36. The gas-phase reaction 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 × 105 745 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.

36. The gas-phase reaction 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 × 105 745 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

Consider the reaction X → Y + Z. Write an expression for the rate law
The reaction C4H8(g)→2C2H4(g) Ea = 262 kJ/mol, T = 600K, k = 6.1\times 10-8 s-1. What is the value of the rate constant at 800.0 K?
For the gas phase decomposition of t-butyl alcohol, (CH3)3 COH → (CH3)2C=CH2 + H₂O -1 the rate constant has been determined at several temperatures. When In k in s¯¹ is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -3.30 × 104 K and a y-intercept of 33.8. The activation energy for the gas phase decomposition of t-butyl alcohol is kJ/mol.
С,Н, Br, (аq) + 3Г (аq) С, Н, (g) + 2 Br (aq) + I; (aq) The rate law is k[C,H,Br, ][I¯] rate = where k = 0.00526 M-'. s-1. •S What are the missing entries in the table? Run [C,H,Br,lo (M) | [I-lo (M) Initial rate of formation of C,H, (M-s -1) 1 0.278 0.00163 2 0.278 y 0.000813 3 0.278 0.278 x = M y = M M-s-1 = Z
The rate constant for a certain reaction is k = 1.60x10-3 s-1. If the initial reactant concentration was 0.900 M, what will the concentration be after 17.0 minutes? Express your answer with the appropriate units.
Calculate the rate constant, ?k, for a reaction at 69.069.0 °C that has an activation energy of 81.581.5 kJ/mol and a frequency factor of 5.23×10 11 s−1. k=
How to use calculus to integrate the differential rate law and obtain the first-order integrated rate law. k[A] = -∆k[A] / ∆t -----> ln[A]t = -kt + ln[A]0
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.
Calculate the rate constant, k, for a reaction at 60.0 °C that has an activation energy of 77.7 kJ/mol and a frequency factor of 6.59 x 101 s-1. k =
Consider the following elementary reaction: NO2(g)+F2(g)→NO2F(g)+F(g) Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of NO2F in terms of k1, k−1, and the equilibrium concentrations of NO2, F2, and F. [NO2F] =
A possible mechanism for the next decomposition reaction is A(g) ⇄ 2B(g) + C (fast equilibrium) C + A(g) → 2B(g) (slow) What is a rate law that is consistent with this mechanism?
The formation of nitrosyl chloride is described by the following chemical equation: 2NO (g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Cl₂ (g) NOCI₂ (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 11 × Ś