Initial rates of an enzyme -catalysed reaction at different substrate concentrations are listed in Table 2.1s, mol/L0.00410.000950.000520.0001030.000049v, mol/(L. min) x 10°177173125106800.00001060.0000051a) Evaluate K and vmax by a Lineweaver-Burk plotb) Using the Eadie-Hofstee plot, evaluate K and Vmaxc) Using theHanes-Woolf plot, evaluate K and Vmaxd) Comment on the accuracy of the three methods6743E

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Answered: Initial rates of an enzyme -catalysed…

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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For the gas phase decomposition of dimethyl ether at 500 °C CH3OCH3 CH4+H, + CO the following data have been obtained: [CH-ОCH;], M 0.141 9.27×10-2 6.10×10-2 4.01×10-2 time, min 17.5 34.9 52.4 The average rate of disappearance of CH3OCH3 over the time period from t= 34.9 min to t= 52.4 min is M min!.
The rate law for the decomposition of A→P is investigated by measuring the initial rate of the reaction for several concentrations of A. The data are shown below. Assuming that the rate law is of the form v=k[A]n, use a graphical method to determine the value of n. [A]/M Initial Rate/(Torr s-1) [A]/M Initial Rate/(Torr s-1) 1.000 0.1422 0.700 0.0718 0.950 0.1248 0.650 0.0625 0.900 0.1123 0.600 0.0518 0.850 0.0983 0.550 0.0445 0.800 0.0857 0.500 0.0382 0.750 0.0782
7Devived an cnfe guated expression for a Second - order rate lau V= K {A3 (B] for a reacton 2A + 3B -> P. of Stocchcomefry |8]At a given temperature. the half-life period for the decomposi trou of anamonta in contact with tingsten was as follow: Pcommts Relahice Half-lefe 50 100 200 3.52 1.82 0.93
Chemistry The hydrolysis of a substance is catalyzed by hydrogen ions and the velocity constant is equal to: k / dm3 mol-1 s-1 = 4.7 x 10-2 ([H +] / mol dm-3). When the substance is dissolved in a 10-3 M HA acid solution the velocity constant becomes 3.2 x 10-5 dm3 mol-1 s-1. Calculate the dimension constant of the HA acid.
For the gas phase decomposition of sulfuryl chloride at 600 K SO,C12→SO2 + Cl2 the following data have been obtained: [SO2C12], M 3.00x10-3 2.00x10-3 1.33x10-3 8.87x104 time, min 145 290 435 The average rate of disappearance of SO,Cl2 over the time period from t = 0 min to t= 145 min is M min-1
Expt. 1 2 3 NH; (aq) + NO; (aq) >Nz (aq) + 2 H2O (l) [NO₂] Rate (at 298 K) 0.020 M/s 0.020 M 0.020 M 0.030 M/s 0.010 M 0.0050 M/s [NH+] 0.010 M 0.015 M 0.010 M Determine the complete rate law (rate law and rate constant) for the reaction. Show all work. What is the initial rate of this reaction if the concentrations in Expt. 2 above are tripled. Show work. What is the rate of H₂O formation in Expt. 1? A 4th trial is conducted at 273 K, using the concentrations from Expt. 1. If the rate was found to be 0.016 M/s, calculate the activation energy of this reaction.
An orange juice is thermally processed for determining ascorbic acid degradation kinetics. After different temperature experiments, the following ascorbic acid concentration values were obtained: Ascorbic Acid (mg/L) Processing Time (second) 0 15 30 60 90 120 Temperature (oC) 75 558.3 546.5 535 526.5 519.6 508.6 85 608.6 595.2 587.4 572.7 557.5 542.3 95 612.6 601.5 588.2 546.1 521.8 509.5 According to the results; Determine ascorbic acid degradation order Derive the equations related to the degradation order (general equation and t1/2) Calculate k-values at the constant processing temperatures Calculate activation energy (Ea) of the degradation reaction Calculate half-life time of ascorbic acid for all processing (For better evaluation, add figures for the addressed questions, if necessary)
Please help me determine the integrated rate law and justify the answer
P17A.3 The following kinetic data (v, is the initial rate) were obtained for the reaction 2ICI(g) + H,(g) → L(g) + 2 HCI(g): Experiment [ICI],(mmol dm³) [H,]/(mmol dm³) v(moldm³s") 1 1.5 1.5 3.7 x 107 2 7.4 x 107 3.0 1.5 3 3.0 4.5 22 x 107 4 4.7 2.7 ? (a) Write the rate law for the reaction. (b) From the data, determine the value of the rate constant. (c) Use the data to predict the reaction rate for experiment 4.
Ethyl chloride vapor decomposes by the first-order reactionC2H5Cl→C2H4+HClC2H5Cl→C2H4+HClThe activation energy is 249 kJmol−1kJmol−1 and the frequency factor is 1.6×1014s−11.6×1014s−1. ind the value of the specific rate constant at 720 KK . Express your answer using two significant figures. Find the fraction of the ethyl chloride that decomposes in 16 minutes at this temperature. Express your answer using one significant figure. Find the temperature at which the rate of the reaction would be twice as fast. Express your answer using two significant figures.
(2) The reaction-rate data given below were obtained using a batch reaction system for the reaction A→products. Plot the data in appropriate form to test the fit for zero- and first-order kinetics. From the plot that gives the best fit, determine the appropriate reaction rate constant (remember the units). Time, min CA, (g/m3) 0 30 0.5 25.4 1 21.6 2 16.9 4 13.1 8 8.3 16 3.2 32 0.31
X2Y2 + 2Z + 2Y→ Z2 + 2Y2X Trial [X2Y2 ], (M) [Z], (M) [У, (М) Initial Rate (M/min) 1 0.25 0.11 0.33 0.025 0.11 0.33 0.2 3 0.25 0.66 0.33 0.15 4 0.25 0.11 0.66 0.025 A) What is the rate law? B) What is the rate constant? C) What is the initial rate if you have 0.061 M of X, 0.092 M of Y, and 0.043 M of Z?

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