Ch.7 Chemical Reactions: Energy, Rate and Equilibrium

McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition

McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Non è quello che usi tu?Cambia libro di testo

McMurry 8th Edition

Ch.7 Chemical Reactions: Energy, Rate and Equilibrium

Problema 45

Capitolo 7, Problema 45

What is a catalyst, and what effect does it have on the activation energy of a reaction?

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A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction itself. It participates in the reaction but is regenerated at the end.

The role of a catalyst is to provide an alternative reaction pathway with a lower activation energy compared to the uncatalyzed reaction.

Activation energy is the minimum energy required for reactants to collide and form products. A lower activation energy means that more reactant molecules have sufficient energy to overcome this barrier, leading to a faster reaction rate.

The catalyst achieves this by stabilizing the transition state or forming intermediate species that require less energy to proceed to the products.

It is important to note that while a catalyst speeds up the reaction, it does not alter the equilibrium position or the overall energy change (ΔH) of the reaction.

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Catalyst

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It achieves this by providing an alternative reaction pathway with a lower activation energy, allowing the reaction to proceed more quickly. Catalysts are crucial in various industrial processes and biological systems, where they facilitate reactions that would otherwise occur too slowly.

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Activation Energy

Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to transform into products. By lowering the activation energy, catalysts enable more reactant molecules to have sufficient energy to react, thereby increasing the reaction rate and efficiency.

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Reaction Mechanism

A reaction mechanism is a detailed description of the step-by-step process by which reactants are converted into products in a chemical reaction. It outlines the individual steps, intermediates, and transition states involved. Understanding the reaction mechanism is essential for comprehending how catalysts influence the reaction pathway and the overall energy changes during the reaction.

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Domanda del libro di testo

If a catalyst changes the activation energy of a forward reaction from 28.0 kcal/mol to 23.0 kcal/mol, what effect does it have on the reverse reaction?

2006

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Domanda del libro di testo

The following reaction is used in the industrial synthesis of polyvinyl chloride (PVC) polymer:

Cl₂(g) + H₂C=CH₂(g) → ClCH₂CH₂Cl(l) ∆H = –52 kcal/mol (–218 kJ/mol)

a. Is ∆S positive or negative for this process?

1471

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Domanda del libro di testo

For the reaction C(s, diamond) → C(s, graphite), ∆G = -0.693 kcal/mol (-2.90 kJ/mol) at 25 °C.

a. According to this information, do diamonds spontaneously turn into graphite?

1899