I need to determine the orders for the reactants, the rate expression, and the r

Question

I need to determine the orders for the reactants, the rate expression, and the rate constant for the reaction between iodine and acetone. Any help is appreciated.. I'm pretty lost when it comes to this.

Here is the data we collected:

I. Determination of Orders

Rate = k[acetone]m[I2] n [H+ ] p

Order of Acetone “m” __________

Order of Iodine “n” ___________

Order of Hydrogen Ion “p” __________

The Rate Law for the reaction is: ________

II. Determine the Rate Constant k

Trial 1 ____

Trial 2 ____

Trial 3 ____

Trial 4 ____

Average Value for k __________

III. Prediction of Reaction Rate

Use the data from Trial 5 to compare actual and predicted rates of reaction.

Rate = k[acetone]m[I2] n [H+ ] p

[acetone] = __________

[I2] = _________ [

H+ ] = _________

k(average) = _________

Predicted Rate = _______________

Experimental Rate = [I2]/t = _______________

Thank you!!

Explanation / Answer

In exp. 1 & 2 keeping all other reactants concentration constant.

when we doubled the amount of acetone rate becomes 53.5 s.that is reaction rate increases by 1.822 approximately also 2 times.

so Order of Acetone m = 1st oder = 1

In exp. 1 &3 keeping all other reactants concentration constant

when we doubled the amount of HCl rate becomes 56.5 s .that is reaction rate increases by 1.72566 times that is appr. 2 times

Order of Hydrogen Ion “p” = 1st oder =1

In exp. 1 &4 keeping all other reactants concentration constant

when we doubled the amount of iodine rate become 204.5 s that is rate is decreases by 0.475 times that is appro 1/2 times.

Order of Iodine “n”= 1/2

The Rate Law for the reaction is = k[acetone]1[I2] 1/2 [H+ ] 1

Rate Constant = rate / [acetone]1[I2] 1/2 [H+ ] 1

trial 1, K = 97.5 / [10] [10]^1/2 [10] = 97.5/316.23 = 0.308

trial 2, K = 53.5 / [20] [10]^1/2 [10] = 53.5 / 200x 3.16 = 0.084

trial 3, K = 56.5 /[10] [10]61/2 [20] =56.5 / 632 = 0.089

trial 4 , K = 204.5 [10][20]^1/2 [10] = 204.5 / 100x 4.472 = 0.45

Average Value for k = 0.308+ 0.084 + 0.089 + 0.45 / 4 = 0.931/4= 0.2327

3- Rate = k[acetone]1[I2] 1/2 [H+ ] 1

[acetone] =[30]

[iodine]=[ 5]^1/2

[H+] = [10]

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