Gas Laws & Kinetic Molecular Theory
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12 Terms
Matter
Anything that has mass and takes up space, composed of particles that are always moving.
Kinetic Energy
The energy an object has due to its motion; more kinetic energy corresponds to higher temperature.
Brownian Motion
Random movement of particles suspended in a fluid, caused by collisions with smaller, faster-moving particles.
Temperature
A measure of the average kinetic energy of the particles in a substance, measured in Kelvin.
States of Matter
Different forms that matter can take: solid, liquid, and gas, ranked from least to most energy.
Phase Diagram
A graphical representation showing the relationship between pressure and temperature and how they determine the state of a substance.
Triple Point
The specific temperature and pressure where all three states of matter coexist.
Pressure
The force exerted by gas particles colliding with the walls of a container, measured in pascals (Pa), atmospheres (atm), or mmHg.
Boyle's Law
States that the pressure and volume of a gas have an inverse relationship when temperature and gas amount are constant: P1V1=P2V2.
Charles's Law
States that the volume of a gas is directly proportional to its temperature when pressure and gas amount are constant: V1/T1=V2/T2.
Gay-Lussac's Law
States that the pressure of a gas is directly proportional to its temperature when volume is constant: P1/T1=P2/T2.
Combined Gas Law
Describes the relationship between pressure, volume, and temperature of a gas while keeping the amount of gas constant: P1V1/T1=P2V2/T2.