I’m pretty stuck here, I’m not even sure if I did the values in the second table

Question

I’m pretty stuck here, I’m not even sure if I did the values in the second table correct, I used M1V1=M2V2 I just want to know how to solve this table using what values. Kinetics of an Iodine Clock Reaction Data, Calculations, and Results Data and Calculations Table 1: Drops Table of solutions for each run. Duplicate this table in your formal lab report. Run | 0.2% | 0.012 M | 0.20 M | 0.20 M 1 0.20 M | 0.20 M No. starch Na S203 KI KNO, (NH4 S20s (NH4)2SO 10 10 10 20 10 20 10 10 10 10 10 10 15 Test Tube 10 mL Beaker Table 2: Times, temperatures for runs 1-9. Complete and duplicate this table in your formal lab repor Trial 2, s Trial 3, s Run Temperature (C Trial 1, s 3o.lo2 12luS3TOZ.TRU .5.22 1.18 unle from trial I, run L of each calculation below in your formal lab

Explanation / Answer

Hi!Since you've asked for the method behind solving the problem I'll help you with that. The Iodine clock reaction involves the following recurrent steps :

S2O82-(aq) + 2I-(aq) ------> I2(aq) + 2SO42-(aq)

I2(aq) + 2S2O32-(aq) -------> 2I-(aq) + S4O62-(aq)

rate= k [S2O82-] [I-]2

where quantities in [ ] denote the concentration of the reactants and k is the rate constant.

The rate of reaction can also be given as

rate= d [S2O82-] /dt = 1/2 d [S2O32-] /dt

you need to calculate the rate by dividing the change in concentration of S2O32- by the time taken for the change and multiply it by 1/2

now that you have the initial rate of reaction, you can calculate the reaction constant k.

k=initial rate of reaction / [S2O82-] [I-]2

ONCE YOU HAVE k YOU CAN EASILY CALCULATE THE RATE OF REACTION FOR EACH RUN BY SUBSTITUTING THE MOLARITIES OF [S2O82-] & [I-]2 GIVEN IN TABLE 3a.

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