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15. Chemical Kinetics
Rate Law

15. Chemical Kinetics

Rate Law

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Textbook Question
The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (c) How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution?
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Textbook Question
Consider the reaction of peroxydisulfate ion 1S2O82-2 with iodide ion 1I - 2 in aqueous solution: S2O8 2 - 1aq2 + 3 I - 1aq2¡2 SO42 - 1aq2 + I3- 1aq2 At a particular temperature, the initial rate of disappearance of S2O82 - varies with reactant concentrations in the following manner: Experiment 3S2o8 24 1M 2 3I4 1M 2 Initial Rate 1M,s2 1 0.018 0.036 2.6 * 10-6 2 0.027 0.036 3.9 * 10-6 3 0.036 0.054 7.8 * 10-6 4 0.050 0.072 1.4 * 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant.
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Textbook Question
Initial rate data at 25 °C are listed in the table for the reaction NH4 +1aq2 + NO2 -1aq2S N21g2 + 2 H2O1l2 (b) What is the value of the rate constant?

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(b) What would be the initial rate in an experiment with initial concentrations 31CH323 N4 = 4.2 * 10-2 M and 3ClO24 = 3.4 * 10-2 M?
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Textbook Question
Consider the following reaction between mercury(II) chloride and oxalate ion: 2 HgCl21aq2 + C2O4 2 - 1aq2¡2 Cl - 1aq2 + 2 CO21g2 + Hg2Cl21s2 The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O4 2 -, and the following rate data were obtained for the rate of disappearance of C2O4 2 - : Experiment 3HgCl2 4 1M 2 3C2o4 24 1M 2 Rate 1M,s2 1 0.164 0.15 3.2 * 10-5 2 0.164 0.45 2.9 * 10-4 3 0.082 0.45 1.4 * 10-4 4 0.246 0.15 4.8 * 10-5 (c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of C2O4 2- is 0.25 M if the temperature is the same as that used to obtain the data shown?
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(c) What is the rate law?

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(a) Write a balanced equation for the reaction.
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(b) Determine the rate law, and calculate the value of the rate constant.

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Textbook Question
Consider the reversible, first-order interconversion of two molecules A and B: A kfkrB where kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (b) Draw a qualitative graph that shows how the rates of the forward and reverse reactions vary with time.

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Textbook Question
Consider the reversible, first-order interconversion of two molecules A and B: A kfkrB where kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (c) What are the relative concentrations of B and A when the rates of the forward and reverse reactions become equal?

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Textbook Question
Consider the reversible, first-order interconversion of two molecules A and B: A kfkrBwhere kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (a) What are the rate laws for the forward and reverse reactions?

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What is the rate law for the reaction? What is the numerical value of the rate constant k, including the correct units?
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