EXPERIMENT 10: IODINE CLOCK REACTION- DETERMINATION OF THE RATE EXPRESSION Date:

Question

EXPERIMENT 10: IODINE CLOCK REACTION- DETERMINATION OF THE RATE EXPRESSION Date: In-Lab Guidelines (This is a guide to the information you should observe while in the laboratory Record this information on your lab data sheets. Turn in the du to your Instructor before you leave the laboratory period.) Roon Temperature = °C Solution A Molarity KIO, Solution B Molarity H.SO, PART A. You may wish to have all the volumes already recorded in your table since these are Experimental Procedure. Then all you need to record is the listed in the Mixture A (KIO Soln. B (H,SO) mL H,O sec mL ml oml 110 sec ml0ml 2.0 sec mL. ml. mL 1 PART B. TEMPERATURE have tolook them u, enabing you to finish more quickly Mixture (KIO) u may wish to have the volumes already filled in when you come to lab. This way you won't Soln. B Temp.Time mL Observations (Record any obervations you tmalke how the color appeared spill, cvolution of hesat, etc.) Experiment 10 lodine Clock Reaction-Determination of the Rate Expression

Explanation / Answer

Rate = k [A]^x[B]^y

rate1/rate2 = k [A1]^x[B1]^y/k [A2]^x[B2]^y

(0.3*10^-6)/(8.1*10^-6) = ((1*10^-2)^x*(1)^y)/((1*10^-2)^x*3^y)

y = 3 order with respect to B

rate2/rate3 = k [A2]^x[B2]^y/k [A3]^x[B3]^y

(8.1*10^-6)/(3.24*10^-5) = ((1*10^-2)^x*3^y)/((2*10^-2)^x*3^y)

x = 2 order with respect to A

Rate law is given by,

Rate = k [A]^2[B]^3

0.3*10^-6 = k(1*10^-2)^2*(1)^3

Rate Constant k = 3 * 10^-3

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