Chapter 14, Problem 38a
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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The following data were measured for the reaction
(b) What is the overall order of the reaction?
The following data were measured for the reaction
(c) Calculate the rate constant with proper units?
Consider the gas-phase reaction between nitric oxide and bromine at 273 C: 2 NO1g2 + Br21g2¡2 NOBr1g2. The following data for the initial rate of appearance of NOBr were obtained: Experiment 3no4 1M 2 3br2 4 1M 2 Initial Rate 1M,s2 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 (b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.
(a) For the generic reaction A S B what quantity, when graphed versus time, will yield a straight line for a first-order reaction?
(a) The gas-phase decomposition of SO2Cl2, SO2Cl21g2 ¡SO21g2 + Cl21g2, is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 * 105 s. What is the rate constant at this temperature?
As described in Exercise 14.41, the decomposition of sulfuryl chloride 1SO2Cl22 is a first-order process. The rate constant for the decomposition at 660 K is 4.5 * 10-2 s-1. (b) At what time will the partial pressure of SO2Cl2 decline to one-tenth its initial value?