Use the previous example for the chemical reaction2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s)The following initial rates of reactions were determined for the reactant concentrationsgiven:Experiment #[HgCl₂]0.1000.1000.050123[C₂O4²-]0.200.40 1.2 x 10-40.40 6.2 x 10-5Initial rate (M/sec)3.1 x 10-5(a) Find the order of the reaction with respect to HgCl2₂.(b)Find the order of the reaction with respect to C₂04²(c)Write the rate law for this reaction.(d)Calculate the value for the rate constant based on the data for experiment #1 andprovide the proper units.

Answered: Image /qna-images/answer/f1f75ffc-5737-4ba1-9db5-a748ed5cc294.jpg

Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O²(aq) → 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 3.1 x 10-5 Initial rate (M/sec) 0.40 1.2 x 10-4 0.40 6.2 x 10-5 (a)Find the order of the reaction with respect to HgCl₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.

Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O²(aq) → 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 3.1 x 10-5 Initial rate (M/sec) 0.40 1.2 x 10-4 0.40 6.2 x 10-5 (a)Find the order of the reaction with respect to HgCl₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 76AE: One of the concerns about the use of Freons is that they will migrate to the upper atmosphere, where...

See similar textbooks

Similar questions

One of the concerns about the use of Freons is that they will migrate to the upper atmosphere, where chlorine atoms can be generated by the following reaction: CCl2F2(g)Freon-12hvCF2Cl(g)+Cl(g) Chlorine atoms can act as a catalyst for the destruction of ozone. The activation energy for the reaction Cl(g) + O3(g) ClO(g) + O2(g) Is 2.1 kJ/mol. Which is the more effective catalyst for the destruction of ozone, Cl or NO? (See Exercise 75.)
Which reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.