2-9 2 CHEMICAL KINETICS NAME Pre-Lab Assignment 1415 Section Assignment submission: Your instructor will inform you when the assignment is due and how it is to be submitted. NOTE: The time data used here are for illustrative purposes. The time data you obtain will be different Refer to the Summary of Runs Table, p 3-4, and determine [Fo) for each run using the dilution formula. Reminder: Man = Show an illustrative calculation for run 3 as an example. Enter the results in the following table. EXAMPLE: 0.0025 M PRACTICE: Refer to the Summary of Runs Table, p 3-4, and determine [ Jinnial for each run using the dilution formula. Reminder: Me M. Show an illustrative calculation for run 3 as an example. Enter the results in the following table. EXAMPLE: 0.0050 M PRACTICE Determine the rate for each run. Show an illustrative calculation for run 3 as an example. Enter the results in the following table. Report rates to at least one more digit than allowed by applying the rules for significant digits. EXAMPLE: 3.53 x 10 Ms. (Note: the underscored digit is not a significant figure. It is included to minimize rounding errors.) PRACTICE EXAMPLE Run 1 2 3 Leo. 97 48 34 [Feat.M 0.0025 0.0050 0.0025 [feat. M 0.0025 0.0025 0.0050 rate, M/s 1.24 x 10 2.50 x 10 3.53 x 10 PRACTICE: [Fe M [1]...M Rate, Ms Run 1 2 3 ws 430 149 108 3-4 [Fe3"]initial and [HSCN]inibar are the initial concentrations of reactants after mixing but before = reaction occurs. Like experiment 4, the initial concentrations are obtained using the dilutior formula (Mconcconc = MaiVail) and Main = Minitial. The [Fe(SCN)]2"]initial and [H"]initial are fixed by the experimental set-up. There is no Fe(SCN initially and the [H") is 0.500 M initially. Equilibrium concentrations of Fe3+, HSCN, and He are found with the help of an 'ICE' Table enter known concentrations into the table as shown in bold. Initial Change Equilibrium [Fe3+] 10.0 x 10-4 -0.2628 x 10- 9.7372 x 10- [HSCN) 2.00 x 10-4 -0.2628 x 10-4 1.7372 x 10-4 [Fe(SCN)2+) 0 +0.2628 x 10-4 0.2628 x 10-4 [H] 0.500 +0.2628 x 10-4 0.500 Complete the table. But before doing so, you should note the following: For any component, call it X, in the equilibrium system, its change in concentration in achieving equilibrium, A[X], is: A[X] = [X]ea - [X]initial The sign of A[X] indicates whether the concentration of X increased or decreased in achieving equilibrium. This sign is the same for all species on the same side of the reaction equation. Species on the opposite side of the equation have the annosite sin