4. The following results were obtained for the decomposition of glucose in aqueous solution. [G]/ 10^-3 M 56.0 55.3 54.2 t/ min Show that the reaction is first order and calculate the rate constant for the process and the half-life for glucose uder these conditions. (Avery, 13) 52.5 49.0 0 45 120 240 480

4. The following results were obtained for the decomposition of glucose in aqueous solution. [G]/ 10^-3 M 56.0 55.3 54.2 t/ min Show that the reaction is first order and calculate the rate constant for the process and the half-life for glucose uder these conditions. (Avery, 13) 52.5 49.0 0 45 120 240 480

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

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) the following data were obtained: HI], M seconds 0.274 0.137 6.85×10-2 3.43x10-2 521 782 912 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.274 M is s and when the starting concentration is 0.137 M is (2) The average rate of disappearance of HI from t= 0s to t= 521 s is| Ms!. (3) The average rate of disappearance of HI from t= 521 s to t= 782 s is| Ms! (4) Based on these data, the rate constant for this | | order reaction is Ms!.
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K.SO2Cl2(g) SO2(g) + Cl2(g) [ SO2Cl2 ], M 3.73×10-3 1.87×10-3 9.35×10-4 4.68×10-4 time, min 0 203 406 609 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is ________ min .(2) Based on these data, the rate constant for this _______(zero, first, or second) order reaction is __________min-1.
Give the individual reaction orders for all substances and the overall reaction order from the following rate law: Rate = k [BrO3–] [Br–] [H+]2 [BrO3–] = [Br–] = [H+]2 = overall =
The decomposition of H202 in aqueous solution is a first-order process. If [H202lo = 0.882 M and k = 3.66 x 10 3 s1, after how many seconds will [H202] = 0.600 M? Report your answer in standard notation to the ones place and do not include (s) units.
Please provide the step by step solution for the question attached. Graphics must be included. Please make sure the graphics are visible.
For the gas phase decomposition of ethyl acetate, CH;COOC,H,–CH,COOH + C2H4 the rate constant has been determined at several temperatures. When In k -1 in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41x10* K and a y-intercept of 28.8. The activation energy for the gas phase decomposition of ethyl acetate is kJ/mol.
In a study of the decomposition of nitrous oxide at 565 °C N2₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x10³ 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t = 0 s to t = 1.50x10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47x103 s is (3) Based on these data, the rate constant for this 9.40×10-2 1.04x104 M-1 S-1. order reaction is M-1 S-1. M-¹ S-1. s and when the starting
A student obtained the following data for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H₂(g) 9.40x10-2 [PH3], M time, s 0 4.70x10-2 29.9 2.35x10-2 1.18x10-2 89.7 59.8 (1) What is the half-life for the reaction starting at t = 0 s? What is the half-life for the reaction starting at t = 29.9 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction?
Use the References to access important values if needed for this question. The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)NO(g) + % Ch(g) is second order in NOCI with a rate constant of 5.90x10-4 M's!. If the initial concentration of NOCI is 0.116 M, the concentration of NOCI will be 1.43x102 M after seconds have passed.