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The Iodination of Acetone lab Need help with determining the reaction orders 
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Nov1309, 06:46 PM

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I need to find the variable m in the following equation
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? 


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