3. The following activation parameters have been measured (30 °C in MeOH) for the reaction trans-[PtL2Cl2] + py k2 [PtL2Clpy] + CH L AH+/kJ mol-1 AS/J K¹ mol-1 AV/cm³ mol-1 pyridine 49.3 -94 -8.8 PEt3 53.9 -100 -13.6 i. Explain briefly how the parameters are determined experimentally. ii. What mechanistic information can be obtained from the values? iii. Calculate the rate constant at 25.0 °C when L = pyridine

3. The following activation parameters have been measured (30 °C in MeOH) for the reaction trans-[PtL2Cl2] + py k2 [PtL2Clpy] + CH L AH+/kJ mol-1 AS/J K¹ mol-1 AV/cm³ mol-1 pyridine 49.3 -94 -8.8 PEt3 53.9 -100 -13.6 i. Explain briefly how the parameters are determined experimentally. ii. What mechanistic information can be obtained from the values? iii. Calculate the rate constant at 25.0 °C when L = pyridine

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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Use the References to access important values if needed for this question. For the gas phase isomerization of methyl cis-cinnamate, cis-C6H5 CH=CHCOOCH3 → trans-C6H5 CH=CHCOOCH3 the rate constant at 669 K is 9.12 x 10-4 s and the rate constant at 711 Kis 5.79 x 107 s-¹. -3 The activation energy for the gas phase isomerization of methyl cis-cinnamate is kJ.
7 8 t n= (1.01atm x 0-03461) k (0.092/Lalm/mol .k x 292k) - 0.00 n=0.0014577mel Hz in the reaction Mgcl2 (a9) tH2 9) mass df Mg use ng ) + HCl (aa) Imol of H2 9as produced Imol af mg mass of mg O-00/4577 md mg mg=O:014577x 24.3059/mol 0.03549 =0-0353
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 mol/dm³, and for experiments b. [Y] = 6.1 mol/dm³ Conc. complex/(mol dm-3) Exp. a. v/ (mol dm-3 s-1) Exp. b. v/ (mol dm-3 s-1) O oth order O 1st order O 2nd order O 3rd order 8.01 QUESTION 4 125 640 9.22 (b) use the data above to calculate the rate constant. k= 144 730 (a) What is the order of reaction with respect to the complex AND the reactant Y. Choose one. 12.11 (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal format. 190 960
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 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.
Name: Date: Section: Data Sheet: Investigation of Nickel and Copper Coordination Complexes Part B: The Coordination Number of Ni* Mass of Ni(NO,)2.6H,0 Volume of Deionized H,0 2441.2 291 マリトて Concentration of Ni?* Solution o 91 Moles Ni+ TRIAL #Initial TemperatureFinal TemperatureqreactionAH, reaction- Average Bond Energy Coordination Number of Ni?+ 165
6. Calculate Kc for 2N204(6) + 3021e) - 2N20 (e) K=? using.. Reaction 1 2N2e) + O2le) - 2N,0 (2) K, = 1.2 x 1035 2NO2 (6) K2 = 4.6 x 103 Reaction 2 ½ N21e) + O218) e NO2 (2) K3 = 4.1 x 10° Reaction 3
Cc.80.
The free energy change, AG, in the homogenous cross-exchange ET reaction of [Ru(bpy)2]* and ferricytochrome c is -104.6 kJ mol¯1. The second-order activation-limited rate constant, kobs, is 2.5 × 108 M-1 s-1. Taking KDA = 1.0 M¹, N = 1 × 1011 s-1, and x = 1, estimate the values of AG* and 2. In what kinetic region is this reaction? Hint: By substituting the Marcus equation into the expression for the rate constant of an adiabatic homogenous ET reaction, the rate constant of a cross-exchange ET reaction may be written as (AG+2)² Ket = KVN exp - 4λRT and, by rearrangement, In Ket KV 1 (AG+ 2)² 1 AG2 1 AG == + constant 42 RT 42 RT 2 RT
On the graph below, draw a potential energy diagram for the following reaction: Q + R -> S + T PE of Q + R = 150 kJ PE of S + T = 250 kJ PE of the activated complex = 375 kJ
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