2 HgCl2 + C204²-→2 Cl* + Hg2Cl2 + 2 CO2Initial Rate, MExperiment[HgCl]o, M[C2042-]o, M1S10.3650.4466.85x10-40.7300.4461.37×10-330.3650.8912.74x10-340.7300.8915.47x10-3Complete the rate law for this reaction in the box below.Use the form k[A]m[B]" , where '1' is understood for m or n and concentrations taken to thezero power do not appear. Don't enter 1 for m or n.Rate =From these data, the rate constant isM-2s-1.

Answered: Complete the rate law for this reaction…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2 HgCl2 + C204²-→2 Cl* + Hg2Cl2 + 2 CO2
Initial Rate, M
Experiment
[HgCl]o, M
[C2042-]o, M
1
S
1
0.365
0.446
6.85x10-4
0.730
0.446
1.37×10-3
3
0.365
0.891
2.74x10-3
4
0.730
0.891
5.47x10-3
Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]" , where '1' is understood for m or n and concentrations taken to the
zero power do not appear. Don't enter 1 for m or n.
Rate =
From these data, the rate constant is
M-2s-1.

Expert Solution

Step 1

$r = k {[A]}^{m} {[B]}^{n} r_{1} = 6.85 * 10^{- 4} M s^{- 1} = k {[0.365]}^{m} M {[0.446]}^{n} r_{2} = 1.37 * 10^{- 3} M s^{- 1} = k {[0.730]}^{m} M {[0.446]}^{n}$

$\frac{r_{2}}{r_{1}} = \frac{k {(0.730 M)}^{m} {(0.446 M)}^{n}}{k {(0.365 M)}^{m} {(0.446 M)}^{n}} = \frac{1.37 * 10^{- 3} M s^{- 1}}{6.85 * 10^{- 4} M s^{- 1}}$

(2)^m = 2

m =1

Therefore order with respect to A (i.e.) [HgCl₂] = 1

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