How does Dalton's atomic theory account for the law of mass conservation and the law of definite proportions?

Dalton's atomic theory posits that matter is composed of indivisible atoms, which are the fundamental building blocks of all substances. Each element consists of identical atoms that differ from those of other elements. This theory laid the groundwork for understanding chemical reactions as rearrangements of atoms, rather than changes in the atoms themselves.

The law of mass conservation states that mass is neither created nor destroyed in a chemical reaction. This principle implies that the total mass of reactants must equal the total mass of products. Dalton's atomic theory supports this law by asserting that atoms are simply rearranged during reactions, ensuring that the same number of atoms (and thus mass) is present before and after the reaction.

The law of definite proportions states that a chemical compound always contains its component elements in fixed ratio by mass, regardless of the sample size or source. Dalton's atomic theory explains this by suggesting that compounds are formed from specific combinations of atoms in defined ratios, which leads to consistent proportions of elements in any given compound.