Iodine reacts with a ketone in aqueous solution to give an iodoketone. The stoichiometric equation is: I2 + ketone -> iodoketone + H+ + I-

The rate of reaction can be measured by measuring the disappearance of I2 with time. The data for initial rates and initial concentrations are as follows:

(a) Find the order of the rate of reaction with respect to I2, ketone and H+

(b) Write a differential equation expressing your findings in part (a) and calculate the average rate constant

(c) How long will it take to synthesize 10^-4 mol/L of the iodoketone starting with 0.5 mol/L of ketone and 0.001 mol/L of I2, if the H+ concentration is held constant at 0.1 mol/L?

(d) What will happen to the reaction if we double the concentration of ketone? Or iodine? Or H+?

Transcribed Image Text:

-d[1₂]/dt (mol/L.s) 7 x 10-5 7 x 105 1.7 x 10-4 5.4 x 10-4 [1₂] (mol/L) 5 x 10-4 3 x 10-4 5 x 10-4 5 x 10-4 [ketone] (mol/L) 0.2 0.2 0.5 0.5 [H*] (mol/L) 1.0 x 10-² 1.0 x 10² 1.0 x 102 3.2 x 10² -d[1₂]/dt (mol/L.s) 7 x 10-5 7 x 105 1.7 x 10-4 5.4 x 10-4 [1₂] (mol/L) 5 x 10-4 3 x 10-4 5 x 10-4 5 x 10-4 [ketone] (mol/L) 0.2 0.2 0.5 0.5 [H*] (mol/L) 1.0 x 10-² 1.0 x 10² 1.0 x 102 3.2 x 10²

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The given reaction is Iodene Ketone Iodoketone H I The rate of the reaction R dI 2 dt diodoketonedt Let the order of the reaction with respect to I 2 ... View the full answer