Explain the k in the rate law and the activation energy

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Reference no: EM13321272

A clock reaction is run at 20 °C with several different mixtures of iodide, sodium bromate and acid, to form iodine. Thiosulfate is used to react with the iodine formed initially. Starch indicator is added to form a blue color when all the thiosulfate has been used up and the iodine concentration begins to rise. The following sets of mixtures are used. Initial concentrations in reaction mixtures Run number [I-] [BrO3-] [H+] 1 0.002 0.008 0.02 2 0.002 0.016 0.02 3 0.004 0.008 0.02 4 0.002 0.008 0.04 When the experiment is repeated at 31 °C, the rate constant is found to be 2.0 times larger. [S2O3^-2] is equal to 0.0001M in each reaction mixture. The rate law is : Rate = k [ I-]^a [ BrO3 -]^b [H+]^c Reaction time in run number 1 31 Reaction time in run number 2 31 Reaction time in run number 3 15 Reaction time in run number 4 15 Calculate the following The k in the rate law The activation Energy

Reference no: EM13321272

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