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Chemistry Unit 8

TermDefinition
Kinetic Theory of Gases The particles in a gas are considered to be small, hard spheres with an insignificant volume and no attraction for each other. Motion of the particles is rapid, constant, and random. All collisions are perfectly elastic so no energy is lost
Compressibility A measure of how much the volume of matter decreases under pressure. Easily compress because of the space between the particles
Amount of gas If you increase the amount of particles, the pressure will increase. More collisions = more pressure
Volume By reducing the volume, you can increase the pressure. Same number of particles, but in a smaller area
Temperature An increase in temperature causes an increase in pressure. As gas is heated, the temperature increases and the average kinetic energy of the particles increase. Faster-moving particles inoact the walls of their container with more energy
Boyle's Law (pressure - volume relationship) If the temperature is constant as the pressure of gas increases the volume decreases. Formula: P1 x V1 = P2 x V2
Charles's Law (volume-temperature relationship) As the temperature of an enclosed gas increases, the volume increases, if the pressure is constant. Temperature must be in kelvin. Formula V1/T1 = V2/T2
Gay-Lussac's Law (Pressure - temperature relationship) As the temperature of an enclosed gas increases, the pressure increases if the volume is constant. Temperature must be in kelvin. P1/T2 = P2/T2
Combined Gas Law Describes the relationship among the pressure, volume and temperature of an enclosed gas. Formula P1 x V1/T1 = P2 x V2/T2
Created by: user-1866784
 

 



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