Kinetic Theory Flashcards
Kinetic theory of matter (5)
All matter is made of small particles, spaces between particles, particles held together by attractive forces, particles are always moving (except at absolute 0), particles move faster at higher temperatures
Matter
Anything that has mass and takes up space
Solids
Least kinetic energy, particles close together, particles vibrate but cannot move, strong attractive forces
Liquids
More kinetic energy, particles not packed as closely, particles can move by sliding over each other, forces are moderate
Gases
Most kinetic energy, particles are widely spaced, particles can move freely, no forces between the particles
Density, shape, volume, compressibility and ability to mix in a solid
High density, fixed shape and volume, cannot be compressed, does not mix unless finely divided
Density, shape, volume, compressibility and ability to mix in a liquid
High density, variable shape, fixed volume, cannot be compressed, slowly mixes unless stirred
Density, shape, volume, compressibility and ability to mix in a gas
Low density, variable shape and volume, easy to compress, rapidly mixes together
Kinetic energy
Due to motion
Potential energy
Stored energy
Solid energy
Low potential energy because the distance between each particle is small
Gas energy
High Potential energy because there is a greater amount of energy needed to overcome the attractive forces
Heat
Energy transferred from one place to another due to a temperature difference
Temperature
Measure of the AVERAGE random kinetic energy
Assumptions of kinetic theory gases (7) (ideal gasses)
Gases made up of atoms or molecules, total volume occupied is negligible and distance between each particle is greater than size, particles move randomly in straight line, particles collide, weak forces between particles, kinetic energy conserved between collisions, average kinetic energy increases as temp and pressure increases
Collisions between gas particles involve
Transfer of kinetic energy between particles and a change in the direction of motion
Maxwell-Boltzmann plot
Describes the energy distribution of the particles in the substance
Increased temperature causes
Increase in average kinetic energy
Volume
Quantity used to describe the space a substance occupies
Pressure
Force that is exerted over an area
Boyles law
Pressure and volume are inversely proportional, if temp is constant, volume decreases- pressure increases
Charles law
Temp and volume are directly proportional if the pressure is constant, temp increases- volume increases
Gay-lusacs
volumes of gasses is in the same ratio as the co-efficients of the balanced equation
Exothermic
Releases energy into surroundings (change in enthalpy is negative)
Endothermic
Absorbs energy from surroundings,
Energy in a solid, liquid and gaseous state
Kinetic energy increases, potential energy is constant
Energy when changing state
Potential energy increases, kinetic energy stays constant
Ideal gases
Linear, random, elastic collisions, no intermolecular forces, no volume
Real gases
brownian, not perfectly elastic, weak intermolecular forces, small volume
Conditions for a real gas
Hight temp, low pressure