The Iodination of Acetone lab- Need help with determining the reaction orders

[crabapple11]

I need to find the variable m in the following equation
rate=k(acetone)^m(I₂)ⁿ(H+)^p

Here is our expirmental data
Exp. 1
10 ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I₂ reacted in 68 sec.
Exp. 2
20 ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I₂ reacted in 27.6 sec.


I calculated the initial concentration of each to be
Exp. 1 (Acetone)=0.8 M (H+)=0.2M (I₂)=0.001M
Exp. 1 (Acetone)=1.6 M (H+)=0.2M (I₂)=0.001M
I found the rate of reaction to be
Exp. 1 = 1.47 * 10^-5
Exp. 2 = 3.63 * 10^-5

Then I plugged the data into the equation
rate=k(acetone)^m(I₂)ⁿ(H+)^p
and solved for "m"
but i got 1.26

My question is whether or not this number is even close and if it is should I just round it to 1 or what is the correct answer?

 

[TeethWhitener]

The calculation looks fine. The correct answer can be found with a quick google search, but keep in mind that if you only have two data point, your error bars are likely to be huge.