Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , 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-25-1.

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
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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.
Transcribed Image Text: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 r1= 6.85 * 10-4 M s-1= k[0.365]m M [0.446]n  r2=1.37 * 10-3 M s-1= k[0.730]m M [0.446]n

r2r1 = k (0.730 M)m (0.446 M)nk (0.365 M)m(0.446 M)n =1.37 * 10-3 M s-16.85 * 10-4 M s-1

                                 (2)m = 2

                                  m =1

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

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