The acid-catalyzed reaction of acetone, CH 3 COCH 3 , with iodine can be represe

Question

The acid-catalyzed reaction of acetone, CH3COCH3, with iodine can be represented by the following reaction:

CH3COCH3 + I2 --H+--> CH2ICOCH3 + H+ + I-

It is found experimentally that the rate law for this reaction is Rate= K[CH3COCH3][H+]. Suppose that in trial 1, the initial rate of the reaction is measured with the initial concentrations of acetone, iodine, and hydrogen ion all equal to 0.10 M. Then, in trial 2, the initial rate of the reaction is measured with the intial concentrations all equal to 0.20 M. The initial rate of trial 2 will be larger than the initial rate of trial 1 by a factor of

a) 2.

b) 4.

c) 8.

d) 16.

e) 64.

ps: i know the answer is 4 but I dont know why can someone please explain this to me, thankyou!

Explanation / Answer

Given Rate= K[CH3COCH3][H+]                 -----(1)

In trial 1, the initial rate of the reaction is measured with the initial concentrations of acetone, iodine, and hydrogen ion all equal to 0.10 M. Then Rate,r = Kx0.1x0.1     ----(2)

In trial 2, the initial rate of the reaction is measured with the intial concentrations all equal to 0.20 M then

Rate,r' = Kx0.2x0.2

          = kx(2x0.1) x ( 2x0.1)

          = 4x(kx0.1x0.1)

          = 4xr

So r' = 4xr

        r' / r = 4

   Therefore the initial rate of trial 2 will be larger than the initial rate of trial 1 by a factor of 4

Hence option (b) is correct

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