Kinetic Theory of Temperature and Pressure - AP Physics 2

Collisions are elastic. No energy lost in collisions.

It relates energy units in the ideal gas law. Proportionality constant in gas equations.

Temperature. Pressure and volume vary inversely.

No net energy transfer between objects. Same temperature means equal average energies.

$KE = \frac{1}{2}mv^2$. Energy from mass and velocity squared.

Pascal (Pa). Newton per square meter.

$P_{total} = P_1 + P_2 + \text{...}$. Additive pressures in gas mixtures.

$\rho = \frac{P \times M}{R \times T}$. Derived from ideal gas law rearrangement.

Volume is directly proportional to moles. Equal volumes contain equal moles at STP.

Pressure doubles. Inverse relationship from Boyle's Law.

Energy is distributed according to a Maxwell-Boltzmann distribution. Statistical description of particle energies.

Kinetic energy is directly proportional to temperature. Temperature measures average kinetic energy.

$PV = nRT$. Combines pressure, volume, moles, and temperature.

Kelvin (K). Absolute temperature scale required.

Collisions of gas particles with the walls. Momentum transfer from particle impacts.

Total pressure is the sum of partial pressures. Each gas contributes independently.

Pressure is directly proportional to temperature. At constant volume, $\frac{P}{T} = k$.

Pressure is inversely proportional to volume. At constant temperature, $PV = k$.

Volume is reduced to one-third. Inverse pressure-volume relationship applied.

The temperature at which particle motion stops. Zero kinetic energy at -273.15°C.

Particles are point-like with negligible volume. Ideal gas approximation assumption.

Pressure. Volume and temperature vary at fixed pressure.

Combined Gas Law. Combines Boyle's, Charles's, and Gay-Lussac's laws.

Kinetic energy decreases. Temperature directly affects molecular energy.

$8.314 \frac{J}{mol \times K}$. Standard value for gas calculations.

Speed of sound increases with temperature. Sound speed depends on molecular motion.

$22.4 \text{ L/mol}$. Standard molar volume for ideal gases.

Pressure is halved. Application of Boyle's Law calculation.

Particles are in constant random motion. Foundation of kinetic molecular theory.