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Biology and Chemistry Homework Help
The Iodination of Acetone lab- Need help with determining the reaction orders
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[QUOTE="crabapple11, post: 2440669, member: 212936"] I need to find the variable m in the following equation rate=k(acetone)[SUP]m[/SUP](I[SUB]2[/SUB])[SUP]n[/SUP](H+)[SUP]p[/SUP] Here is our expirmental data Exp. 1 [B]10[/B] ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I[SUB]2[/SUB] reacted in [B]68[/B] sec. Exp. 2 [B]20[/B] ml of 4 M acetone + 10 ml of 1 M HCl + 10 ml 0.005 M I[SUB]2[/SUB] reacted in [B]27.6[/B] sec. I calculated the initial concentration of each to be Exp. 1 (Acetone)=0.8 M (H+)=0.2M (I[SUB]2[/SUB])=0.001M Exp. 1 (Acetone)=1.6 M (H+)=0.2M (I[SUB]2[/SUB])=0.001M I found the rate of reaction to be Exp. 1 = 1.47 * 10[SUP]-5[/SUP] Exp. 2 = 3.63 * 10[SUP]-5[/SUP] Then I plugged the data into the equation rate=k(acetone)[SUP]m[/SUP](I[SUB]2[/SUB])[SUP]n[/SUP](H+)[SUP]p[/SUP] 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? [/QUOTE]
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Biology and Chemistry Homework Help
The Iodination of Acetone lab- Need help with determining the reaction orders
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