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Ch.14 - Chemical Kinetics
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.14 - Chemical KineticsProblema 117
Capitolo 14, Problema 117

Why doesn't a catalyst appear in the overall chemical equation for a reaction?

Guida verificata passo dopo passo
1
Understand that a catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process.
Recognize that a catalyst works by providing an alternative reaction pathway with a lower activation energy.
Note that during the reaction, the catalyst participates in the formation of an intermediate, but it is regenerated by the end of the reaction.
Realize that because the catalyst is not consumed, it does not appear in the overall balanced chemical equation, which only shows the reactants and products.
Remember that the role of a catalyst is to facilitate the reaction, not to be a part of the final product, hence it is not included in the net chemical equation.

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Catalysts

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It works by providing an alternative reaction pathway with a lower activation energy, allowing reactants to convert to products more efficiently. Since catalysts are not consumed, they can participate in multiple reaction cycles.
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01:59
Catalyzed vs. Uncatalyzed Reactions

Chemical Equations

A chemical equation represents the reactants and products of a reaction, showing their relative amounts and the direction of the reaction. In these equations, only the substances that undergo a permanent change are included. Since catalysts do not undergo a permanent change, they are not included in the overall equation.
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01:32
Balancing Chemical Equations

Reaction Mechanism

The reaction mechanism describes the step-by-step sequence of elementary reactions that lead to the overall chemical transformation. Catalysts often participate in these elementary steps, facilitating the reaction without appearing in the final balanced equation. Understanding the mechanism helps clarify how catalysts influence reaction rates without altering the overall stoichiometry.
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03:06
Reaction Mechanism Overview
Pratica correlata
Domanda del libro di testo

A proposed mechanism for the oxidation of nitric oxide to nitrogen dioxide was described in Problem 14.29. Another possible mechanism for this reaction is

(c) Relate the rate constant k to the rate constants for the elementary reactions.

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Domanda del libro di testo

A proposed mechanism for the oxidation of nitric oxide to nitrogen dioxide was described in Problem 14.29. Another possible mechanism for this reaction is

(b) Show that this mechanism is consistent with the experimental rate law, Rate = k[NO4][O2].

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Domanda del libro di testo
Comment on the following statement: 'A catalyst increases the rate of a reaction, but it is not consumed because it does not participate in the reaction.'
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Domanda del libro di testo
Consider the following mechanism for the decomposition of nitramide 1NH2NO22 in aqueous solution: NH2NO21aq2 + OH-1aq2S NHNO2 -1aq2 + H2O1l2 NHNO2 -1aq2S N2O1g2 + OH-1aq2 (c) How will the rate of the overall reaction be affected if HCl is added to the solution?
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