Kinetic Theory of Gases topics include: gases and its reactions, ideal gases. The kinetic theory of gases is a model that describes gases as a large number of submicroscopic particles that are in constant, random motion. The particles frequently collide with each other and with the walls of any container. The kinetic theory relates the independent motion of molecules to the mechanical and thermal properties of gases. These properties include pressure, volume, temperature, viscosity, and heat conductivity. The kinetic theory of gases has five main postulates: The particles in a gas are... Show more Kinetic Theory of Gases topics include: gases and its reactions, ideal gases. The kinetic theory of gases is a model that describes gases as a large number of submicroscopic particles that are in constant, random motion. The particles frequently collide with each other and with the walls of any container. The kinetic theory relates the independent motion of molecules to the mechanical and thermal properties of gases. These properties include pressure, volume, temperature, viscosity, and heat conductivity. The kinetic theory of gases has five main postulates: The particles in a gas are in constant, random motion. The combined volume of the particles is negligible. The particles exert no forces on one another. Any collisions between the particles are completely elastic. Chemical reactions that produce a gas as a product are called gas evolution reactions. These reactions start with two reactants, or chemical compounds, which are changed during the reaction. The reaction ends with two products. An isothermal process is a process where the temperature of a system remains constant. An adiabatic process is a process where no heat is exchanged by the system. An ideal gas is a hypothetical gas that is made up of many randomly moving particles that don't interact with each other. The ideal gas concept is useful because it follows the ideal gas law, a simplified equation of state. Here are some assumptions about ideal gases: The gas particles have a negligible volume. The gas particles are the same size and don't have intermolecular forces with other gas particles. The gas particles move randomly in accordance with Newton's Laws of Motion. The only interaction between ideal gas molecules is an elastic collision when they hit each other or the container walls. The gas particles need to occupy zero volume and have no attractive forces toward each other. The ideal gas law was first stated in 1834 by Benoît Paul Émile Clapeyron. It's a combination of Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law. Show less
Kinetic Theory of Gases topics include: gases and its reactions, ideal gases.
The kinetic theory of gases is a model that describes gases as a large number of submicroscopic particles that are in constant, random motion. The particles frequently collide with each other and with the walls of any container.
The kinetic theory relates the independent motion of molecules to the mechanical and thermal properties of gases. These properties include pressure, volume, temperature, viscosity, and heat conductivity.
The kinetic theory of gases has five main postulates: The particles in a gas are in constant, random motion. The combined volume of the particles is negligible. The particles exert no forces on one another. Any collisions between the particles are completely elastic.
Chemical reactions that produce a gas as a product are called gas evolution reactions. These reactions start with two reactants, or chemical compounds, which are changed during the reaction. The reaction ends with two products.
An isothermal process is a process where the temperature of a system remains constant. An adiabatic process is a process where no heat is exchanged by the system.
An ideal gas is a hypothetical gas that is made up of many randomly moving particles that don't interact with each other. The ideal gas concept is useful because it follows the ideal gas law, a simplified equation of state.
Here are some assumptions about ideal gases: The gas particles have a negligible volume. The gas particles are the same size and don't have intermolecular forces with other gas particles. The gas particles move randomly in accordance with Newton's Laws of Motion. The only interaction between ideal gas molecules is an elastic collision when they hit each other or the container walls. The gas particles need to occupy zero volume and have no attractive forces toward each other.
The ideal gas law was first stated in 1834 by Benoît Paul Émile Clapeyron. It's a combination of Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law.
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