d. What is the rate of disappearance of oxalate ion when [C2O2−4]= 0.10 M[C2O42−]= 0.10 M and [HgCl2] = 0.20 M[HgCl2] = 0.20 M? e. Is the overall reaction likely to be an elementary step? Explain. f. Which species is oxidized in the reaction? Which is reduced?
d. What is the rate of disappearance of oxalate ion when [C2O2−4]= 0.10 M[C2O42−]= 0.10 M and [HgCl2] = 0.20 M[HgCl2] = 0.20 M? e. Is the overall reaction likely to be an elementary step? Explain. f. Which species is oxidized in the reaction? Which is reduced?
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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Rate law = k [HgCl2] [C2O4 -2]^2
I believe k = 0.022584815 s^-1
d. What is the rate of disappearance of oxalate ion when [C2O2−4]= 0.10 M[C2O42−]= 0.10 M and [HgCl2] = 0.20 M[HgCl2] = 0.20 M?
e. Is the overall reaction likely to be an elementary step? Explain.
f. Which species is oxidized in the reaction? Which is reduced?
![Mercury (II) chloride reacts with the oxalate ion according to the equation below:
2 HgCl2(ag) + C20la) →
2 Clag)
+ 2 CO2(9) + H92C12(s)
4(aд)
The initial rate of the reaction was determined for several concentrations of reactants and table below has the data obtained.
Experiment [H9C1»] (mol L-1) [C,0,²] (mol L-1) Rate (mol L-1 s-1)
1
0.144
0.132
5.63 x 10-5
2
0.144
0.396
5.10 x 10°
-4
0.072
0.396
2.51 × 10¬
-4
4
0.288
0.132
1.13 × 10–4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fceeaf470-6394-4005-8c4a-b2e031df5a26%2F933276b9-a5a7-45da-838e-bea8ddd7a08a%2Fxa8wgql_processed.png&w=3840&q=75)
Transcribed Image Text:Mercury (II) chloride reacts with the oxalate ion according to the equation below:
2 HgCl2(ag) + C20la) →
2 Clag)
+ 2 CO2(9) + H92C12(s)
4(aд)
The initial rate of the reaction was determined for several concentrations of reactants and table below has the data obtained.
Experiment [H9C1»] (mol L-1) [C,0,²] (mol L-1) Rate (mol L-1 s-1)
1
0.144
0.132
5.63 x 10-5
2
0.144
0.396
5.10 x 10°
-4
0.072
0.396
2.51 × 10¬
-4
4
0.288
0.132
1.13 × 10–4
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