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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
