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Ch.14 - Chemical Kinetics
All textbooksBrown 14th EditionCh.14 - Chemical KineticsProblem 35c
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Chapter 14, Problem 35c

The following data were measured for the reaction Graph showing reaction data for calculating the rate constant in chemical kinetics.
(c) Calculate the rate constant with proper units?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Rate of Reaction

The rate of reaction refers to the speed at which reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product per unit time. Understanding the rate of reaction is crucial for calculating the rate constant, as it provides the necessary data to determine how quickly a reaction occurs under specific conditions.
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Average Rate of Reaction

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate equation that relates the rate of a reaction to the concentrations of the reactants. It is specific to a particular reaction at a given temperature and is influenced by factors such as temperature and the presence of catalysts. The units of k vary depending on the order of the reaction, making it essential to understand the reaction's stoichiometry to determine the correct units.
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Units of Rate Constant

The units of the rate constant depend on the order of the reaction. For a first-order reaction, the unit is typically s⁻¹, while for a second-order reaction, it is M⁻¹s⁻¹. Understanding how to derive these units from the rate equation is vital for correctly calculating and reporting the rate constant, ensuring that the results are meaningful and applicable in chemical kinetics.
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Related Practice
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 

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

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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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Textbook Question

(a) For the generic reaction A S B what quantity, when graphed versus time, will yield a straight line for a first-order reaction?

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