Part A The following data show the rate constant of a reaction measured at several different temperatures. Use an Arrhenius plot to determine the activation barrier (E) for the reaction. Temperature (K) Rate constant (1/s) Express your answer using three significant figures. 310 0.413 320 1.15 330 3.01 340 7.43 ΑΣφ ? 350 17.4 Ea kJ/mol Submit Request Answer Part B Use an Arrhenius plot to determine the frequency factor for the reaction. Express your answer using two significant figures. ? A =

Part A The following data show the rate constant of a reaction measured at several different temperatures. Use an Arrhenius plot to determine the activation barrier (E) for the reaction. Temperature (K) Rate constant (1/s) Express your answer using three significant figures. 310 0.413 320 1.15 330 3.01 340 7.43 ΑΣφ ? 350 17.4 Ea kJ/mol Submit Request Answer Part B Use an Arrhenius plot to determine the frequency factor for the reaction. Express your answer using two significant figures. ? A =

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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The data below show the rate constant of a reaction measured at several different temperatures Temperature (K) Rate Constant (s) 26.9164 66.1282 153.588 338.961 714.003 300 310 320 330 340 Part A Use an Arrhenius plot to determine the activation barrier for the reaction Express your answer in kilojoules per mole to three significant figures. VAE E₁= Submit Part B A= Submit Request Answer Use an Arrhenius plot to determine frequency factor for the reaction. Express your answer in reciprocal seconds to two significant figures. ΑΣΦΑ Provide Feedback ? Request Answer kJ/mol ? ri
use an Arrhenius plot to determine the activation barrier
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Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
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The rate constant k for a certain reaction is measured at two different temperatures: temperature k 61.0 °C 6.7 x 10° -76.0 °C 4.5 x 10* Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E x10 a mol II
12. The reaction was run at a higher temperatures. At 37.0 °C, the rate constant was measured to be 0.584 M-¹-¹ and at 120.0 °C, it was 10.641 M¹s. What is Ea (kJ/mol)? Give your answer in the #12 blank with 3 significant figures and units.
Use the information provided in the table below to answer the next two questions. The reaction between reactants A and B was studied at-10 °C. The following results were obtained. Experiment Initial [A] (mol/L) Initial [B] (mol/L) Initial Reaction Rate (M/min) 1 0.10 0.10 0.18 0.10 0.20 0.36 3 0.20 0.20 1.45 11. What is the order with respect to [B]? (a) 1 (b) 2 (c) ½ (d) 0 12. What is the order with respect to [A]? (a) 1 (b) 2 (c) ½ (d) 0
The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is