Raised to the power m on the rights. It should be similar in appearance to equat

Question

Raised to the power m on the rights. It should be similar in appearance to equation 6. Put the resulting equation below: The only unknown in the equation is m. Solve for m. Now write equation 3 as it would apply to reaction mixture III and as it would apply to reaction mixture IV: Using the rations of the rates of Mixtures III and IV to those of Mixtures II or I, find the orders of the reaction with respect to H^+ ion and I_2: Determination of the Rate Constant k Given the values of m, p. and n as determined in Part B, calculate the rate constant k for -ach mixture by simply substituting those orders, the initial concentrations, and the observed rate from the table into Equation 3. Prediction of Reaction Kate (Optional) Reaction mixture Initial concentrations (acetone) M (H+) M (I_2) M Predicted rate (Eq.3) Predicted time for reaction sec (Eq.5) Observed time for reaction sec

Explanation / Answer

SOLUTION:

HINT: Rate can be Determined by calculating the change in rate of reaction by changing the concentration.

Order w.r.t. acetone can be found from rate I and rate II. In rate I and rate II the concentration of H+ and I2 remainn constant while the concentration of acetone is halved

Rate II / Rate I = / 7.19 X 10-6 / 3.610 X 10-6 = [Acetone II / acetone I]m

7.19 X 10-6 / 3.610 X 10-6 = [0.4 / 0.8]m

2 = (0.5)m

Or m = -1

Similarly Order w.r.t H+ Can be had from Rate I and Rate III

Rate III / Rate I = 6.76 X 10-6 / 3.610 X 10-6 = (H+ / H+)n

1.87 = (0.1/0.2)n = (0.5)n

Or n = -0.897

Similarly order w.r.t I2

Rate IV / Rate I = 8.7 X 10-7 / 3.61 X 10-6 = (0.0005 / 0.001)p

0.24 = (0.5)p

Or p = 2

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