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Nia kaings Experiment 7: lodine Clock Reaction Kinetics CHEMISTRY REVIEW TOPICS Reading: OpenStax, Chemisi, 2e, Chapter 12, Scctions 12.1 to 12.3 YouTube Video: Kinctics: Chemistry's Demolition Derby. (First 6 min. of video are most relevant,) YouTube Video: The Arhenius Equation, Activation Encrgy, and Catalysis Explained Pt 8 SAFETY Hot Equipment: Be careful with the hot plates. They remain hot for a long time after switched off. Chemical waste: All chemicals can be disposed of in the sink followed by rinsing. INTRODUCTION: In this experiment, you will determine a reaction rate and the effect of changing reactant concentration and temperature on reaction rate of a chemical reaction. The reaction chosen proceeds conveniently slowly near room temperature and can easily be measured by observing a dramatic color change. The reaction is the oxidation of iodide ion (I) to molecular iodine (l») by hydrogen peroxide (H202): :02+2H+21 » +2 HO slow (Eqn. 1) As the reaction proceeds, the colorless reactants gradually generate brown l2 product. It is difficult to time the appearance of Iz, therefore, we make use of a second much faster reaction in the same solution to measure the progress of the slow reaction: Starcih Eqn. 2) GddedasS Ia+2 S20s-21+S40 fast an.indCaHOr Reaction 2 is so fast that I2 produced by reaction 1 is consumed instantaneously by thiosulfate (S20), preventing the brown l2 color appearance. Because both S:0 and S4Oare colorless, therefore the solution remains colorless. However, less thiosulfate is added than will consume all the I2 that will be formed from reaction 1. Therefore the reaction solution stays colorless until the instant at which all the thiosulfate is consumed. The reaction is timed starting at initial mixing until the appearance of color from I2. To help visualize the appearance of I2 starch indicator is added to give an intensely colored dark complex. The stoichiometry of the two reactions will allow the determination of the reaction rate in terms of H:02 by mcasuring the change in S,0as follows: A,0]A L A,L 1AS,O;] 2 Ar rate of reaction = Ar A Ar By repeating the experiment with different concentrations of H202 and different temperatures, we can determine the effect of changing H20 concentration and temperature on the rate of reaction 1. During a chemical reaction, bonds are broken in reactants and new bonds are formed in the products. Reactions can only occur if reactant molecules collide with each other. These collisions Reagent Concentrations: 0.10,M HI, 0.20M H;02, 0.15 M S:0 Run 1 Run 2 Run 3 Run 4 Run 5 1., seconds Q0L.lo sad Y1.o80.Ysesec Ia.&G11.1°C1,5C| 319C|0G 3.H:0:1 M 0.0OM O.0M. O.a0M o.20M 0.a0M_ 5-1,M0.15MO.15M|o.5M o.1SM_ o.5M 2. Temp. 'C 5. AS:0I. M 6. A H:0:], M 7. Rate, M/s 8. k, s 9. In k 10. 1/T, K In the spaces below, show the following calculations for Run 1. 3. [H0] M O.9ON MIV V 4. [S014 M O.15 M 5. AS2021, M 7. Rate, Mis 8. k,s s1 9. In k 10.1/7, K 1. Using the MS Excel graph based on your experimental data provide the following information: Show work where requested for credit. a) The slope for In k vs. 1/T graph straight line is b) The units for slope are Show calculations in the space below. c)The activation energy (E.) is . Show calculations in the space helow. d) The frequency factor (A) is_ Show calculations in the space below 2. Use the data from Runs 1, 2 and 3 confirm that Rcaction I is first-order in H20D. Additional Questions 1. What is the effect of increasing [H:Q2]/ on the rate of reaction in the experiment? Whan Ha0 iNCicad ha Yole of Leacion inckoKO. 2. What is the effect of increasing the temperature on the rat� of reaction in the experiment ncea sing the teperoBwe sfeed up tN rale ot Caction. 3. Iodide ion is oxidized in acidic solution to triiodide ion (l;") by hydrogen peroxide. H2Oz(aq)+ 31(ag) +2H (ag) > Is (ag) +2H20() The following data were obtained from 4 experiments that varied the initial reactant concentrations. Use to answer questions a and b. Initial Concentrations (M) H202 H Initial Rate [M/s] Exp. 1 0.010 0.010 0.00050 1.15 x 106 Exp. 2| Exp.3L Exp. 4 0.00050 0.00050| 0.020 0.010 2.30 x 10° 2.30 x 106 1.15 x 10 0.010 0.020 0.010 0.010 0.00100 a) Detemine the rate law for the above reaction. b) Detcrmine the rate constant of the reaction.