Consider the following reaction between mercury(II) chloride and oxalate ion.2 HgCl2(aq) + C2O42-(aq) 2 Cl -(aq) + 2 CO2(g) + Hg2Cl2(s)The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O42-, and the following rate data were obtained for the rate of disappearance of C2O42-. Experiment[HgCl2] (M)[C2O42-] (M)Rate (M/s) 10.1640.153.2 10-520.1640.452.9 10-430.0820.451.4 10-440.2460.154.8 10-5(a) What is the rate law for this reaction?k[HgCl2][C2O4-2]2k[HgCl2]2[C2O4-2] k[HgCl2]2[C2O4-2]1/2(b) What is the value of the rate constant?_______M-2s-1(c) What is the reaction rate when the concentration of HgCl2 is 0.12 M and that of C2O42- is 0.12 M if the temperature is the same as that used to obtain the data shown above?________M/s

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Answered: Consider the following reaction between…

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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Consider the following reaction between mercury(II) chloride and oxalate ion.

2 HgCl₂(aq) + C₂O₄^2-(aq) 2 Cl ^-(aq) + 2 CO₂(g) + Hg₂Cl₂(s)

The initial rate of this reaction was determined for several concentrations of HgCl₂ and C₂O₄^2-, and the following rate data were obtained for the rate of disappearance of C₂O₄^2-.

Experiment	[HgCl₂] (M)	[C₂O₄^2-] (M)	Rate (M/s)


1	0.164	0.15	3.2 10^-5
2	0.164	0.45	2.9 10^-4
3	0.082	0.45	1.4 10^-4
4	0.246	0.15	4.8 10^-5

(a) What is the rate law for this reaction?

k[HgCl₂][C₂O₄^-2]²k[HgCl₂]²[C₂O₄^-2] k[HgCl₂]²[C₂O₄^-2]^1/2

(b) What is the value of the rate constant?
_______M^-2s^-1

(c) What is the reaction rate when the concentration of HgCl₂ is 0.12 M and that of C₂O₄^2- is 0.12 M if the temperature is the same as that used to obtain the data shown above?
________M/s

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