Use the References to access important values if needed for this question. The decomposition of ammonia on a platinum surface at 856 °C NH3 1/2 N2 + 3/2 H2 is zero order in NH3 with a rate constant of 1.50x10 6 Ms1 If the initial concentration of NH3 is 1.28x10 2 M, the concentration of NH3 will be M after 7.54x103 seconds have passe Submit Answer Try Another Version 3 item attempts remaining

Use the References to access important values if needed for this question. The decomposition of ammonia on a platinum surface at 856 °C NH3 1/2 N2 + 3/2 H2 is zero order in NH3 with a rate constant of 1.50x10 6 Ms1 If the initial concentration of NH3 is 1.28x10 2 M, the concentration of NH3 will be M after 7.54x103 seconds have passe Submit Answer Try Another Version 3 item attempts remaining

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.13QAP: Copper(II) forms a 1:1 complex with the organic complexing agent R in acidic medium. The formation...

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The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
Copper(II) forms a 1:1 complex with the organic complexing agent R in acidic medium. The formation ofthe complex can be monitored by spectrophotometry at 480 nm. Use the following data collected under pseudo-first-order conditions to construct a calibration curve of rate versus concentration of R. Find the concentration of copper(II) in an unknown whose rate under the same conditions was 6.2 10- 3A s-1.
The following data were obtained on the initial rates of reaction of a d-metal complex in aqueous solution. For the experiments a. [Y] = 2.7 mmol/dm3, and for experiments b. [Y] = 6.1 mmol/dm3 Conc. complex/(mmol dm-3) 8.01 9.22 12.11 Exp. a. v/ (mol dm-3 s-1) 125 144 190 Exp. b. v/ (mol dm-3 s-1) 640 730 960 b) use the data above to calculate the rate constant. k = ________ (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal format.
The following data were obtained on the initial rates of reaction of a d-metal complex in aqueous solution. For the experiments a. [Y] = 2.7 mmol/dm3, and for experiments b. [Y] = 6.1 mmol/dm3 Conc. complex/(mmol dm-3) 8.01 9.22 12.11 Exp. a. v/ (mol dm-3 s-1) 125 144 190 Exp. b.   v/ (mol dm-3 s-1) 640 730 960 (a) What is the order of reaction with respect to the complex AND the reactant Y. Choose one. (b) use the data above to calculate the rate constant. k = ________ (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal format.
The following data were obtained on the initial rates of reaction of a d-metal complex in aqueous solution. For the experiments a. [Y] = 2.7 mmol/dm3, and for experiments b. [Y] = 6.1 mmol/dm3 Conc. complex/(mmol dm-3) 8.01 9.22 12.11 Exp. a. v/ (mol dm-3 s-1) 125 144 190 Exp. b.   v/ (mol dm-3 s-1) 640 730 960 (a) What is the order of reaction with respect to the complex AND the reactant Y. (b) use the data above to calculate the rate constant. k = ________ (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal format.
The following data were obtained on the initial rates of reaction of a d-metal complex in aqueous solution. For the experiments a. [Y] = 2.7 mmol/dm3, and for experiments b. [Y] = 6.1 mmol/dm3 Conc. complex/(mmol dm-3) 8.01 9.22 12.11 Exp. a. v/ (mol dm-3 s-1) 125 144 190 Exp. b.   v/ (mol dm-3 s-1) 640 730 960 (a) What is the order of reaction with respect to the complex AND the reactant Y. Choose one.
Theoretically, it was concluded that the activation energy required to form one interatomic atom, (one void) of copper is approximately (4ev), assuming that this value is correct. Calculate the concentration of these defects (vacuum per cm^3) at the thermal equilibrium degree (1350k).
Calculate the concentration of vacancies in in fcc silver at 250 oC given that the activation energy for vacancy creation in silver is 79.5 kJ/mol. The units for your answer should be vacancies/cm3
Benzene on graphite follows the Langmuir isotherm. At a pressure of 1 atm, theThe volume of benzene adsorbed on a sample of graphite was 4.2 mm3 atconditions T = 0°C and 1 atm. At 3 atm it was 8.5 mm3. Suppose 1 molecule ofbenzene occupies 30Å and estimate the surface area of graphite.
A metal has a certain fraction f = 10-5 of vacancies at the atomic level at finite temperatures. If the activation energy for vacancy formation was increased by 50%, what would be the new vacancy concentration? a. 5.48E-4 b. 6.22 E-5 c. 1.24E-6 d. 7.43E-10 e. 3.16E-8
For the reaction NH2SO2OH + H2O → NH4HSO4 In aqueous solution at 80.35oC, the following constants were observed at the indicated ionic strength μ x103 k (L/mol hr) 5.06 1.07 11.21 1.02 15.85 0.976 22.94 0.886 From these data ascertain: a.) the valence of the reacting ions and b.) the rate constant for the primary salt effect.
The molecu le 2,2'-bipyridine (1, bpy) forms a complex with the Ru2+ ion. Ruthenium(ll) tris-(2,2'-bipyridyl), Ru(bpy)3,2+(2), has a strong electronic absorpt ion at 450 nm . The quenching of the * Ru(bpy)3 2+ excited state by Fe(OH2)63+. in acidic solution was monitored by measuring excited state lifetimes at 600 nm. Determine the quenching rate constant for this reaction from the following data: