Question

fill in the statements below that describe how kinetic molecular theory explains the gas laws.
boyles law
if the gas volume is decreased, the container wall area -- and the molecule - wall collision frequency --, both of which -- the pressure exerted by the gas.
daltons law
because of the large distances between them, the molecules of one gas in a mixture bombard the container walls with --, and the total pressure of a gas mixture equals the --.
gay - lusacs law
if the temperature is increased, the average speed and kinetic energy of the gas molecules --. if the volume is held constant, this results in -- frequent and forceful collisions with the walls of the container, therefore -- the pressure.
charless law
if the temperature of a gas is increased, a constant pressure may be maintained only if the volume occupied by the gas --. this will result in -- average distances traveled by the molecules to reach the container walls, as well as wall surface area. these conditions will -- both the frequency of molecule - wall collisions and the number of collisions per unit area, the combined effects of which balance the effect of increased collision forces due to the greater kinetic energy at the higher temperature.

Explanation:

• Boyle's Law: According to kinetic molecular theory, when gas volume decreases, container wall area decreases (less space for molecules to spread out). With fewer molecules per unit area initially, but as volume drops, molecule - wall collision frequency increases (molecules have less space to move, so they hit the walls more often). Both these factors (decreased area and increased collision frequency) increase pressure (pressure is force per unit area, more collisions and less area lead to higher force per unit area).
• Dalton's Law: Gas molecules in a mixture are far apart (assumption of kinetic molecular theory for ideal gases). So, molecules of one gas bombard container walls independently (no significant intermolecular forces to affect their motion relative to the container walls). The total pressure of a gas mixture equals the sum of the partial pressures of each gas (each gas behaves as if it were alone in the container, so we add up their individual pressures).
• Gay - Lusacs Law: When temperature increases, average speed and kinetic energy of gas molecules increase (temperature is a measure of average kinetic energy in kinetic molecular theory). If volume is constant, this results in more frequent and forceful collisions (faster molecules hit the walls more often and with more force). Therefore, pressure increases (more forceful and frequent collisions mean higher force per unit area).
• Charles’s Law: If gas temperature increases, to maintain constant pressure, volume occupied by the gas must increase (from the ideal gas law \(PV = nRT\), at constant \(P\) and \(n\), \(V\propto T\)). This results in greater average distances traveled by molecules to reach container walls (more volume, so molecules have to move farther on average) and increased wall surface area (volume increase often means larger container, so more surface area). These conditions decrease both the frequency of molecule - wall collisions (more space, so less frequent hits) and the number of collisions per unit area (more area, so fewer collisions per unit area). The combined effects balance the effect of increased collision forces (from higher temperature) to keep pressure constant.

Answer:

• Boyle's Law: decreases; increases; increase
• Dalton's Law: independence; sum of the partial pressures of each gas
• Gay - Lusacs Law: increase; more; increasing
• Charles’s Law: increases; greater; decrease