0.29299999999999998 0.28000000000000003 0.28199999999999997 0.28299999999999997 0.27600000000000002 0.26400000000000001 0.25900000000000001 0.25800000000000001 0.25700000000000001 0.248 0.24399999999999999 0.24099999999999999 0.24299999999999999 0.23699999999999999 0.23300000000000001 0.23100000000000001 0.22500000000000001 0.23400000000000001 0.221 0.222 0.222 0.215 0.21299999999999999 0.21099999999999999 0.223 0.20499999999999999 0.20499999999999999 0.20300000000000001 0.19600000000000001 0.19800000000000001 0.188 T AExperiment 8: DETERMINATION OF AN EQUILIBRIUM CONSTANT 77 Purpose: The equilibrium constant for the formation of iron(III) thiocyanate complex ion is to be determined. Introduction: In the previous week, we qualitatively investigated how an equilibrium shifts in response to a stress to re-establish equilibrium. This week we will quantitatively assess the equilibrium constant for the same reaction: the reaction of iron(III) cation complexing with a thiocyanate anion (SCN–) to form the iron(III) thiocyanate complex, Fe(SCN)2+ (Equation 1). Its equilibrium expression is as shown in Equation 2. Fe3+ (aq) + SCN (aq) Fe(SCN)2+ (aq) Equation 1 2+ eq 3+ [Fe(SCN) ] K = -[Fe ][SCN ] Equation 2 If Keq is a large number (>1), then the chemical equilibrium favors the formation of product (large numerator). If Keq is a small number (<1) then the chemical equilibrium favors the formation of reactants (large denominator). In this experiment, several solutions of varying initial concentrations of the reactants are to be prepared. Despite the different concentrations, the equilibrium constants calculated from their equilibrium concentrations should be the same, as long as the temperature is kept constant. Before we begin the study of the equilibrium concentrations, we must first prepare a standard curve to help us determine the concentration of Fe(SCN)2+ at equilibrium. Le Châtelier’s Principle states that if at equilibrium a change is applied to a system, the species will react to offset the change so as to maintain the equilibrium. We will use this principle to aid in the preparation of the standard curve. It will be made by plotting the absorbance versus concentration of the red iron(III) thiocyanate complex, (Fe(SCN)2+). If the concentration of the reactant, iron(III) nitrate, is increased (0.200 M), so as to become much larger than the thiocyanate anion concentration (0.00200M), then the reaction (Equation 1) will be forced almost completely to products. In this situation, the iron(III) concentration is 100 times that of the thiocyanate, therefore essentially all the SCN– anions will react to produce the red colored product, Fe(SCN)2+. Thus, within the limits of our detection apparatus, the final concentration of Fe(SCN)2+ is equal to the initial concentration of SCN–. The intensity of the red color will be measured spectrophotometrically and will be directly proportional to the equilibrium concentration of the Fe(SCN)2+ species. (Review Beer’s Law from Experiment 3.) After a standard curve is produced, the conditions will be altered so that the concentrations of each of the two reacting species (Fe3+ and SCN–) will be the same order of magnitude (~0.00200 M each). Because the concentrations will be so similar, the system will no longer be forced all the way to the right (towards the products) and you will be able to determine an equilibVernier Format 2 KdatA.txt 6/11/2020 20:14:44 Run 1 conc Abs @ 446.2 nm c A M 0 0.000 .0001 0.416 .00015 0.687 .0002 0.895 .00025 1.215 .0003 1.429Vernier Format 2 kdta2.txt 6/11/2020 20:30:35 Run 1 conc Abs @ 446.2 nm c A M 0 0.000 .0002 0.104 .0004 0.239 .0006 0.462 .0008 0.585 0.001 0.718
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