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The Maxwell-Boltzmann equation, which forms the basis of the kinetic theory of gases, defines the distribution of speeds for a gas at a certain temperature. From this distribution function, the most probable speed, the average speed, and the root-mean-square speed can be derived.
- 3.1.3: Mean Free Path
Physical Chemistry for the Life Sciences. New York: Oxford...
- Ideal Gas
The Ideal Gas Equation. Before we look at the Ideal Gas...
- 3.1.3: Mean Free Path
- Molecules in A Gas
- Catalysts and Rate of Reaction
- Effect of Catalysts on The Rate of Reaction
- Catalyst Use in Industry
Understanding the Maxwell-Boltzmann Distribution
If you consider all the molecules in a gas, not all of the particles will have the same amount of kinetic energy. Some will have lots of kinetic energy, whilst some will have less kinetic energy. We can therefore plot a Maxwell-Boltzmann Distributionto show the distribution of energies between different molecules. In terms of its definition, the Maxwell-Boltzmann Distributionrepresents the distribution of molecular energies in gases. It is a plot of the number of particles, where each particl...
Plotting a Maxwell-Boltzmann Distribution
You should be able to draw, label and interpret a Maxwell-Boltzmann distribution plot like the one below. Here are some rules you need to know before you interpret a Maxwell-Boltzmann distribution: 1. Area under curve– the area under the curve is a measure of the total number of particles present. 2. Activation energy– A dotted line or straight line is used to represent the activation energy. 3. Shaded region– the shaded region to the right of the activation energy line represents the only pa...
The Maxwell-Boltzmann Distribution and Temperature Changes
As we saw on the previous chapter, increasing the temperature of a system will increase the kinetic energy of reactant particles so that a larger proportion of the particles have at least in the system will have enough energy to undergo successful collisions. This can be represented on a Mazwell-Boltzmann Distribution curve and you should also be able to draw and interpret Maxwell-Boltzmann Distribution curves for different temperatures: According to this Maxwell-Boltzmann distribution: 1. Wh...
Mechanism of Catalysts
A catalyst is a substance that increases the rate of a chemical reaction without being changed in chemical composition or amount. The catalyst works by providing an alternative routeto a reaction which has a lower activation energy, which means that a smaller amount of energy is needed to start a reaction. The way catalysts achieve this depends on whether they are heterogeneous or homogeneous catalysts.
Heterogeneous Catalysts
A heterogeneous catalystis in a different physical state (or phase) from the reactants. They provide a surface for the reaction to take place on, which facilitates reactant molecules to react with each other at a lower activation energy. The process by which heterogeneous catalyst work involves three steps: 1. Adsorption – Reactant molecules arrive at the surface of the solid heterogeneous catalyst and form weak bonds with it by a process known as adsorption. 2. Reaction – Intermolecular bond...
Homogeneous Catalysts
A homogeneous catalystis in the same physical state (or phase) as the reactants. Homogeneous catalysts work by forming intermediate specieswith the reactant particles, which then react to form the products and reform the catalyst. The activation energies of this stepwise reaction are overall lower than the activation energy for the uncatalysed reaction.
Re-Use of Catalysts
If a catalyst is present at the start of a reaction, it will also be present at the end of the reaction. This means that catalysts can be re-usedin several reactions. You should be able to explain the qualitative effect of using a catalyst on the rate of reaction using a Maxwell Boltzmann distribution: According to this Maxwell-Boltzmann distribution: 1. Only the particles that are represented by the area to the right of the activation energy will react when they collide. 2. When the catalyst...
The Haber Process mentioned previously is an example of how catalysts can be used in industry. Catalysts are very widely used in industrial processes for their multiple economic benefits: 1. Catalyst use lowers production costs.By allowing for the reaction to take place at a lower temperature and pressures, which decreases energy demands; as well a...
Dec 15, 2018 · The Maxwell-Boltzmann equation, which forms the basis of the kinetic theory of gases, defines the distribution of speeds for a gas at a certain temperature. From this distribution function, the most probable speed, the average speed, and the root-mean-square speed can be derived.
Revision notes on 1.7.3 Maxwell–Boltzmann Distributions for the AQA A Level Chemistry syllabus, written by the Chemistry experts at Save My Exams.
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Jan 30, 2021 · A Maxwell–Boltzmann distribution shows the distribution of particle energies at a given temperature and allows for a qualitative estimation of the fraction of particles with...
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Aug 30, 2024 · The Maxwell-Boltzmann distribution is a description of the statistical distribution of the energies of the molecules of a classical gas. This distribution was first set forth by Scottish physicist James Clerk Maxwell, on the basis of probabilistic arguments, and was generalized by Austrian physicist Ludwig Boltzmann.
