(b) Consider the following elementary bimolecular gas-phase reactions below at 850K:H2 (g) 12 (g) → 2 HI (g)(i)Calculate the reduced mass, μ. HINT: take mн2 = 2.016mμ and m12 = 253.8mu(ii) Calculate the value of the second order rate constant for the reaction. The collisioncross-section is 0.36 nm², and the activation energy is 171 kJ mol-1.

Results: (i) Reduced Mass, μ: μ=2.000 u (ii) Second-Order Rate Constant, k: First, the…

Answered: (b) Consider the following elementary…

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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1. The mechanism of a certain non-elementary reaction is given below: (1) NO2Cl = NO2 + Cl k1, k-1 (2) Cl + NO2Cl → NO2 + Cl2 k2 derive (a) Using the steady-state approximation, the differential rate law for the formation of molecular chlorine, Cl2, as a function of time on the basis of the above mechanism.
The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O5 (g) 2N₂O₂(g) + O₂(g) Determine graphically the activation energy for the reaction. Be sure your answer has the correct number of significant digits. T(K)|*(--) S 298. 1.74 x 10 308. 6.61 × 10 318. 2.52 × 10 328. 7.59 × 10 338. 2.40 × 10 - 5 -5 -4 -4 3 Note: Reference the Fundamental constants table for additional information.
Obtain the 2"-1 – 1 | T (п - 1)k. а"-1 relation between the order of the reaction (n), the reaction rate constant (k), the initial concentration (a), and the half-life (T).
what is the activation energy for a first-order reaction if k = 2.5 x 10-3 s-1 at 332 K and k = 0.15 s-1 at 375 K?
For the first-order reaction N2O5( g) • 2 NO:(8) +0x8) t1/2 = 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1013 s-1, determine the value of k at 50°C. 3.
6
A gas phase reaction has a rate coefficient of 1.3·104 L mol–1s–1 at 300 K and its activation energy is 8.3 kJ mol–1. Indicate the order of the reaction.
The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3) 8.01 9.22 12.11v/(mol dm-3 s-1) (a) 125 144 190 (b) 640 730 960
The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g) NO(g) + ½ Cl½(g) is second order in NOCI with a rate constant of 5.90×10+ M's'. If the initial concentration of NOCI is 4.60×10 ² M, the concentration of NOCI will be 8.51x10 3M after seconds have passed.
(a) Distinguish between reactions rate and reaction mechanism (b) The following data were obtained for the reaction I'aq + OCI aq→ IO" + CI'aq [OCI ] [1] mol/dm3 Initial Rate mol/dm3 mol/dm?/s 1.8 x 103 3.6 х 103 2.1 x 103 5.4 x 105 2.1 x 103 10.8 x 10$ I II I 1.8х 103 (i)What is the order of the reaction with respect to [I'] and [OCI] (ii) Calculate the rate constant using the results of experiment II (iii) What is the rate law or rate equation for this reaction? 6.3х 103 4.9 x 104
56. For the first-order reaction 2 NO₂(g) + O₂(g) N₂O5(g) t1/2 = 22.5 h at 20 °C and 1.5 h at 40 °C. -1 (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.05 × 10¹³ s-¹, determine the value of k at 30 °C.
Enter your answer in the provided box. The variation of the rate constant with temperature for the first-order reaction 2N205(g) 2N204(g) + 02(g) is given in the following table. Determine graphically the activation energy in kJ/mol for the reaction. T(K)k(s1) 298 1.74 x 10-5 308 6.61 x 10-5 318 2.52 x 10 4 328 7.59 x 10 338 2.40 x 103 kJ/mol

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