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Kinetic Molecular Theory explains the behavior of gases by assuming that they are composed of a large number of small particles in constant, random motion, and that the collisions between these particles and the walls of their container account for gas pressure. This theory helps to understand macroscopic properties of gases such as temperature, pressure, and volume through the microscopic interactions of particles.
Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass, implying that lighter gases effuse more quickly than heavier ones. This principle is crucial for understanding gas behavior in various scientific applications, including separation processes and kinetic molecular theory.
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Molar mass is the mass of one mole of a substance, typically expressed in grams per mole, and is calculated by summing the atomic masses of all atoms in a molecule as given on the periodic table. It is a fundamental concept in chemistry that connects the macroscopic world of grams and liters to the microscopic world of atoms and molecules, allowing for stoichiometric calculations in chemical reactions.
Mean free path is the average distance a particle travels between collisions in a medium, reflecting the medium's density and the particle's cross-sectional area. It is a crucial parameter in understanding transport phenomena in gases, plasmas, and other systems where particles move freely between interactions.
A concentration gradient is the gradual change in the concentration of solutes in a solution between two regions, which often drives the movement of substances in biological and chemical processes. This gradient is a fundamental principle in diffusion, where particles move from areas of higher concentration to areas of lower concentration until equilibrium is reached.
Brownian motion is the random movement of particles suspended in a fluid, resulting from their collision with the fast-moving molecules in the fluid. It is a fundamental concept in statistical physics and serves as a mathematical model for stochastic processes, with applications in fields such as finance, biology, and physics.
The Ideal Gas Law is a fundamental equation in chemistry and physics that relates the pressure, volume, temperature, and amount of an ideal gas using the formula PV=nRT. It assumes no interactions between gas molecules and that the molecules occupy no volume, making it most accurate for gases at low pressure and high temperature.
Partial pressure refers to the pressure that a single component of a mixture of gases would exert if it occupied the entire volume alone at the same temperature. It is a crucial concept in understanding gas mixtures, as it allows for the calculation of individual gas contributions to the total pressure, which is essential in fields like chemistry, physics, and engineering.
The gaseous state is a form of matter where particles are in constant, rapid motion and fill up the entire volume available to them, resulting in no definite shape or volume. This state is characterized by low density and high kinetic energy compared to solids and liquids, due to the large distances between particles and minimal intermolecular forces.
Gas mixtures consist of two or more different gases combined without chemical bonding, where each component retains its own distinct properties. The behavior and properties of Gas mixtures can be studied using principles like Dalton's Law and the Ideal Gas Law to predict how they interact and function collectively under varying conditions.
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