Properties of Substances and Mixtures

These flashcards cover key concepts related to the properties of substances and mixtures, focusing on the Kinetic Molecular Theory and its implications in gas behavior.

Kinetic Molecular Theory (KMT)

A theory that explains the behavior of gases in terms of particles in constant random motion.

Pressure

The force exerted by gas particles colliding with the walls of a container.

Ideal Gas Law

An equation of state for an ideal gas that describes the relationship between pressure (P), volume (V), temperature (T), and number of moles (n).

Maxwell-Boltzmann Distribution

A statistical distribution of the speeds of particles in a gas, indicating that they do not all move at the same speed.

Average Kinetic Energy

The measure of the energy of motion of particles, which is directly proportional to the temperature in Kelvin.

Elastic Collisions

Collisions between gas particles that conserve momentum and kinetic energy.

Atmospheric Pressure Conversion

1 atm is equivalent to 760 mm Hg or 760 torr.

Temperature Effect on Reaction Rate

A higher temperature increases the number of effective molecular collisions, thereby increasing the reaction rate.

Volume Occupied by Gas Particles

In gases, the volume occupied by individual particles is negligible compared to the total volume of the gas.

Effect of Temperature on Maxwell-Boltzmann Curve

As temperature increases, the distribution curve flattens and shifts right, indicating more particles have higher kinetic energy.