Day 1: KMT

These flashcards cover key concepts of the Kinetic Molecular Theory, properties of gases, and pressure measurements.

Kinetic Molecular Theory

A simple model for gases that predicts their behavior under many conditions.

Elastic Collisions

Collisions between gas particles where no energy is lost or gained.

Negligible Particle Size

The size of gas particles is so small compared to the distance between them that it can be considered unimportant.

Proportional to Temperature

The average kinetic energy of gas particles increases with the temperature in Kelvin.

Compressibility of Gases

Gases can be compressed because there is a lot of space between their particles.

Gas Pressure

The amount of force exerted per unit area, caused by collisions of gas particles with the walls of their container.

Units of Pressure

Common units of pressure include pascal, atmosphere, millimeters of mercury, torr, pounds per square inch (psi), and inches of mercury.

Atmospheric Pressure at Sea Level

Standard pressure at sea level is defined as one atmosphere, equivalent to 101,325 pascals.

Kelvin Temperature

A temperature scale where absolute zero is zero kelvins; calculations with gases must use this scale.

Density of Gases

Gases have much lower densities compared to liquids and solids due to the large spaces between particles.