1. States of matter
• Matter is anything that has mass and occupies space. According to the kinetic theory of matter, all matter is made up of atoms or molecules which are in continuous random motion. It is represented by a model called kinetic molecular model of matter.
• The different state of matter (solid, liquid, and gas) have different properties.
• This difference could be explained based on how individual atoms or molecules are held together in a matter.
• The following table summarizes properties of solids, liquids, and gases, and identifies the microscopic behavior responsible for each property.
Properties Solid Liquid Gas
Shape Fixed shape No fixed shape, takes vessel shape No fixed shape, takes entire container shape
Molecular
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• Diffusion is the process of spreading out of molecules due to its random motion. Diffusion in liquid occurs at much slower rate compared to gas.
• Rate of diffusion of gas depends on o Gas density (denser gas has slower diffusion rate) o Temperature (higher temperature causes faster diffusion)
4. Pressure, Volume and Temperature of Gas Particles
4.1. Pressure
• Explanation: o The gas particles collide with one another and with the walls of the container. o While the particles strike and rebound on the walls, a force is exerted. o These large numbers of collisions produces a measurable total average force on the walls. o Assumes that the molecules are moving randomly in all directions, the force per unit area, which is pressure exerted by the gas, is equal in all directions.
4.2. Volume
• Tthe gas particles are distributed evenly to occupy the space of the container.
4.3. Temperature
• Increasing the temperature increases the average kinetic energy of particles as particles move faster.
5. Relationship between Pressure, Volume, and Temperature
• Mathematically, these three quantities are related by the