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The same sample of gas at different temperatures shows that at low
temperatures, most molecules have speeds close to their average
speed.
What does the Maxwell-Boltzmann distribution graph show?
Put simply, a Maxwell-Boltzmann distribution graph shows how the energy of gas particles varies within a system.
This is solely a measurement of the speeds of particles because kinetic energy is directly related to speed.
The Maxwell-Boltzmann distribution in chemistry is the subject of this article.
We will begin by describing how to read a graph of the Maxwell-Boltzmann distribution. This will involve taking a closer look at things like the typical energy and the most likely energy.
The graph will then be changed under various circumstances, such as when a catalyst is added or the temperature is raised.
The Maxwell-Boltzmann distribution, which we previously mentioned, is a probability function that depicts the distribution of energy among the particles of an ideal gas. (For more information on this topic, see Chemical Kinetics.)
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A plot of the maxwell distribution of speeds for the same sample of gas at different temperatures shows that at low temperatures, most molecules have speeds close to their average speed.
What is the maxwell distribution of speed?
The distribution of energy between identical but distinct particles is the subject of the Maxwell-Boltzmann distribution.
The distribution of speeds for gas at a specific temperature is specified by the Maxwell-Boltzmann equation, which is the foundation of the kinetic theory of gases.
The speed that is most likely to occur, the speed that is average, and the root-mean-square speed can all be calculated using this distribution function.
The number of molecules moving at a given speed is represented by the Maxwell-Boltzmann graph's y-axis.
Therefore, if the graph is higher in a certain area, it indicates that there are more gas molecules traveling at such speeds in that area.
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