Graham's Law of Diffusion *EXPLAINED*

What is Graham's Law of Diffusion? This video covers the medical definition and provides a brief overview of this topic.
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➡️ Diffusion
Diffusion is the process by which particles move from an area of high concentration to an area of lower concentration. This movement occurs until a state of equilibrium is reached, where the concentration of particles is the same throughout the space.

➡️ Graham's Law
According to Graham's Law, the rate of diffusion of a gas is inversely proportional to the square root of its molecular weight. In other words, the lighter the gas molecule, the faster it will diffuse or effuse through a membrane. The solubility coefficient of a gas also plays a role in its diffusion rate. This is a measure of how easily a gas dissolves in a liquid. The more soluble a gas is, the slower it will diffuse. This is because the gas molecules are more likely to dissolve in the liquid rather than move through a membrane.

➡️ Formula
Mathematically, Graham's Law can be expressed as follows:

- Rate1 is the rate of diffusion for gas 1.
- Rate2 is the rate of diffusion for gas 2.
- M1 is the molar mass of gas 1
- M2 is the molar mass of gas 2.

This equation shows that the rate of diffusion is inversely proportional to the square root of the molecular weight. So, if two gases have the same solubility coefficient, the lighter gas will diffuse faster than the heavier gas. However, if two gases have the same molecular weight, their diffusion rates will be the same regardless of their solubility coefficients.

➡️ Conditions
It's important to note that Graham's Law is based on ideal conditions, which assume that the gas molecules are non-interacting and that there are no temperature or pressure differences between the two sides of the membrane. In reality, there are many factors that can affect the diffusion rate of a gas, such as temperature, pressure, and the presence of other molecules. Despite its limitations, Graham's Law remains a useful tool for understanding the diffusion of gases. It has applications in many areas of science, such as in the study of atmospheric chemistry, the behavior of gases in the human body, and the diffusion of gases in industrial processes. It's a simple yet powerful concept that helps us understand the behavior of gases in a wide range of contexts.

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🚑MEDICAL DISCLAIMER
This content is for educational and informational purposes only. It is not intended to be a substitute for professional medical advice, diagnosis, or treatment. Please consult with a physician with any questions that you may have regarding a medical condition. Never disregard professional medical advice or delay in seeking it because of something you watch in this video. We strive for 100% accuracy, but errors may occur, and medications, protocols, and treatment methods may change over time.

💡AFFILIATE DISCLAIMER
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⏰TIMESTAMPS
0:00 - Intro
0:28 - Diffusion
1:21 - Graham's Law as Tool

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