Scheme 12. Sml2-Promoted Anionic DominoReactionон2 Sml270-90%4243OH

Answered: Scheme 12. Sml2-Promoted Anionic Domino…

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Scheme 12. Sml2-Promoted Anionic Domino Reaction OH 2 Sml2 70-90% 42 43 OH

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.6: Disturbing A Chemical Equilibrium

Problem 2.2ACP

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2. From the perspective of thermodynamics, the total free energy change of antibody (Ab) and antigen (Ag) interaction can be expressed as AG = -RTln(K·1M), where R = 8.3145 J/(mol·K) is the gas constant, T is the temperature in the unit of Kelvin (K = °C + 273.15), and K is affinity constant of Ab-Ag interaction. Note: 1M here means 1 Molar, so that affinity constant K has the unit of 1/M. A negative value of free energy change AG indicates energy release, while a positive value of free energy change AG indicates energy absorption. a) At body temperature T = 37°C, if we know the affinity constant K = 108/M, please compute the total free energy change AG. b) The presence of a single charged group on epitope or antigenic determinant of an antigen, typically increases the energy release by 20 kJ/mol for Ab-Ag interaction. Please compute the
have a rate 13.124. Testing for a Banned Herbicide Sodium chlorate w in EU countries since 2009. A simple colorimetric test for the presence of the chlorate ion in a solution of herbicide was used relies on the following reaction: 2 MnO4 (ag) + 5 C103 (aq) + 6 H*(aq) → 2 Mn2+ (aq) + 5 C104¯(ag) + 3 H,0(0) The table contains rate data for this reaction. [CIO3 ]o (M) [H*]% (M) Initial Rate [MnO4 lo (M) (Mis) Experiment 5.2 X 10 0.10 0.10 0.10 1 3.3x 10 0.10 0.10 0.25 1.6 x 10 0.10 0.30 0.10 7.4 X 103 0.20 0.10 0.10 4 HO THE Determine the rate law and the rate constant for this reaction. 3,125 T 3.
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
For the reaction PCglu) • Clzlo) true based on the above? PCIsla) at a particular temperature, Ke - 243. Suppose a system at that temperature is prepared with [PC31 -010 M. [C12)- 015 M. and [PCIs) - 0.60 M. Which of the following is Mukiple Choice Q > Ko the reection proceeds from left to right to resch equibrium Q Kg, the reaction proceeds from let so right to reach equibrium QcKo the reection is currenty at equilbrium Q >K, the reection proceeds from night t10 left to reach equlbnum Q
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.
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. (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.
with amine concentration as shown below. A time-resolved laser spectroscopy experiment had also shown that the half-life of the phosphorescence in the absence of quencher is 29 us. What is the value of k,? [Q/(mmol dm) 1.0 5.0 10.0 I/(arbitrary units) 0.41 0.25 0.16 P17G.4 When benzophenone is exposed to ultraviolet radiation it is excited into a singlet state. This singlet changes rapidly into a triplet, which phosphoresces. Triethylamine acts as a quencher for the triplet. In an experiment in the solvent methanol, the phosphorescence intensity varied
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+ Moore 5e_Ch11 SP2020.pptx: SP X * OWLV2 | Online teaching and lea X oping Cart | The UAB Blazer x VtakeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topica) [References) Use the References to access important values if needed for this question. In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + % I(g) the following data were obtained: HI), M 0.401 0.201 0.101 5.05x102 seconds 519 779 910 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.401 M is s and when the starting concentration is 0.201 M is req (2) 2req The average rate of disappearance of HI from t=0 s to t= 519 s is Ms! (3) The average rate of disappearance of HI from t = 519 s to t= 779 s is Ms! (4) Based on these data, the rate constant for this v order reaction is Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning | Cengage Technical Support Tch 55 F7…