INTERACTIVE EXAMPLE Determining the Rate Law from Initial Rates Chlorine dioxide, CIO,, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO, and CIO," lons. 2 clo;(aq) + 2 OH (aq) - CIO, (aq) + CIO2 (aq) + H20(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of CIO, was determined. Use the data here to determine the order of the reaction for CIO, and OH", and the value of the rate constant. [C10,linit [OH"linit Initial Rate, mol/(Les) Exp. 1 0.030 0.030 0.0062 Exp. 2 0.060 0.030 0.0248 Exp. 3 0.030 0.060 0.0124 Order for CIO2: Order for OH: Rate constant = Submit Show Tutor Steps

INTERACTIVE EXAMPLE Determining the Rate Law from Initial Rates Chlorine dioxide, CIO,, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO, and CIO," lons. 2 clo;(aq) + 2 OH (aq) - CIO, (aq) + CIO2 (aq) + H20(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of CIO, was determined. Use the data here to determine the order of the reaction for CIO, and OH", and the value of the rate constant. [C10,linit [OH"linit Initial Rate, mol/(Les) Exp. 1 0.030 0.030 0.0062 Exp. 2 0.060 0.030 0.0248 Exp. 3 0.030 0.060 0.0124 Order for CIO2: Order for OH: Rate constant = Submit Show Tutor Steps

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 5P

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A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
When nitrogen dioxide reacts with carbon monoxide, the following reaction occurs. Â NO2(g)+CO(g)NO(g)+CO2(g)The following data are obtained at a certain temperature: (a) What is the order of the reaction with respect to NO2, CO, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) When [ NO2 ]=0.421Mand [ CO ]=0.816M, what is the rate of the reaction at the temperature of the experiments?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 4.00 105 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 102 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 102 M C2H5OH to decompose?
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