Answer all questions in this section. 1. (a) H2S(aq) + Cl2(g) S(s) + 2HCI(aq) i. Given that, when the concentration of H2S is doubled, rate also double while double the concentration Cl2 will cause the rate of reaction increase 4 times. Write the rate law of the reaction. ii. The overall reaction order iii. The rate of reaction at 300K if the rate constant is 2.8 x 10²M²s' and the concentration of H2S and Cl2 are 2.7×10²M and 7.0x102 M respectively.

Answer all questions in this section. 1. (a) H2S(aq) + Cl2(g) S(s) + 2HCI(aq) i. Given that, when the concentration of H2S is doubled, rate also double while double the concentration Cl2 will cause the rate of reaction increase 4 times. Write the rate law of the reaction. ii. The overall reaction order iii. The rate of reaction at 300K if the rate constant is 2.8 x 10²M²s' and the concentration of H2S and Cl2 are 2.7×10²M and 7.0x102 M respectively.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 98CWP: A certain reaction has the form aAProducts At a particular temperature, concentration versus time...

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A certain reaction has the form aAProducts At a particular temperature, concentration versus time data were collected. A plot of 1/ [A] versus Lime (in seconds) gave a straight line with a slope of 6.90 102. What is the differential rate law for this reaction? What is the integrated rate law for this reaction? What is the value of the rate constant for this reaction? If [A]0 for this reaction is 0.100 M, what is the first half-life (in seconds)? If the original concentration (at t = 0) is 0.100 M, what is the second half-life (in seconds)?
For the reaction of crystal violet with NaOH(aq), the measured rate of reaction is 1.27 106 mol L1 s1 when the concentration of crystal violet cation is 4.13 105 mol/L. (a) Estimate how long it will take for the concentration of crystal violet to drop from 4.30 105 mol/L to 3.96 105 mol/L. (b) Could you use the same method to make an accurate estimate of how long it would take for the concentration of crystal violet to drop from 4.30 105 mol/L to 0.43 105 mol/L? Explain why or why not.
Why awe elementary reactions involving three or more reactants very uncommon?
Most reactions occur by a series of steps. The energy profile for a certain reaction that proceeds by a two-step mechanism is On the energy profile, indicate a. the positions of reactants and products. b. the activation energy for the overall reaction. c. E for the reaction. d. Which point on the plot represents the energy of the intermediate in the two-step reaction? e. Which step in the mechanism for this reaction is rate determining, the first or the second step? Explain.
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
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?
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
If you know some calculus, derive the integrated second-order rate law for the reaction 2Aproducts Follow the same steps listed in Question 121.
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.