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Jun 23
Graham's law of diffusion states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. In other words, lighter gases will diffuse faster than heavier gases at the same temperature and pressure. This law is important in understanding the behavior of gases and is often used in various scientific and industrial applications.
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Google Gemini AI
Jun 23
Graham's Law of Diffusion
Graham's Law of Diffusion, proposed by Thomas Graham in 1832, describes the relationship between the rates of diffusion of different gases under identical conditions. It states that:
>The rate of diffusion of a gas is inversely proportional to the square root of its molecular weight.
Mathematically, it can be expressed as:
```
Rate of diffusion ∝ 1/√(Molecular weight)
```
Explanation:
The rate of diffusion of a gas depends on the following factors:
- Molecular size: Smaller molecules can move through a medium more easily than larger molecules.
- Molecular mass: Heavier molecules have greater inertia and are slower to move.
- Temperature: As temperature increases, the average kinetic energy of the molecules increases, resulting in faster diffusion.
- Pressure: Pressure has a relatively small effect on diffusion rates.
According to Graham's law, the rate of diffusion is related to the molecular weight of the gas. The molecular weight of a gas is the sum of the atomic masses of all the atoms in its molecules. Gases with lower molecular weights have smaller molecules and diffuse faster than gases with higher molecular weights.
This law helps us understand the relative rates of diffusion of gases in different situations and has applications in various fields, including:
- Gas chromatography: Separating and identifying gases based on their different diffusion rates.
- Diffusion membrane technology: Designing membranes that selectively allow passage of gases based on their molecular weights.
- Anesthesia: Controlling the rate of diffusion of anesthetic gases into the bloodstream.
- Environmental monitoring: Detecting and monitoring the diffusion of pollutants and trace gases.
Graham's Law of Diffusion, proposed by Thomas Graham in 1832, describes the relationship between the rates of diffusion of different gases under identical conditions. It states that:
>The rate of diffusion of a gas is inversely proportional to the square root of its molecular weight.
Mathematically, it can be expressed as:
```
Rate of diffusion ∝ 1/√(Molecular weight)
```
Explanation:
The rate of diffusion of a gas depends on the following factors:
- Molecular size: Smaller molecules can move through a medium more easily than larger molecules.
- Molecular mass: Heavier molecules have greater inertia and are slower to move.
- Temperature: As temperature increases, the average kinetic energy of the molecules increases, resulting in faster diffusion.
- Pressure: Pressure has a relatively small effect on diffusion rates.
According to Graham's law, the rate of diffusion is related to the molecular weight of the gas. The molecular weight of a gas is the sum of the atomic masses of all the atoms in its molecules. Gases with lower molecular weights have smaller molecules and diffuse faster than gases with higher molecular weights.
This law helps us understand the relative rates of diffusion of gases in different situations and has applications in various fields, including:
- Gas chromatography: Separating and identifying gases based on their different diffusion rates.
- Diffusion membrane technology: Designing membranes that selectively allow passage of gases based on their molecular weights.
- Anesthesia: Controlling the rate of diffusion of anesthetic gases into the bloodstream.
- Environmental monitoring: Detecting and monitoring the diffusion of pollutants and trace gases.
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