Gases KMT: Boyle's Law and Charle's Law

KMT?

Kinetic Molecular Theory

Properties of Gas:

? or more gases form a homogenous mixture

Two or more gases form a homogenous mixture

No definite ? or ?

Gas expands ? to fill its container

No definite volume or shape

Gas expands spontaneously to fill its container

• ? compressible

  • Gas molecules can be pushed closer together because the gas particles are far apart.

• Highly compressible

  • Gas molecules can be pushed closer together because the gas particles are far apart.

Exerts ? on the walls of the container

Exerts pressure on the walls of the container

• Explain the states of matter

• Describes the behavior of an ideal gas

• The foundation for the gas laws

Kinetic-Molecular Theory

What shape particles are the gases?

spherical particles that are far apart

They move in ? rapid motion in ? directions

in constant rapid motion in random directions.

? forces of attraction or repulsion between gas particles

NO forces of attraction or repulsion between gas particles

Collisions between molecules and container are perfectly ? collisions

Collisions between molecules and container are perfectly elastic collisions

The average kinetic energy of gas particles is ? upon the temperature

The average kinetic energy of gas particles is dependent upon the temperature

At a constant temperature, the change in pressure is ? proportional to the change in volume.

At a constant temperature, the change in pressure is inversely proportional to the change in volume.

Formula for Boyle’s Law

Standard Pressure (STP) = ?

Standard Pressure (STP) = 1.0 atm

At a constant pressure, the change in volume is ? proportional to the change in absolute temperature.

At a constant pressure, the change in volume is directly proportional to the change in absolute temperature.

What is the Formula for Charles’s Law

Standard Temperature = ?

Standard Temperature = 273.15 K

Formula for Celsius to Kelvin

Formula for Fahrenheit to Celsius