ctivation Energy from Experimental Data K11 of 14 he iodination of acetone, CHs

Question

ctivation Energy from Experimental Data K11 of 14 he iodination of acetone, CHs COCHj, in aqueous solution is catalyzed by the hydrogen ion The following data were acquired in an iodination experiment involving acetone. All reaction times a in terms of the rate of disappearance of I2 H+ H* Volume of Volume Volume Volume of 0.050 of 1.0 M of Temperature Reaction time The reaction can be followed visually by adding starch. The purple starch-iodine complex forms immediately, then disappears when the iodine has been consumed. The kinetics of the reaction may be determined by recording the time required for the color to disappear, which is the time required for the iodine, 12, to be consumed MIMHCl acetone water C) (mL) (mL) A 5.0 10.0 10.0 25.0 25.0 B 10.0 10.010.0 20.0 25.0 C 10.0 20.0 100 10.025.0 25.0 E 10.0 10.0 100 20.0 42.4 130 249 128 131 38 D 10.0 10.0 20.0 10.0

Explanation / Answer

For part C of your question, the rate of reaction is pretty easy to find - we just need to find the amount of I2 present initially and divide it by the 38 seconds that it took for all of the I2 to react (your question doesn't specify how the answer should be expressed):

First, the amount of I2:
10 mL of 0.0010M I2
= .01 L at .001 moles per liter
= .00001 moles of I2
I2 has a molecular weight of 254 g/mol (127 x 2),
so .00001 x 254 = .00254 g or 2.54 mg

If this amount took 38 seconds to react, then the rate of reaction is:
2.54 mg / 38 seconds  
= .0668 mg per sec.  

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