Kinetic and Molecular Theory

Gas particles are in constant random motion, moving in straight lines until they collide with other particles or with the walls of their container. This leads to a distribution of speed known as the __________ distribution.

Maxwell-Boltzmann

The average kinetic energy of gas particles is given by the equation KE = __________.

(3/2) kT

As temperature __________, the average kinetic energy increases, causing particles to move faster.

increases

In gas phases, the actual volume of individual gas particles is __________ compared to the total volume of the gas.

negligible

Under ideal conditions, there are __________ between gas particles, allowing them to behave independently.

no attractive or repulsive forces

Boyle's Law states that P1 V1 = P2 V2, indicating an __________ relationship between pressure and volume.

inverse

Charles's Law illustrates the direct relationship between volume and __________.

temperature

Avogadro's Law states that equal volumes of gases at the same temperature and pressure contain equal numbers of __________.

molecules

The Ideal Gas Law is represented by the equation PV = nRT, where R is the __________ gas constant.

universal

The rate of effusion of a gas is inversely proportional to the square root of its __________.

molar mass

Real gases exhibit behavior that can deviate significantly from the predictions of the Ideal Gas Law due to the influence of __________.

intermolecular forces

The Van der Waals equation corrects for deviations from ideal behavior by adding terms for __________ and volume.

attractive forces

Real gases can behave more like ideal gases under conditions of __________ pressure and __________ temperature.

low; high

The presence of __________, such as van der Waals forces, significantly affects interactions between gas particles.

intermolecular forces