Initial rate question?

Rate law question..........?

• The acid-catalyzed reaction of acetone, CH3COCH3, with iodine can be represented by the following net reaction: CH3COCH3 + I2 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 initial 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. 8. b. 64. c. 2. d. 16. e. 4.

• Answer:

  I am not exactly sure why you are asking this question. Just replace the .1 with the .2 Since that is 2 times larger, it will be raised by a factor of 2 squared: 4