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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.14 - Chemical KineticsProblema 70c
Capitolo 14, Problema 70c

Consider the following energy profile.
(c) Which step is rate limiting?

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Identify the highest energy transition state on the energy profile diagram.
Compare the energy of this transition state to the energies of other transition states in the reaction mechanism.
The step with the highest energy transition state is typically the slowest step in the reaction mechanism.
The slowest step in the reaction mechanism is considered the rate-limiting step because it determines the overall rate of the reaction.
Conclude that the step with the highest energy transition state is the rate-limiting step.

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Energy Profile Diagram

An energy profile diagram visually represents the energy changes during a chemical reaction. It typically shows the energy of reactants, products, and the transition states, illustrating the activation energy required for the reaction to proceed. Understanding this diagram is crucial for identifying the rate-limiting step, which is the slowest step in the reaction mechanism.
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Energy Diagrams

Activation Energy

Activation energy is the minimum energy required for reactants to undergo a chemical reaction. It is represented as the energy barrier that must be overcome for the transition state to form. The step with the highest activation energy in a reaction mechanism is often the rate-limiting step, as it dictates the overall speed of the reaction.
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Activity Series Chart

Rate-Limiting Step

The rate-limiting step is the slowest step in a reaction mechanism that determines the overall rate of the reaction. It acts as a bottleneck, meaning that even if other steps are faster, the rate of the entire process cannot exceed the rate of this step. Identifying the rate-limiting step is essential for understanding reaction kinetics and optimizing reaction conditions.
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Limiting Reagent Example
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Domanda del libro di testo

(c) Which step is the fastest?

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Domanda del libro di testo

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:

H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)

IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)

(a) Write the chemical equation for the overall process.

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Domanda del libro di testo

Consider the following energy profile.

(b) How many intermediates are formed in the reaction?

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Domanda del libro di testo

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:

H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)

IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)

(c) Assuming that the first step of the mechanism is rate determining, predict the rate law for the overall process.

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Domanda del libro di testo

Consider the following energy profile.

(a) How many elementary reactions are in the reaction mechanism?

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Domanda del libro di testo

The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:

H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)

IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)

(b) Identify the intermediate, if any, in the mechanism.

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