P17D.4 The second- order rate constants for the reaction of oxygen atoms with aromatic hydrocarbons have been measured (R. Atkinson and J.N. Pitts, J. Phys. Chem. 79, 295 (1975)). In the reaction with benzene the rate constants are 1.44 x 10 dm3 mol s at 300.3 K, 3.03 x 10 dm mol s at 341.2 K, and 6.9 x 10 dm3 mols at 392.2K. Find the frequency factor and activation energy of the reaction.
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- The rate constant for the fi rst-order decomposition of N2O5 in the reaction 2 N2 O5(g) → 4 NO2(g) + O2(g) with v = kr[N2O5] is kr = 3.38 x 10-5 s-1 at 25 oC. What is the ha lf- life of N2O5? What w ill be the total pressure, init ial ly 78.4 kPa for the pure N2O5 vapour, (a) 5.0 s, (b) 5.0 min after init iation of the reaction?The diameter of the methyl radical is about 308 pm. What is the maximum rate constant in the expression d[C2H6]/dt = kr[CH3]2 for second-order recombination of radicals at 298 K? It is reported that 10 per cent of a sample of ethane of volume 1.0 dm3 at 298 K and 100 kPa is dissociated into methyl radicals. What is the minimum time for 90 per cent recombination?Give clear handwritten answer- Derive an expression for the time dependence of the degree of polymerization (the average number of monomer residues per polymer molecule) for a condensation polymerization in which the reaction is known to have rate law d[M]/dt = -k[M] 3 , where [M] represents the concentration of the monomer!
- Why may some gas-phase reactions show fi rst-order kinetics?The second-order rate constants for the reaction of oxygen atoms ·with aromatic hydrocarbons have been measured (R. Atkinson and J.N . Pitts, J. Phys. Chem. 79, 295 (1975)). In the reaction with benzene the rate constants are 1.44x 107dm' mor ' s ' at 300.3 K, 3.03 x 107 dm' mol"'s"' at 34 1.2K, and 6.9 x 107 dm' mor's ' at 392.2K. Find the frequency factor and activation energy of the reaction.The composition of a liquid phase reaction 2A → B was monitored by aspectrophotometric method with the following results: t, s [B], mol/L 0 0 600 0.089 1200 0.153 1800 0.200 2400 0.230 ∞ 0.312 Identify the rate law, integrated rate law, and rate constant for thereaction based on the obtained data.
- The oxidation of HSO3− by O2 in an aqueous solution is a reaction of importance to the processes of acid rain formation and flue gas desulfurization. R.E. Connick et al. (Inorg. Chem. 34, 4543 (1995)) report that the reaction 2 HSO3−(aq) + O2(g) → 2 SO42−(aq) + 2 H+(aq) follows the rate law v = kr[HSO3−]2[O2]2. Given pH = 5.6 and an O2 molar concentration of 0.24 mmol dm−3 (both presumed constant), an initial HSO3− molar concentration of 50 μmol dm−3, and a rate constant of 3.6 × 106 dm9 mol−3 s−1, what is the initial rate of reaction? How long would it take for HSO3− to reach half its initial concentration?The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.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 320 K for the recombination of two atoms in benzene, for which η = 0.601 cP. Assuming the concentration of the reacting species is 2.0 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.Distinguish between kinetic and the rmodynamic control of a reaction. Suggest criteria for expecting one rather than the other.Given the 1st order rxn A(g) --- > B(g) + C(g) + 3D(g) with a rate constant of 6.0x10-4 s-1 at 298 K. With a starting mol of 1.00 mol of A(g), how long in seconds does it decrease to 0.500 mol?