The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place according to thefollowing chemical equation:Fe(phen) 3 24 + 3 H 30 * + 3 H 20 Fe(H 20) 6 2*+.+ 3 phenHIf the activation energy, E a, is 126 kj/mol and the rate constant at 30°C is 9.8 x 10 -3 min-1. what is the rate constant at 45°C?9.6 x 10° min 11.1 x 10 min 19.3 x 10" min 11.1 x 10° min 1

Answered: Image /qna-images/answer/14d6aa18-dc16-442d-9517-3b25c76dc4f5.jpg

The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place according to the following chemical equation: Fe(phen) 3 2+ +3 H 30* +3 H 20 → Fe(H 20) 6 2+ + 3 phenH If the activation energy, E a, is 126 kJ/mol and the rate constant at 30°C is 9.8 x 10 -3n min -1. what is the rate constant at 45°C? 9.6 x 10° min-1 1.1 x 10' min 1 9.3 x 10 min 1 1.1 x 10 min1

The aquation of tris(1,10-phenanthroline)iron(II) in acid solution takes place according to the following chemical equation: Fe(phen) 3 2+ +3 H 30* +3 H 20 → Fe(H 20) 6 2+ + 3 phenH If the activation energy, E a, is 126 kJ/mol and the rate constant at 30°C is 9.8 x 10 -3n min -1. what is the rate constant at 45°C? 9.6 x 10° min-1 1.1 x 10' min 1 9.3 x 10 min 1 1.1 x 10 min1

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 108CP: The decomposition of NO2(g) occurs by the following bimolecular elementary reaction:...

See similar textbooks

Similar questions

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.)
Aluminum forms a 1:1 complex with 2-hydroxy-1-naphthaldehyde p -methoxybenzoylhydraxonal, which absorbs UV radiation at 285 nm. Under pseudo-first-order conditions, a plot of the initial rate of the reaction (absorbance units per second) versus the concentration of aluminum (in M) yields a straight linedescribed by the equation rate =1.92 c Al- 0.250 Find the concentration of aluminum in a solution that exhibits a rate of 0.53 absorbance units per second under the same experimental conditions.
You and a coworker have developed a molecule thathas shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law Rate=k[AV]1[V]1 You have been given the following data from your coworker: [V]0=0.20M[AV]0=1.0104M A plot of ln[AV] versus t(s) gives a straight line with a slope of 0.32 s1. What is the value of the rate constant (k) for this reaction?
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2NO2(g)2NO(g)+O2(g) The rate constant at 273 K is 2.3 1012 L/mol s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.5 atm to 1.5 atm at 500. K? Assume ideal gas behavior.
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
The rote of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20C. The following data were collected with all concentration units in mol/L. (A hemoglobin concentration of 2.21 mol/L is equal to 2.21 106 mol/L.) [Hb]0(mol/L) [CO]0(mol/L) Initial Rate (mol/L s) 2.21 1.00 0.619 4.42 1.00 1.24 4.42 3.00 3.71 a. Determine the orders of this reaction with respect to Hb and CO. b. Determine the rate law. c. Calculate the value of the rate constant. d. What would be the initial rate for an experiment with [Hb]0 = 3.36 mol/L and [CO]0 = 2.40 mol/L?
In the presence of excess thiocyanate ion, SCN, the following reaction is first order in chromium(III) ion, Cr3; the rate constant is 2.0 106/s. Cr3+(aq)+SCN(aq)Cr(SCN)2+(aq) What is the half-life in hours? How many hours would be required for the initial concentration of Cr3 to decrease to each of the following values: 25.0% left, 12.5% left, 6.25% left, 3.125% left?