- #1

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rate=k(acetone)

^{m}(I

_{2})

^{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 I

_{2}reacted in

**68**sec.

Exp. 2

**20**ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I

_{2}reacted in

**27.6**sec.

I calculated the initial concentration of each to be

Exp. 1 (Acetone)=0.8 M (H+)=0.2M (I

_{2})=0.001M

Exp. 1 (Acetone)=1.6 M (H+)=0.2M (I

_{2})=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}(I

_{2})

^{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?