I Review | Constants | Periodio The rate constant of a chemical reaction increased from 0.100 s 1 to 2.90 s1 upon raising the temperature from 25.0 °C to 35.0 °C Learning Goal: To use the Arrhenius equation to calculate the activation energy. Part A As temperature rises, the average kinetic energy of molecules increases, In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation (4) Calculate the value of where T is the initial temperature and T is the final temperature. k = Ae E/RT Express your answer numerically. where k is the rate constant, A is the frequency factor, E, is the activation energy, R = 8.3145 J/(K - mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: > View Available Hint(s) ΠV ΑΣφ :)- ($) (뉴-%) K- In where k, is the rate constant at temperature T, and k2 is the rate constant at temperature T. Submit

I Review | Constants | Periodio The rate constant of a chemical reaction increased from 0.100 s 1 to 2.90 s1 upon raising the temperature from 25.0 °C to 35.0 °C Learning Goal: To use the Arrhenius equation to calculate the activation energy. Part A As temperature rises, the average kinetic energy of molecules increases, In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation (4) Calculate the value of where T is the initial temperature and T is the final temperature. k = Ae E/RT Express your answer numerically. where k is the rate constant, A is the frequency factor, E, is the activation energy, R = 8.3145 J/(K - mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: > View Available Hint(s) ΠV ΑΣφ :)- ($) (뉴-%) K- In where k, is the rate constant at temperature T, and k2 is the rate constant at temperature T. Submit

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 11.ACP: (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a...

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For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Consider the general reaction aA+bBcC and the following average rate data over some time period t: At=0.0080mol/LsBt=0.0120mol/LsCt=0.0160mol/Ls Determine a set of possible coefficients to balance this general reaction.
For the following reaction profile, indicate a. the positions of reactants and products. b. the activation energy. c. E for the reaction.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
Why awe elementary reactions involving three or more reactants very uncommon?
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?
Compare the functions of homogeneous and heterogeneous catalysts.
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.
. Account for the increase in reaction rate brought about by a catalyst.