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Chapter 1: Problem 15

State and explain the law of definite proportions.

Short Answer

Expert verified
The Law of Definite Proportions states that a chemical compound always contains exactly the same proportion of elements by mass. For example, water has a consistent hydrogen to oxygen mass ratio of 1:8.

Step by step solution

01

Understanding the Law

The Law of Definite Proportions, also known as Proust's Law, states that a chemical compound always contains exactly the same proportion of elements by mass. This law means that for any given compound, the ratio of the mass of one element to the mass of another element is always the same, regardless of the source of the compound or the amount of the compound that is being examined.
02

Example of the Law

To illustrate the law, consider water (H_2O). Every sample of water contains 2 grams of hydrogen for every 16 grams of oxygen. This means the ratio of hydrogen to oxygen by mass in water is always 2:16 or 1:8. No matter how much water you have, this mass proportion of hydrogen to oxygen will not vary.
03

Application of the Law

This law can be applied when analyzing a compound in a chemistry lab. If a compound is broken down into its constituent elements, the mass of each element can be measured. Then, the ratio of the masses of the elements can be compared to known values to help identify the compound and confirm that it adheres to the Law of Definite Proportions.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Compound Composition
Understanding the composition of a chemical compound is fundamental in the study of chemistry. Simply put, a chemical compound is a substance made up of two or more different types of atoms that are chemically bonded together. These atoms combine in a specific ratio, which is consistent across all samples of the compound. Consider table salt, which is a compound called sodium chloride. It is always made of one atom of sodium (Na) for every atom of chlorine (Cl). This one-to-one ratio is key to determining the properties of the compound, including melting point, boiling point, and reactivity.
Element Mass Ratio
The element mass ratio is a comparison of the amount of one element to another in a compound, measured by mass. This ratio is very precise and can be used as a signature for that compound. For instance, in carbon dioxide (CO2), there is one part by mass of carbon (C) to two parts by mass of oxygen (O). Even if we examine a single molecule or a truckload of CO2, the mass ratio remains a constant 1:2. Such unwavering ratios are essential for calculations and reactions in chemistry as they provide a reliable measure of how different elements will interact with one another.
Proust's Law
The Law of Definite Proportions, famously known as Proust's Law, is a classical law in chemistry proposed by Joseph Proust in the late 18th century. It asserts that a chemical compound will always be composed of the same elements in the same proportion by mass, regardless of the size of the sample or its source. This means that no matter how a compound is prepared, the mass percentages of the elements will remain constant. For example, whether you produce water chemically by combining hydrogen and oxygen or you simply take it from a river, the mass ratio of hydrogen to oxygen in water will always be found to be 1:8.
Chemical Compound Analysis
The process of chemical compound analysis involves determining the elements that make up a compound and their respective ratios. This can be achieved through various methods like spectroscopy, chromatography, or mass spectrometry. For example, to analyze a water sample, one might use electrolysis to separate it into hydrogen and oxygen gases. The mass of each gas could then be measured and compared. Such analytical techniques are critical for quality control in manufacturing, forensic science, environmental monitoring, and research into new substances, ensuring that the compounds meet the expected criteria laid out by principles like the Law of Definite Proportions.

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Most popular questions from this chapter

Sulfur and oxygen form both sulfur dioxide and sulfur trioxide. When samples of thesc are decomposed, the sulfur dioxide produces 3.49 \(\mathrm{g}\) oxygen and 3.50 \(\mathrm{g}\) sulfur, while the sulfur trioxide produces 6.75 \(\mathrm{g}\) oxygen and 4.50 g sulfur. Calculate the mass of oxygen per gram of sulfur for each sample and show that these results are consistent with the law of multiple proportions.

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