A chemist finds that 30.82 g of nitrogen will react with 17.60, 35.20, 70.40, or 88.00 g of oxygen to form four different compounds. (b) How do the numbers in part (a) support Dalton's atomic theory?

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Identify the mass ratios of oxygen that react with a fixed mass of nitrogen in each compound. These ratios are 17.60 g, 35.20 g, 70.40 g, and 88.00 g of oxygen for every 30.82 g of nitrogen.

Calculate the ratios of the masses of oxygen to nitrogen for each compound. For example, for the first compound, divide the mass of oxygen (17.60 g) by the mass of nitrogen (30.82 g). Repeat this for each of the other masses of oxygen.

Observe that each of these ratios represents a simple whole number multiple of the smallest ratio. This suggests that the different amounts of oxygen are combining in whole number ratios to form different compounds.

Relate these findings to Dalton's atomic theory, which states that elements combine in simple whole number ratios to form compounds. The data supports this by showing that oxygen atoms combine with nitrogen atoms in fixed, simple, whole number ratios to form different chemical compounds.

Conclude that the experimental data provided supports Dalton's atomic theory, reinforcing the idea that atoms are indivisible particles that combine in specific proportions to form compounds.

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Dalton's Atomic Theory

Dalton's Atomic Theory posits that matter is composed of indivisible atoms, which combine in fixed ratios to form compounds. This theory explains the conservation of mass in chemical reactions and the distinct properties of different substances based on their atomic composition. The idea that elements combine in specific proportions is fundamental to understanding chemical reactions.

Law of Multiple Proportions

The Law of Multiple Proportions states that when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other can be expressed as a ratio of small whole numbers. This principle supports Dalton's theory by demonstrating that compounds are formed from atoms in specific, quantifiable ratios, as seen in the varying amounts of oxygen reacting with nitrogen.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass and the mole concept. It allows chemists to predict the amounts of substances consumed and produced in a reaction. In the context of the question, stoichiometry helps to analyze how different masses of oxygen react with a fixed mass of nitrogen, illustrating the principles of Dalton's theory.