DATA TABLE [FeCl3] Initial rate (s¹) Trial [KI] 1 0.01 M 0.01 M 0.00087586 2 0.01 M 0.005 M 0.0043348 3 0.005 M 0.01 M 0

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Data Table Fecl3 Initial Rate S Trial Ki 1 0 01 M 0 01 M 0 00087586 2 0 01 M 0 005 M 0 0043348 3 0 005 M 0 01 M 0 1 (51.75 KiB) Viewed 60 times

DATA TABLE [FeCl3] Initial rate (s¹) Trial [KI] 1 0.01 M 0.01 M 0.00087586 2 0.01 M 0.005 M 0.0043348 3 0.005 M 0.01 M 0.0039242 4 0.0075 M 0.005 M 0.007531 5 0.005 M 0.0075 M 0.003426 DATA ANALYSIS 1. Calculate the molar concentration of FeCl3 and KI for each reaction and record the values in the table above. Provide one example to show how you completed the calculation. m1v1=m2v2 0.02M*20mL=m1*40mL (0.02M*20mL)/40mL = 0.01M 2. What is the order of the reaction in FeCl3 and KI? Explain. 3. Write the rate law expression for the reaction. 4. Is it possible to calculate the rate constant, k, from your data? If so, calculate the rate constant. If not, explain why not. It isn't possible for this lab since we only have the initial rate.