Maxwell - Boltzman distribution

In summary, the conversation discussed the creation of a spreadsheet to plot the 3d speed distribution from the Maxwell-Boltzmann probability function. The resulting graph matched published graphs, but when the area was calculated by integrating over interval widths and probability, the result was around 5 or 6 instead of the expected 1. After trying smaller intervals and consulting an article on the M-B distribution, it was determined that the area under the curve had not been properly normalized. This issue was resolved and the final area was found to be 0.98 through numerical integration.
  • #1
mattT1227
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I made a spreadsheet to plot the 3d speed distribution from the MB probability function. It matches the peak and fall-off of published graphs. I then tried to integrate it by summing over interval widths times probability. I thought the area should be 1. My result is around 5 or 6. I've tried really small intervals, around 0.25 m/s, that didn't help. Must be I don't understand what the area under the probability curve represents.
 
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  • #4
Thanks all. Problem solved. Area under curve is 0.98 by numerical integration, close enough.
 
  • #5


The Maxwell-Boltzmann distribution is a probability distribution that describes the speed distribution of particles in a gas at a given temperature. It is a fundamental concept in statistical mechanics and has various applications in physics and chemistry.

Your approach of using a spreadsheet to plot the 3D speed distribution from the MB probability function is a valid method to visualize the distribution. It is also commendable that your results match the peak and fall-off of published graphs, which indicates that your calculations are accurate.

However, your difficulty in integrating the probability function and obtaining a result of around 5 or 6 instead of 1 is understandable. The area under the probability curve represents the total probability of finding a particle within a certain speed range. In other words, it represents the total likelihood of a particle having a speed within that range. Therefore, the area under the curve should always be equal to 1, as the total probability of finding a particle within the entire speed range is 100%.

Based on your description, it seems that your approach of summing over interval widths times probability may not be accurate. I would suggest consulting with a statistician or a colleague who has expertise in probability distributions to ensure that your calculations are correct.

In conclusion, the Maxwell-Boltzmann distribution is a crucial concept in statistical mechanics, and it is essential to have a thorough understanding of its properties and applications. Keep in mind that the area under the probability curve represents the total probability, and it should always be equal to 1. I wish you all the best in your future experiments and calculations.
 

FAQ: Maxwell - Boltzman distribution

What is the Maxwell-Boltzmann distribution?

The Maxwell-Boltzmann distribution is a probability distribution that describes the distribution of speeds of particles in a gas or liquid at a given temperature. It was developed by James Clerk Maxwell and Ludwig Boltzmann in the late 19th century.

What factors affect the shape of the Maxwell-Boltzmann distribution?

The shape of the Maxwell-Boltzmann distribution is affected by the temperature of the system, the mass of the particles, and the speed of the particles. An increase in temperature or a decrease in particle mass results in a wider distribution, while an increase in particle speed narrows the distribution.

How does the Maxwell-Boltzmann distribution relate to the kinetic theory of gases?

The Maxwell-Boltzmann distribution is a direct result of the kinetic theory of gases, which states that gas particles move randomly and collide with each other and the walls of the container. The distribution describes the range of speeds that the particles will have at a given temperature.

What is the significance of the Maxwell-Boltzmann distribution in chemistry?

The Maxwell-Boltzmann distribution is important in chemistry because it helps us understand the behavior of gas molecules, such as their average speed and the likelihood of certain collisions. It is also used to calculate reaction rates and understand the relationship between temperature and the amount of energy transferred during collisions.

Can the Maxwell-Boltzmann distribution be applied to systems other than gases?

While the Maxwell-Boltzmann distribution was originally developed for gases, it can also be applied to other systems, such as liquids or plasmas. However, it is important to note that the distribution may need to be modified to account for different factors, such as intermolecular forces or particle interactions, in these systems.

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