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- https://chem.libretexts.org/Courses/City_College_of_San_Francisco/Chemistry_101A/Topic_C%3A_Gas_Laws_and_Kinetic_Molecular_Theory/05%3A_Gases/5.11%3A_Molecular_Effusion_and_DiffusionDiffusion is the gradual mixing of gases to form a sample of uniform composition even in the absence of mechanical agitation. In contrast, effusion is the escape of a gas from a container through a ti...Diffusion is the gradual mixing of gases to form a sample of uniform composition even in the absence of mechanical agitation. In contrast, effusion is the escape of a gas from a container through a tiny opening into an evacuated space. The rate of effusion of a gas is inversely proportional to the square root of its molar mass (Graham’s law), a relationship that closely approximates the rate of diffusion. As a result, light gases tend to diffuse and effuse much more rapidly than heavier gases.
- https://chem.libretexts.org/Courses/National_Yang_Ming_Chiao_Tung_University/Chemical_Principles_for_Medical_Students/05%3A_Gases/5.08%3A_Molecular_Effusion_and_DiffusionDiffusion is the gradual mixing of gases to form a sample of uniform composition even in the absence of mechanical agitation. In contrast, effusion is the escape of a gas from a container through a ti...Diffusion is the gradual mixing of gases to form a sample of uniform composition even in the absence of mechanical agitation. In contrast, effusion is the escape of a gas from a container through a tiny opening into an evacuated space. The rate of effusion of a gas is inversely proportional to the square root of its molar mass (Graham’s law), a relationship that closely approximates the rate of diffusion. As a result, light gases tend to diffuse and effuse much more rapidly than heavier gases.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/02%3A_Gases/2.06%3A_Collisions_with_Other_MoleculesThe page discusses the importance of understanding molecular collisions in gas-phase experiments, specifically molecular beams. It explains how to predict collision frequency by considering molecules ...The page discusses the importance of understanding molecular collisions in gas-phase experiments, specifically molecular beams. It explains how to predict collision frequency by considering molecules as spheres and outlines the concept of a "collision cylinder." Relevant formulas are provided for calculating the number of collisions, frequency of collisions, and mean free path, taking into account factors like pressure, temperature, and molecular size.
- https://chem.libretexts.org/Under_Construction/Purgatory/CHM_363%3A_Physical_Chemistry_I/13%3A_Kinetic_Theory_of_Gases/13.02%3A_Collision_TheoryThe mean free path is the distance a particle will travel, on average, before experiencing a collision event. This is defined as the product of the speed of a particle and the time between collisions.
- https://chem.libretexts.org/Courses/CSU_San_Bernardino/CHEM_2200%3A_General_Chemistry_II_(Mink)/09%3A_Gases/9.05%3A_Effusion_and_Diffusion_of_GasesGaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to region...Gaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to regions of relatively low concentration. Effusion is a similar process with gaseous species passing from a container to vacuum through a small orifices. The rates of effusion of gases are inversely proportional to the square roots of their densities or to the square roots of their atoms/molecules’ masses.
- https://chem.libretexts.org/Courses/Louisville_Collegiate_School/General_Chemistry/LibreTexts_Louisville_Collegiate_School_Chapters_09%3A_Gases/LibreTexts%2F%2FLouisville_Collegiate_School%2F%2FChapters%2F%2F09%3A_Gases%2F%2F9.4%3A_Effusion_and_Diffusion_of_GasesGaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to region...Gaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to regions of relatively low concentration. Effusion is a similar process with gaseous species passing from a container to vacuum through a small orifices. The rates of effusion of gases are inversely proportional to the square roots of their densities or to the square roots of their atoms/molecules’ masses.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_I/07%3A_Kinetic-Molecular_Theory_and_States_of_Matter/7.05%3A_Effusion_and_Diffusion_of_GasesGaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to region...Gaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to regions of relatively low concentration. Effusion is a similar process with gaseous species passing from a container to vacuum through a small orifices. The rates of effusion of gases are inversely proportional to the square roots of their densities or to the square roots of their atoms/molecules’ masses.
- https://chem.libretexts.org/Courses/Widener_University/CHEM_145%3A_FA22_Van_Bramer/05%3A_Gases/5.04%3A_Effusion_and_Diffusion_of_GasesGaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to region...Gaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to regions of relatively low concentration. Effusion is a similar process with gaseous species passing from a container to vacuum through a small orifices. The rates of effusion of gases are inversely proportional to the square roots of their densities or to the square roots of their atoms/molecules’ masses.
- https://chem.libretexts.org/Courses/New_York_University/CHEM-UA_652%3A_Thermodynamics_and_Kinetics/01%3A_Lectures/1.06%3A_Equipartitioning_collisions_and_random_walks\[\begin{align} \text{ln} \: P(k) &\approx N \: \text{ln} \: N - N - N \: \text{ln} \: 2 - \dfrac{1}{2} (N + k) \: \text{ln} \: \dfrac{1}{2} (N + k) + \dfrac{1}{2} (N + k) - \dfrac{1}{2} (N - k) \: \t...\[\begin{align} \text{ln} \: P(k) &\approx N \: \text{ln} \: N - N - N \: \text{ln} \: 2 - \dfrac{1}{2} (N + k) \: \text{ln} \: \dfrac{1}{2} (N + k) + \dfrac{1}{2} (N + k) - \dfrac{1}{2} (N - k) \: \text{ln} \: \dfrac{1}{2} (N - k) + \dfrac{1}{2} (N - k) \\ &= N \: \text{ln} \: N - N \: \text{ln} \: 2 + \dfrac{1}{2} (N + k) \: \text{ln} \: \dfrac{1}{2} - \dfrac{1}{2} (N + k) \: \text{ln} \: (N + k) - \dfrac{1}{2} (N - k) \: \text{ln} \: \dfrac{1}{2} - \dfrac{1}{2} (N - k) \: \text{ln} \: (N - k…
- https://chem.libretexts.org/Workbench/Username%3A_marzluff@grinnell.edu/CHM363_Chapter/13%3A_Kinetic_Theory_of_Gases/13.2%3A_Collision_TheoryThe mean free path is the distance a particle will travel, on average, before experiencing a collision event. This is defined as the product of the speed of a particle and the time between collisions.
- https://chem.libretexts.org/Courses/Nassau_Community_College/General_Chemistry_1/08%3A_Gases/8.04%3A_Effusion_and_Diffusion_of_GasesGaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to region...Gaseous atoms and molecules move freely and randomly through space. Diffusion is the process whereby gaseous atoms and molecules are transferred from regions of relatively high concentration to regions of relatively low concentration. Effusion is a similar process with gaseous species passing from a container to vacuum through a small orifices. The rates of effusion of gases are inversely proportional to the square roots of their densities or to the square roots of their atoms/molecules’ masses.
