Consider the bimolecular reaction of nitrogen dioxide at 750 K in the gasphase, producing NO and O2 as follows:2NO22NO + O2.Suppose that the Arrhenius parameter (frequency factor A) is given as 1.79 x 106m³ mol¹ s¹ and the actual cross-section for a reactive collision is σ = 0.60 nm².Calculate the reactive cross section (σ*) and the steric factor, P.HINT: take μ = 1/2m(NO2)And MNO2 = 46.0mu, where mu is the atomic mass constant.

calculate μ (reduced mass): μ = ½m(NO₂) = ½ * 46.0mu = 23.0muconvert the temperature from K to J…

Answered: Consider the bimolecular reaction of…

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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A rate constant is found to fit the expression kr = Ae−(4972 K)/T with A = 4.98 × 1013 dm3 mol−1 s−1 near 25 °C. Calculate Δ‡G for the reaction at 25 °C; assume κ = 1.
The frequency factor for a second-order gas-phase decomposition of a species at low pressures is 2.3 × 1013 dm3 mol−1 s−1 and its activation energy is 30.0 kJ mol−1. What are (i) the entropy of activation, (ii) the enthalpy of activation, (iii) the Gibbs energy of activation at 298 K? Assume κ = 1.
The rate constant for the reaction 2NO2 → 2NO + O2 is experimentally determined to be 0.153 mol−1 dm3 s −1 at 300°C and 0.993 mol−1 dm3 s −1 at 350°C. Estimate the effective radius of an NO2 molecule. The steric factor for this reaction is 0.05.
Suppose it is known that ozone adsorbs on a certain surface in accord with a Langmuir isotherm. How could you use the pressure dependence of the fractional coverage to distinguish between adsorption (i) without dissociation, (ii) with dissociation into O + O2, (c) with dissociation into O + O + O?
The adsorption of a gas is described by the Langmuir isotherm with α = 0.75 kPa−1 at 25 °C. Calculate the pressure at which the fractional surface coverage is (i) 0.15, (ii) 0.95.
For the gas-phase reaction A + A → A2, the experimental rate constant, kr, has been fitted to the Arrhenius equation with a frequency factor A = 4.07 × 105 dm3 mol−1 s−1 at 300 K and an activation energy of 65.4 kJ mol−1. Calculate Δ‡S, Δ‡H, Δ‡U, and Δ‡G for the reaction.
25) Consider the following set of reactions. Assume that A, B, C and D are atoms. (1) A + A → B (2) А-В + С-D А-С-D-B (3) A + B-C → A-B-C Order these reactions in terms of increasing significance of the orientation probability (that is the A in the Arrhenius equation). А. (1) (2) < (3) В. (3) < (2) <(1) C. (1) < (3) <(2) D. (1) = (2) = (3) E. (1) < (2) = (3)
As described in Problem P17D.5, reaction with the hydroxyl radical OH is the main path by which CH4 is removed from the lower atmosphere. T. Gierczak et al. (J. Phys. Chem. A 101, 3125 (1997)) measured the rate constants for the bimolecular gas-phase reaction CH4 + OH → CH3 + H2O and found A = 1.13 × 109 dm3 mol−1 s−1 and Ea = 14.1 kJ mol−1 for the Arrhenius parameters. (a) Estimate the rate of consumption of CH4 under the following conditions: take the average OH concentration to be 3.5 × 10−15 mol dm−3, that of CH4 to be 40 nmol dm−3, and the temperature to be −10 °C. (b) Estimate the global annual mass of CH4 consumed by this reaction (which is slightly less than the mass introduced to the atmosphere) given an effective volume for the Earth’s lower atmosphere of 4 × 1021 dm3.
Estimate the magnitude of the primary kinetic isotope effect on the relative rates of displacement of 1H and 3H in a C–H bond. Will raising the temperature enhance the difference? Take kf(C–H) = 450 N m−1.
For the gaseous reaction A + B → P, the reactive cross-section obtained from the experimental value of the frequency factor is 9.2 × 10−22 m2. The collision cross-sections of A and B estimated from the transport properties are 0.95 nm2 and 0.65 nm2, respectively. Calculate the steric factor, P, for the reaction.
The degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.
In the dimerization of methyl radicals at 25 °C, the experimentally determined frequency factor is 2.4 × 1010 dm3 mol−1 s−1. What are (a) the reactive cross-section, and (b) the steric factor for the reaction given that the C–H bond length is 154 pm?

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