Iodine Reaction Rate Lab Report

Abstract
The purpose of this experiment was to find the rate law for the reaction of iodine with acetone using the initial rates method. The rates of each reaction was found by measuring the time elapsed between the addition of iodine to the solution and for the color of iodine to completely disappear in various trials. After the experiment was completed, the rates of iodine, the constant and the standard deviation were calculated and the rate law for the reaction of iodine was found to be: Rate=8.075 ±0.359 〖[A]〗^1 〖[HCl]〗^1 〖[I]〗^0
Introduction
The purpose of this experiment was to ascertain the rate law for the reaction of iodine with acetone, also known as iodination, by using proper experimental methods and calculations with the method

The chemical equation that causes this to occur is: (2)
The rate law is the relationship between the rate of a reaction and the concentrations of reactants.(3) In order to find the rate law the following equations must be used:
Equation 1: Used to find the iodine concentration rate for each reaction.
([I])/t×〖10〗^5
Where [I] is the concentration of Iodine (moles/L) and t is the time in seconds taken for the iodine to completely disappear during the reaction.
Equation 2: Used to find the concentration orders for acetone, hydrochloric acid and iodine.
(〖[Rate〗_1]=k 〖[A_1]〗^a 〖[〖HCl〗_1]〗^h 〖[I_1]〗^i)/(〖[Rate〗_2]=k 〖[A_2]〗^a 〖[〖HCl〗_2]〗^h 〖[I_2]〗^i

After all of the time data was collected, the molarity of each amount had to be recalculated, (refer to Table 3 for new molarities).
Molarity (m/L) Acetone HCL Iodine
Reaction 1 0.6666667 0.1666667 0.0011111
Reaction 2 1.3333333 0.1666667 0.0011111
Reaction 3 2 0.1666667 0.0011111
Reaction 4 0.6666667 0.3333333 0.0011111
Reaction 5 0.6666667 0.5 0.0011111
Reaction 6 0.6666667 0.1666667 0.0022222
Reaction 7 0.6666667 0.1666667 0.0033333
Table 3: Corrected molarity for acetone, hydrochloric acid and iodine for each reaction
Next, the iodine concentration rate for each reaction needed to be calculated. This was completed using the Equation 1 for Trial 1: Reaction 1:
0.00111/130×〖10〗^5=0.855 (moles/L)/second
The concentration of Iodine (found in Table 3) : 0.00111 moles/L
The time elapsed during Trial 1: Reaction 1 (found in Table 2) : 130 seconds
[I] Rate Trial 1 Trial 2 Trial 3 Mean Stdev
Reaction 1 0.8547009 0.9337068 0.9033424 0.89725 0.039854
Reaction 2 1.8832392 2.020202 1.984127 1.962523 0.070991
Reaction 3 2.6455026 2.8490028 2.9239766 2.806161 0.144096
Reaction 4 1.8214936 1.9157088 2.020202 1.919135 0.099398
Reaction 5 2.5252525 2.7777778 2.7777778 2.693603