c. Ea for the uncatalyzed reaction 03 (9) + O(g) → 20,(9) is 14.0 kJ. E, for the same reaction when catalyzed is11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 23°C? Assume the frequency factor A is the same for each reaction. Ratio =

c. Ea for the uncatalyzed reaction 03 (9) + O(g) → 20,(9) is 14.0 kJ. E, for the same reaction when catalyzed is11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 23°C? Assume the frequency factor A is the same for each reaction. Ratio =

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

None
ess important values if needed for this question. For the decomposition of hydrogen lodide on a gold surface at 150 °C 2 HI(g) → H₂(g)+ 12 (9) the average rate of disappearance of HI over the time period from t=0s to t=2610s is found to be 1.20 x 10 M-s¹. The average rate of formation of I₂ over the same time period is M-s Submit Answer Retry Entire Group 9 more group attempts remaining
14.70 b A reaction has a rate constant of 1.26×10−4 s−1s−1 at 27 ∘C ∘C and 0.226 s−1s−1 at 77 ∘C ∘C .
For the gas phase decomposition of nitrogen dioxide at 383 °C 2 NO2 2 NO +02 the following data have been obtained: [NO2], M time, s 6.85x10 2 3.25x102 2.13x102 0 30.0 60.0 1.55x10-2 90.0 The average rate of disappearance of NO2 over the time period from t = 30.0 s to t = 60.0 s is Submit Answer Retry Entire Group 8 more group attempts remaining Ms.
Q4
How Rate laws for new reactions with unknown mechanisms are determined ?
Explain each criteria for determining a rate law through elementary steps and why it is important to fulfil both to have a correct rate law.
he rate constant of a chemical reaction increased from 0.100 s−1s−1 to 3.30 s−1s−1 upon raising the temperature from 25.0 ∘C∘C to 43.0 ∘C∘C . Calculate the value of (1T2−1T1)(1�2−1�1) where T1�1 is the initial temperature and T2�2 is the final temperature. Express your answer numerically. View Available Hint(s)for Part ACalculate the value of ln(k2k1) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.Express your answer numerically.View Available Hint(s)for Part What is the activation energy of the reaction?Express your answer numerically in kilojoules per mole.View Available Hint(s)
In the reaction N2 +3 H2 à 2NH3 if the Δ[H2]/t is -1.5 x 10-3 M/s, What is the Δ[NH3] at the same point? (How fast is the NH3 being produced)?
Use the References to access important values if needed for this question. of cyclopropane to propene at 500 °C The rearrangement (CH₂)3 CH3 CH=CH2 is first order in (CH2)3 with a rate constant of 6.70 x 10- 4 S -1 If the initial concentration of (CH₂)3 is 0.141 M, the concentration of (CH₂)3 will be 0.0180 M after s have passed. Submit Answer Retry Entire Group 7 more group attempts remaining
ints eBook Print References Enter your answer in the provided box. The rate constant for the following elementary reaction is 2.4 x 10° M2.5¹ at 25°C: 2C(g) 2A(g) +B(g) - - 0 AG (kJ/mol) A 85.972 B0 C 54.414 What is the rate constant for the reverse reaction at the same temperature? 0.07 M21
Given the following data for the reaction AB, determine the frequency factor, A, of the reaction to three significant figures. k(5¹) 0.730 0.739 T(K) 2.50 102 4.50 x 10² a) -0.287 s1¹ b) 2.05 ¹ Od 0.719 s¹¹ d) 0.287 s e) 0.750 1