E17F.5(b) The enzyme-catalysed conversion of a substrate at 298 K has K 0.032mol dm and 425x10 mol dm when the enzyme concentration is 3.60 x 10 mol dm. Calculate the catalytic efficiency of the enzyme, as defined in Exercise E17F.5(a) wwwwam ES ES vk,[ES ES'E+P vkES] Show that the rate of formation of product has the same form as that shown in eqn 17F.16, but with and K given by k (k+k) sk(kk) kkE К, ktk www

E17F.5(b) The enzyme-catalysed conversion of a substrate at 298 K has K 0.032mol dm and 425x10 mol dm when the enzyme concentration is 3.60 x 10 mol dm. Calculate the catalytic efficiency of the enzyme, as defined in Exercise E17F.5(a) wwwwam ES ES vk,[ES ES'E+P vkES] Show that the rate of formation of product has the same form as that shown in eqn 17F.16, but with and K given by k (k+k) sk(kk) kkE К, ktk www

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...

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3a
In a study of the decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)N20(g) + H20(1) the concentration of NH2NO2 was followed as a function of time. It was found that a graph of In[NH,NO2] versus time in seconds gave a straight line with a slope of -6.72x105 s and a y-intercept of -0.911 . Based on this plot, the reaction is | reaction is |order in NH2NO2 and the half life for the seconds.
1. The following data was obtained from decomposition of nitrogen oxide (NO). 2HX H2 + X2 T(K) 703 733 759 791 811 836 865 k (L mol-¹s-¹) Find; 0.011 0.035 0.105 0.343 0.790 2.14 4.95 (a) The activation energy, Ea. (b) The Arrhenius constant, A (c) The collision frequency, ZAA (d) The following mechanism was suggested for the reaction. Is the mechanism meet with the order of reaction? X₂ = X + X X + H2 H + XH + HX2 X + H₂ Fast Slow Fast
Show that if it can be assumed that there is a pre-equilibrium involving step (1), the rate of formation of ethylene oxide is v = k,K[CH,CICH,OH][OH ], where K is the equilibrium constant for the first step and k, is the rate constant for the second step. E17E.2(b) 'The mechanism for the reaction between 2-chloroethanol, CH,CICH,OH, and hydroxide ions in aqueous solution to form ethylene oxide, (CH,CH,)0, is thought to consist of the steps (1) CH,CICH,OH+OH 2CH,CICH,O¯+H,O (2) CH,CICH,O¯ –→(CH,CH,)O+CI
In a chemical reaction with activation energy E. = 20 kJ/mol, (a) how many folds the rate constant is increased when the temperature increases from 300 K to 1000 K? That is, the ratio of k(1000K)/k(300K). (b) In the presence of a catalyst, the activation energy is brought down to 10 kJ/mol, how many folds the rate constant is increased at the same temperature 300K?