Use the References to access important values if needed for this question. The f

Question

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion Experiment HgCl2lo, M2042]M Initial Rate, M s 0.118 0.236 0.118 0.236 0.402 0.402 0.804 0.804 1.82x10-4 3.63x10-4 7.26x10-4 1.45x10-3 2 4 Complete the rate law for this reaction in the box below Use the form k[A taken to the zero power do not appear. Don't enter 1 for m or n [m[Bj", where '1' is understood for 1' is understood for m or n and concentrations Rate- From these data, the rate constant is M-25-1

Explanation / Answer

Initial rate method:

R = K [HgCl2]m [C2O42-]n

We have to calculate value of m and n.

First consider experiment 1 and 2.

R1 = 1.82 x 10-4 = K [0.118]m [0.402]n

R2 = 3.63 x 10-4 = K [0.236]m [0.402]n

Divide R2 by R1:

R2 / R1 = 3.63 x 10-4 /1.82 x 10-4 = [0.236]m [0.402]n / [0.118]m [0.402]n

(2)1 = (2)m

m = 1 (Order w.r.t. HgCl2)

Now consider experiment 1 and 3

R1 = 1.82 x 10-4 = K [0.118]m [0.402]n

R3 = 7.26 x 10-4 = K [0.118]m [0.804]n

Divide R3 by R1:

R3 / R1 = 7.26 x 10-4 /1.82 x 10-4 = [0.118]m [0.804]n / [0.118]m [0.402]n

4 = (2)n

(2)2 = (2)n

n = 2 (Order w.r.t. C2O42-)

Overall Order = m + n = 1 + 2 = 3

Rate,R = K [HgCl2]1 [C2O42-]2

K = R / [HgCl2]1 [C2O42-]2

From experiment 1, put the values

K = 1.82 x 10-4 / (0.118) x (0.402)2

K = 0.954 x 10-2 M-2s-1

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