Gas Laws and Kinetic Theory Quiz

In Boyle's Law, the pressure and volume of a gas are inversely proportional, meaning as one increases, the other decreases.

The kinetic theory states that gas particles are considered point masses with negligible volume compared to the space they occupy.

The SI unit of pressure is the Pascal (Pa), named after Blaise Pascal, and is equivalent to one Newton per square meter.

The mathematical relationship in Boyle's Law is expressed as P ∝ 1/V, indicating that pressure is inversely proportional to volume.

According to Avogadro's Law, at constant temperature and pressure, the volume of a gas is directly proportional to its number of moles.

Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature.

STP is defined as 0°C temperature and 1 atmosphere pressure, commonly used as a reference point in gas law calculations.

Gay-Lussac's Law states that the pressure of a gas is directly proportional to its absolute temperature when volume is held constant.

The Combined Gas Law combines Boyle's, Charles's, and Gay-Lussac's Laws into a single equation describing the relationship between pressure, volume, and temperature.

The ideal gas law equation, PV = nRT, describes the relationship between pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) for an ideal gas.

Dalton's Law states that in a mixture of gases, the total pressure is the sum of the partial pressures exerted by each gas.

The van der Waals equation corrects for the ideal gas law's assumptions by considering attractions between gas particles and adjusting for their finite volumes.

The root mean square speed of gas molecules is directly proportional to the square root of their temperature, according to kinetic theory.

The Boltzmann constant relates the average kinetic energy of gas particles to the temperature of the gas in kinetic theory.