Textbook Question
The addition of NO accelerates the decomposition of N2O, possibly by the following mechanism: NO1g2 + N2O1g2¡N21g2 + NO21g2 2 NO21g2¡2 NO1g2 + O21g2 (b) Is NO serving as a catalyst or an intermediate in this reaction?
Ch.14 - Chemical Kinetics
Chapter 14, Problem 81b
Many metallic catalysts, particularly the precious-metal ones, are often deposited as very thin films on a substance of high surface area per unit mass, such as alumina (Al2O3) or silica (SiO2). (b) How does the surface area affect the rate of reaction?
Verified step by step guidance1
Step 1: Understand the role of catalysts. Catalysts are substances that increase the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy. They do this by offering a surface where the reactants can come together to react.
Step 2: Recognize the importance of surface area. The greater the surface area of the catalyst, the more space there is for reactants to come into contact with the catalyst. This increases the number of successful collisions between reactant particles and the catalyst, which in turn increases the rate of reaction.
Step 3: Apply this understanding to the given problem. In the case of metallic catalysts deposited as thin films on substances like alumina or silica, the high surface area of these substances allows for more catalyst to be exposed to the reactants. This increases the number of successful collisions and thus the rate of reaction.
Step 4: Understand the practical implications. This is why catalysts are often deposited as thin films on high surface area substances - it allows for the most efficient use of often expensive catalyst materials, while maximizing the rate of reaction.
Step 5: Remember that while catalysts increase the rate of reaction, they do not affect the position of the equilibrium or the enthalpy change of the reaction. They simply allow the reaction to reach equilibrium more quickly.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Surface Area to Volume Ratio
The surface area to volume ratio is a critical factor in chemical reactions, particularly for catalysts. A higher surface area allows more reactant molecules to interact with the catalyst at any given time, increasing the likelihood of collisions and, consequently, the rate of reaction. This principle is especially important in heterogeneous catalysis, where the catalyst is in a different phase than the reactants.
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Perimeter, Area, Volume
Catalysis
Catalysis refers to the process of increasing the rate of a chemical reaction by adding a substance known as a catalyst. Catalysts work by providing an alternative reaction pathway with a lower activation energy, allowing more reactant molecules to convert into products more quickly. In the context of metallic catalysts, their effectiveness is often enhanced by their high surface area, which facilitates more active sites for reactions.
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Reaction Rate
The reaction rate is a measure of how quickly reactants are converted into products in a chemical reaction. It can be influenced by several factors, including concentration, temperature, and the presence of a catalyst. In the case of catalysts with high surface areas, the increased availability of active sites leads to a higher frequency of effective collisions, thereby accelerating the overall reaction rate.
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Related Practice
Textbook Question
The enzyme urease catalyzes the reaction of urea, (NH2CONH2), with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 × 10-5 s-1 at 100°C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 × 104 s-1 at 21°C. (b) If the rate of the catalyzed reaction were the same at 100°C as it is at 21°C, what would be the difference in the activation energy between the catalyzed and uncatalyzed reactions?