Chemistry · States of Matter - Gases, Liquids and Solids

The correct answer is Avogadro's Law. This fundamental principle states that equal volumes of gases, at the same temperature and pressure, will contain an equal number of molecules. This is pivotal for understanding gas behavior in chemistry and physics.

Graham's Law is concerned with the diffusion and effusion rates of gases, which depend on molecular weight, not volume and particle number.

Dalton's Law explains the pressure contributions of individual gases in a mixture, but does not relate to volume and molecule count.

Hund's Rule pertains to electron occupation in atomic orbitals, which is irrelevant to gas laws and molecular volume relationships.

Avogadro's Law states that when temperature and pressure are held constant, equal volumes of different gases contain the same number of molecules. This concept is rooted in the behavior of ideal gases and is crucial for understanding stoichiometry and gas reactions.

Graham's Law deals with the rates of diffusion and effusion of gases, indicating that these rates are inversely proportional to the square root of the gas's molecular weight. It is not related to the volume and number of molecules in gases.

Dalton's Law of Partial Pressures states that in a mixture of non-reacting gases, the total pressure is the sum of the partial pressures of each individual gas. It does not address the relationship between volume and the number of molecules.

Hund's Rule relates to electron configurations in atomic orbitals, stating that electrons will fill an unoccupied orbital before pairing up. It is not applicable to gases or their volumes.