P17E9* J. Czarnowski and H.J. Schuhmacher (Chem. Phys. Lett. 17, 235 (1972)) suggested the following mechanism for the thermal decomposition of F,O in the reaction 2 F,O(g) → 2 F,(g) + 0,(g): (1) F,O + F,0 → F+ OF + F,0 k, (2) F+F,O → F, + OF k, (3) OF + OF → O, + F+F ke (4) F+F+F,O → F, + F,0 ka Use the steady-state approximation to show that this mechanism is consistent with the experimental rate law –d[F,O]/dt = k,[F,O]² + K{[F,O]².

P17E9* J. Czarnowski and H.J. Schuhmacher (Chem. Phys. Lett. 17, 235 (1972)) suggested the following mechanism for the thermal decomposition of F,O in the reaction 2 F,O(g) → 2 F,(g) + 0,(g): (1) F,O + F,0 → F+ OF + F,0 k, (2) F+F,O → F, + OF k, (3) OF + OF → O, + F+F ke (4) F+F+F,O → F, + F,0 ka Use the steady-state approximation to show that this mechanism is consistent with the experimental rate law –d[F,O]/dt = k,[F,O]² + K{[F,O]².

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

Discuss the featu res. applications. and limitations of the Michaelis-Menten mechanism of enzyme action .
Derive the rate law for the reaction 2NO + O2 -> 2 NO2 with the following mechanism : NO + O2 -> NO3 K1 NO3 -> NO + O2 K2 NO3 + NO -> 2NO2 K3
10. The rate of change in colour of iodide (yellow) can be measured as it reacts with colourless hypochlorite, OCI (ag): I (aq) + OCI(aq) I0- (aq) + Cl (aq) a. Different concentrations of reactants are combined at the same temperature and the rate of yellow colour disappearance were measured: Rate of colour Trial Initial [I] (mol/L) Initial [OCI(ag)) change (mol/(L s) 0.12 0.18 7.91 x 102 1 0.18 3.95 x 102 0.060 0.090 0.030 9.88 x 103 3 0.24 7.91 x 102 4 0.090 Using the data provided, calculate the value of the rate constant, including units b. Predict the rate of reaction if both reactants have an equal starting concentration of 0.10 mol/1.
Distinguish between kinetic and the rmodynamic control of a reaction. Suggest criteria for expecting one rather than the other.
The conversion of high molecular weight olefins into saturated hydrocarbons makes use ofH 2 and is a heterogeneous process catalyzed by nickel. Draw and describe the mechanismaccording to the LH mechanism.
WRITE C OM PLETE MECHANISMI
The Arrhenius parameters for the gas-phase decomposit ion of cyclobutane, C4H8(g)→ 2 C2H4(g). are log(A/s-1) = 15.6 and Ea = 261 kJ mol- 1. What is the ha lf- life of cyclobutane at (a) 20 °C, (b) 500 °C?
Calculate the magnitude of the diffusion-controlled rate constant at 298 K for a species in (a) water, (b) pentane. The viscosit ies are 1.00 x 10-3 kg m-1 s-1 and 2.2 x 10-4 kg m-1 s-1.respectively.
Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1. If the reaction is subject to a temperature jump, derive the equation for d[D]/dt in terms of a relaxation constant t.
It has been proposed that the gas NO2C1 decomposes by the mechanism: NO2CI(g) kı NO2(g) + Cl(g) NO2CI(g) + Cl(g) k2 NO2(g) + Cl2(g) Apply the Steady State Approximation to derive an expression for the concentration of the intermediate, Cl(g). Show your working out. States not required.
Distinguish between a first-order phase transition, a second-order phase transition, and a λ-transition at both molecular and macroscopic levels.