36. The gas-phase reactionH+D2 → HD+Dis the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The followingdata were obtained for the rate constant k of this reaction:Temperature (K)k (L mol¬ s-1)2991.56 x 1043273.77 x 1043467.6 x 1014401065491.07 x 1067458.7 × 107(a) Calculate the activation energy of this reaction.(b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rateconstant.

Answered: Image /qna-images/answer/645f908a-f82f-40c5-a7c9-681774e78ff4.jpg

H+D2 → HD+D is the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The following data were obtained for the rate constant k of this reaction: Temperature (K) k (L mol¬1 s-1) 299 1.56 x 104 327 3.77 x 104 346 7.6 x 104 440 106 549 1.07 x 106 745 8.7 x 107 (a) Calculate the activation energy of this reaction. (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.

H+D2 → HD+D is the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The following data were obtained for the rate constant k of this reaction: Temperature (K) k (L mol¬1 s-1) 299 1.56 x 104 327 3.77 x 104 346 7.6 x 104 440 106 549 1.07 x 106 745 8.7 x 107 (a) Calculate the activation energy of this reaction. (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.

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...

See similar textbooks

Similar questions

Define:(i)Elementary reaction in a process (ii) Rate of a reaction.
4) Use the data below to determine the rate law and the value of k for the following reaction CHC13 (g) + Cl2 (9) → CC14 (g) + HCl (g) [CHCI3] (M) [Cl2] (M) Initial Rate 0.0035 Experiment 1 0.010 0.010 2 0.020 0.010 0.0069 3 0.020 0.020 0.0098 4 0.040 0.040 0.0270
Consider the mechanism. Step 1: 2 A = B + C equilibrium Step 2: В +D — E slow Overall: 2A + D — С +Е Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =
The rate constant for the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four temperatures shown in the table below. T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.
A certain reaction has an activation energy of 63.0 kJ mol−1kJ mol−1 and a frequency factor of A1�1 = 5.20×1012 L mol−1 s−1L mol−1 s−1 . What is the rate constant, k�, of this reaction at 29.0 ∘C∘C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash.
Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C2(NO2)6, decomposes according to the equation C2(NO2)6- 2NO, + 4NO + 2CO, The reaction in CCl, solvent is first order with respect to Cz{NO2)s At 63.7°C, k= 0.000254 s* and at 112.6°C, k = 0.0126s*. (a) What is the half-life of C2{NO2); at 63.7 °C? i seconds e Textbook and Media (b) What is the half-life of C2(NO2)s at 112.6 °C? seconds (c) IF0.100 mol of C2(NO2)6 is dissolved in CCI4 at 63.7°C to give 1.00 L of solution, what will be the C2(NO2), concentration after 50.0 minutes? i M (d) What is the value of the activation energy of this reaction, expressed in kilojoules? i kJ/mol (e) What is the rate constant at 159.4 °C?
Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C₂(NO2)6, decomposes according to the equation C₂(NO2)6→ 2NO2 + 4NO+2CO2 The reaction in CCl4 solvent is first order with respect to C₂(NO₂)6. At 73.8 °C, k = 0.000330 s¹ and at 103.0 °C, k=0.0189 s ¹. (a) What is the half-life of C₂(NO2)6 at 73.8 °C? i eTextbook and Media (b) What is the half-life of C₂(NO₂)6 at 103.0 °C? i seconds (c) If 0.100 mol of C₂(NO2)6 is dissolved in CCl4 at 73.8°C to give 1.00 L of solution, what will be the C₂(NO2)6 concentration after 50.0 minutes? i M (e) What is the rate constant at 154.8 °C? i seconds (d) What is the value of the activation energy of this reaction, expressed in kilojoules? kJ/mol 51
Find the rate law equation and the value of k.
The reaction 2A--->P has a rate constant k= 3.50 x 10-4 dm6 mol-2s-1What is the order of this reaction? Why?
The values of the rate constant for the A→Products reaction are given in the table below with the change of temperature. Find the activation energy for this reaction. k 0.027 0.040 0.059 0.085 0.12 0.17 0.24 t (oC) 1 6 11 16 21 26 31
6
-1 For a certain reaction, the frequency factor A is 7.5 × 10⁹ s1 and the activation energy is 21.4 What is the rate constant for the reaction at 95. °C? Round your answer to 2 significant digits. Note: Reference the Fundamental constants table for additional information. k = -1 S X kJ mol S