2 The reaction A+B+C ABC is zero order with respect to one reactant, first order with respect to another reactant and second order with respect to another reactant. ai Explain what is meant by the term order of reaction with respect to a given reactant. i Use the data in the table below to deduce the order with respect to each of the reactants, A, B and C. Experiment (A)/moldm (B]/moldm (C]/moldm³ Rate/mol dm³5- 0.100 1.00 100 0.00783 2 0.200 1.00 1.00 0.00802 0.300 1.00 1.00 0.00796 4 1.00 0.100 1.00 0.00008 1.00 0.200 1.00 0.00031 1.00 0.300 1.00 0.00073 7. 1.00 1.00 0.100 0.00078 1.00 1.00 0.200 0.00158 1.00 1.00 0.300 0.00236 bi Write the rate equation for this reaction. i State the overall order of the reaction. i Calculate the value of the rate constant using experiment 6. Include the units in your answer. c Suggest a possible mechanism consistent with the rate equation y chemical equation you have proposed and the

2 The reaction A+B+C ABC is zero order with respect to one reactant, first order with respect to another reactant and second order with respect to another reactant. ai Explain what is meant by the term order of reaction with respect to a given reactant. i Use the data in the table below to deduce the order with respect to each of the reactants, A, B and C. Experiment (A)/moldm (B]/moldm (C]/moldm³ Rate/mol dm³5- 0.100 1.00 100 0.00783 2 0.200 1.00 1.00 0.00802 0.300 1.00 1.00 0.00796 4 1.00 0.100 1.00 0.00008 1.00 0.200 1.00 0.00031 1.00 0.300 1.00 0.00073 7. 1.00 1.00 0.100 0.00078 1.00 1.00 0.200 0.00158 1.00 1.00 0.300 0.00236 bi Write the rate equation for this reaction. i State the overall order of the reaction. i Calculate the value of the rate constant using experiment 6. Include the units in your answer. c Suggest a possible mechanism consistent with the rate equation y chemical equation you have proposed and the

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 41E: The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was...

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The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
You and a coworker have developed a molecule thathas shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law Rate=k[AV]1[V]1 You have been given the following data from your coworker: [V]0=0.20M[AV]0=1.0104M A plot of ln[AV] versus t(s) gives a straight line with a slope of 0.32 s1. What is the value of the rate constant (k) for this reaction?
The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
Use the data provided to graphically determine the order and rate constant of the following reaction: SO2CI2SO2+CI2 Time(s) 0 5.00103 1.00104 1.50104 [SO2CI2] (M) 0.100 0.0896 0.0802 0.0719 Time(s) 2.50104 3.00104 4.00104 [SO2CI2] (M) 0.0577 0.0517 0.0415
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)
The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCI3, is 6.2104 min-1. 2N2O54NO2+O2 What is the rate of the reaction when [N2O5] = 0.40 M?
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?