Atomic Models

Dalton's Atomic Theory was a significant step in the development of modern chemistry, but it had some limitations:

- Law of constant proportion: According to Dalton's theory, each compound is composed of atoms of different elements combined in fixed ratios. This is consistent with the law of constant proportion, which Dalton’s theory could explain.
- Law of multiple proportion: Dalton's theory also explained the law of multiple proportions, where elements combine in simple, whole-number ratios to form different compounds.
- Law of gaseous volume: The law of gaseous volume (Gay-Lussac's Law) states that gases combine in simple whole-number ratios by volume when measured at the same temperature and pressure. Dalton’s Atomic Theory could not explain this law because it assumed that the atoms of different elements were indivisible and had fixed volumes, but Gay-Lussac's law involves the behavior of gases, which require a more advanced understanding of molecular behavior.
- Law of conservation of mass: Dalton’s theory also aligned with the law of conservation of mass, as it implied that the mass of reactants equals the mass of products, since atoms are neither created nor destroyed.

Thus, the correct answer is (3) Law of gaseous volume, as Dalton’s Atomic Theory could not explain this phenomenon.