Kinetic Molecular Theory - AP Chemistry

Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

Particles move in straight lines until collision. Linear motion between elastic collisions.

Particles move in straight lines until collision. Linear motion between elastic collisions.

Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

$KE = \frac{3}{2} k T$. Where $k$ is Boltzmann constant and $T$ is temperature.

No attractive forces between particles. Ideal gas assumption for simplified behavior.

Average kinetic energy doubles. Kinetic energy directly proportional to temperature.

Molar mass affects particle speed; heavier particles move slower. Lighter molecules move faster at same temperature.

Average kinetic energy at constant temperature. At constant $T$, all gas particles have the same average $KE$.

Particles are in constant, random motion. This is the first fundamental postulate of kinetic theory.

Pressure increases as volume decreases. Less space means more frequent wall collisions.

Speed increases with temperature. Higher temperature means greater kinetic energy and velocity.

Particle volume is negligible compared to container volume. Point particles assumption for ideal gas behavior.

Pressure is due to collisions of particles with container walls. Moving particles strike walls, creating force per unit area.

Pressure is halved. Direct proportionality: $P \propto T$ at constant volume.

Kinetic energy is directly proportional to temperature in Kelvin. $KE \propto T$ where $T$ is in Kelvin scale.

Gas pressure increases as temperature increases. More collisions with walls due to faster particle motion.

Temperature remains constant. Isothermal means constant temperature process.

Real gases deviate due to intermolecular forces. Attractions reduce pressure; finite size affects volume.

Pressure is directly proportional to temperature. Gay-Lussac's law at constant volume.

Thermal energy. Temperature is a measure of average kinetic energy.

Particles move faster as temperature increases. Higher $T$ means greater average kinetic energy and speed.

Ideal Gas Law: $PV = nRT$. Derived from kinetic theory assumptions about gas behavior.

Inverse of the square root of molar mass. Graham's law: rate $\propto \frac{1}{\sqrt{M}}$.

Particles are far apart, allowing compression. Large spaces between molecules allow volume reduction.

Random motion allows particles to spread out over time. Random paths lead to net movement from high to low concentration.

Random motion allows particles to spread out over time. Random paths lead to net movement from high to low concentration.

Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

Particles move in straight lines until collision. Linear motion between elastic collisions.