Part AIf a temperature increase from 10.0 °C to 20.0 °C doubles the rate constant for a reaction, what is the value of the activation barrier for the reaction?Ea =kJ/mol%3DSubmitRequest Answer

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter30: Kinetic Methods Of Analysis

Section: Chapter Questions

Problem 30.7QAP

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Each of the statements given below is false. Explain why. a. The activation energy of a reaction depends on the overall energy change (E) for the reaction. b. The rate law for a reaction can be deduced from examination of the overall balanced equation for the reaction. c. Most reactions occur by one-step mechanisms.
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
Nitrosyl chloride, NOCI, decomposes to NO and CI2. 2NOCI(g)2NO(g)+CI2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.20 0.30 Rate (mol/L/h) 8.01010 3.2109 7.2109
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?
A substance undergoes first-order decomposition. After 40.0 min at 500°C, only 12.5% of the original sample remains. YYliat is the half-life of the decomposition? If the original sample weighed 243 g, how much would remain after 2.00 h?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
11.34 Rate data were obtained at 25°C for the following reaction. What is the rate law expression for this reaction? A + 2B — C + 2D Expt Initial [A] (mol L-’) Initial [B] (mol L_1) Initial Rate ofFormation of C (mol L-1 min-1) 1 0.10 0.10 3.0 X 10~4 2 0.30 0.30 9.0 X 10"4 3 0.10 0.30 3.0 X 10~4 4 0.20 0.40 6.0 X 10"4
The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2(g)+2NO(g)N2O(g)+H2O(g) Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data: [NO] (M) 0.30 0.60 0.60 [H2] (M) 0.35 0.35 0.70 Rate (mol/L/s) 2.835103 1.134102 2.268102
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?
The mechanism for the gas-phase reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be NO2+NO2NO3+NOSlowNO3+CONO2+CO2Fast Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction?
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.

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If a temperature increase from 10.0 °C to 20.0 ° C doubles the rate constant for a reaction, what is the value of the activation barrier for the reaction? Ea = kJ/mol