Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

In solids, particles are closely packed and vibrate in fixed positions, resulting in the least kinetic energy compared to liquids, gases, and plasmas.

In plasma, particles have the highest kinetic energy due to the extreme temperatures that ionize the gas.

According to Charles's Law, the volume of a gas increases with an increase in temperature at constant pressure.

The critical point is the temperature and pressure at which the gas and liquid phases of a substance become indistinguishable.

The ideal gas law is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.

Sublimation is the phase change from solid directly to gas without passing through the liquid phase.

The state of matter is primarily determined by the balance between temperature (kinetic energy) and intermolecular forces.

According to Gay-Lussac's Law, pressure is directly proportional to temperature when volume is held constant.

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

The ideal gas constant R is 0.0821 L·atm/(K·mol), which is commonly used in the ideal gas law.

Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature (PV = constant).

Real gases behave more ideally at low pressure and high temperature, where intermolecular forces and molecular volume become less significant.