KMT and Ideal Gas Law Flashcards

Vocabulary flashcards based on lecture notes about Kinetic Molecular Theory and the Ideal Gas Law.

Kinetic Molecular Theory (KMT)

Provides the simplest model for the behavior of gases; helps us picture what is happening to gas particles when conditions such as pressure or temperature change.

KMT Postulate 1: Particle Size

The size of gas particles is negligible due to the large space between them.

KMT Postulate 2: Particle Motion

Gas particles are in constant, random motion, moving in straight lines until they collide.

KMT Postulate 3: Elastic Collisions

Collisions between gas particles are completely elastic, meaning there is no overall loss of energy.

KMT Postulate 4: Intermolecular Forces

Gas particles have negligible attractive or repulsive forces between them; intermolecular forces can be ignored.

KMT Postulate 5: Kinetic Energy and Temperature

The average kinetic energy of a gas sample is proportional to the Kelvin temperature of the gas.

KMT Summary

Gas molecules are dots that randomly bump into each other and have NO intermolecular forces.

Temperature of a Gas

A measurement of a gas's kinetic energy.

Gas Speed and Temperature

At equal temperatures, light gases move faster, and heavy gases move slower.

Gas Pressure

Force per unit area exerted by a gas colliding with a surface.

SI Unit for Pressure

Pascal (Pa)

Average Atmospheric Pressure at Sea Level

760 mmHg or 101.325 kPa

Variables in Ideal Gas Law

Pressure (P), Volume (V), Amount of substance (n), Ideal gas constant (R), Temperature (T)

Value of Ideal Gas Constant (R)

0.08206 L atm / mol K

Ideal Gas Law

PV = nRT