A kinetic isotope effect (km/KD) of-1.05 has been estimated for the following reaction. Please provide a reasonable explanation for the origin of this kinetic isotope effect. F3C. H/D. Br F.BF3 50 °C Br F3C H/D. Br

A kinetic isotope effect (km/KD) of-1.05 has been estimated for the following reaction. Please provide a reasonable explanation for the origin of this kinetic isotope effect. F3C. H/D. Br F.BF3 50 °C Br F3C H/D. Br

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the accepted value for the Ksp of Ca(OH)2, including the conditions for its determination?
4) a) A reaction chamber is divided into two sections by a partition on which a valve is inserted. One section contains pure gas A and the other section has a mixture of gases A and B. What happens when the valve is opened? Explain this process in terms of chemical potential. b) The decomposition of etane into etene and hydrogen takes places at 1000 K and under 1 bar total pressure. C,H6(g) → C2H48) + H2«g) The composition of the mixture at equilibrium is as follows : H2(g): 32, C2H4(g): 32, and C,H6(g):36 (mol, %). According to the data; Calculate K, at 1000K Calculate Kp at 298.15 K, AH° = 145 kJ/mol Calculate AG° at 298.15 K
One of the major factors influencing seasonal ozone loss in the Antarctic winter is the dimerization of CIO in the stratosphere. The equilibrium constant (K) for the reaction 2 CIO(g) → (CIO)2 (g) at different temperatures is shown below. (Data obtained from Nature 332, 796 (1988)). • T(K) 233 248 258 268 273 280 288 295 303 4.13 5.00 1.45 5.37 3.20 K 9.62 4.28 1.67 7.02 ×108 ×107 ×107 ×106 ×106 ×10$ x105 ×105 ×104 a) Determine the standard enthalpy and standard entropy of this reaction. b) Calculate the standard enthalpy of formation and the standard molar entropy of (CIO)2 given that AH°(CIO) = 101.8 kJ/mol and AS° (cio) = 226.6 J/molk
b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
Calculate the value of the equilibrium constant, Ke, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Ke = M(g) = Z(g) 6R(g) = 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) .116 Kel = 3.57 Kc2 = 0.524 Kc3 = 14.6
1) Discuss the factors affecting the sign of AG in the relationship AG= AH - TAS. Give examples for cach of the situations.
Will calcium carbonate CaCO3 change its physical properties (for example, solubility in hydrochloric acid or will it become less bioavailable for human assimilation) if it is previously subjected to prolonged heat treatment at a temperature of 100 degrees Celsius?
Calculate the value of the equilibrium constant, Ke, for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) Z(g) 6 R(g) = 2 N(g) +4Z(g) 3 X(g) +3Q(g) 9 R(g) Kel 3.88 Kez = 0.445 %3D Ke3 = 13.5 %3D
18. From the following reacțions and thermal data at 25°C 3 2 Fe(s) +O:(g) 2 Fe,O:(s) ΔΗ - 196,500 cal %3D 1 2 FeO(s) + ; 0:(g) - Fe2O:(s) AH° = -67,900 cal Fe(s) + 2 H* (a = 1) = Fe++ (a = 1) + H2(g) AH° = -21,000 cal %3D %3D 1 H:(g) H* (a = 1) AHº = 0 cal %3D Hig) +0:(g) = H;0(1) AH° = -68,320 cal %3D calculate AH° of the reaction: FeO(s) + 2 H+ (a = 1) = H;0(1) + Fe++ (a = 1) %3D
(a) (c) HO OH 1. BH3 2. H₂O₂, NaOH 3. PCC 4. CH3MgBr 5. H3O+ workup Na₂Cr₂O7 H₂SO4, H₂O
One application of adsorption on surfaces is to measure the ability of acti- vated charcoal to adsorb acid. (Activated charcoal, a form of treated carbon, is very porous and is used to adsorb impurities from water. Its use in aquar- iums typifies this behavior.) In a lab experiment, a student mixes a given amount of powdered charcoal into a series of acetic acid solutions. The acetic acid solutions have different initial concentrations. Some of the acid is ad- sorbed onto the charcoal. By taking aliquots after equilibrium is established, the student determines the change in acid concentration. Plot a Langmuir isotherm for the experimental data and determine the equilibrium constant for the adsorption. The experimental data are as follows: Original concentration (M) 0.7001 Change in concentration (M) 0.3694 0.1515 0.0437 0.0169 0.00665 0.00588 0.00553 0.00283 0.00153
Given the equilibrium constants for the following reactions: 4Cu (s)+O2 (g)》2Cu2O (s), K1=9.76 4 CuO(s)》2Cu2O (s)+ O2 (g), K=0.54. What is the K for the system 2Cu (s)+O2 (g)》2CuO (s) equivalent to?