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Ch.14 - Chemical Kinetics
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All textbooksBrown 15th EditionCh.14 - Chemical KineticsProblem 35b

Chapter 14, Problem 35b

The following data were measured for the reaction 

(b) What is the overall order of the reaction?

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everyone. See we have the following reaction below. We have the following data table. You are asked to determine the overall order of the reaction. We know that the rate law equation is the right equal to the rate constant construction of a the power of X. And X. Is the order with respect to a construction of beat the power of why and why is the order with respect to be the first, determine the order with respect to W. X. Y. Z. To find the right order for W. X. We're gonna use our 2nd and 3rd experiment. So 0.007224 mother per second. You go to the right constant Time. smaller. The path adds 0. smaller the power of Why. You have 0.014449/s. You go to the rate constant from 0.056, smaller the power of X. From 0.089 smaller the power of Y. Now these are gonna cancel out and okay cancel out as well. 11 0.5. It goes 0.5 to the power of eggs. It was one and W. X. Is first order and to find the right order for Y. Z. We're gonna use our 1st and 5th experiment. You have 0.008027 per second to the right constant. From 0.078, smaller the power eggs 0. moller the power of Why. 0.016055. smaller per second. Because of the rate constant. From 0.78 smaller. The power of X. Times 0.71 smaller. To the part of why? You know these cancel out. Okay, cancel out as well. 0.5 Because 0.5 to the power of one. So why it was one the Y. Z. Is also first order. And now for the overall order we're gonna have the sum of the individual rates. It's gonna be one plus one plus. Give us two. It's gonna be second order. Thanks for watching my video and I hope it was up for
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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(a) Write the rate law for this reaction.

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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(b) Calculate the rate constant with proper units.

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Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4 (c) Calculate the rate when [OCl-] = 2.0 * 10-3 M and [I-] = 5.0 * 10 - 4 M.

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Textbook Question

The following data were measured for the reaction 

(c) Calculate the rate constant with proper units?

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Textbook Question

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.

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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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