Ch.2 - Atoms & Elements

Problem 35

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Chapter 2, Problem 35

Two different compounds containing osmium and oxygen have the following masses of oxygen per gram of osmium: 0.168 and 0.3369 g. Show that these amounts are consistent with the law of multiple proportions.

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Identify the two compounds as Compound A and Compound B, where Compound A has 0.168 g of oxygen per gram of osmium and Compound B has 0.3369 g of oxygen per gram of osmium.

According to the law of multiple proportions, if two elements form more than one compound, the masses of one element that combine with a fixed mass of the other are in the ratio of small whole numbers.

Calculate the ratio of the masses of oxygen in the two compounds by dividing the mass of oxygen in Compound B by the mass of oxygen in Compound A: \( \frac{0.3369}{0.168} \).

Simplify the ratio obtained in the previous step to see if it can be expressed as a ratio of small whole numbers.

Conclude that if the ratio is a small whole number, the compounds are consistent with the law of multiple proportions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Law of Multiple Proportions

The Law of Multiple Proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element can be expressed as small whole numbers. This principle highlights the discrete nature of chemical combinations and supports the idea that compounds are formed from specific ratios of atoms.

Mass Ratio Calculation

To demonstrate the Law of Multiple Proportions, one must calculate the mass ratios of oxygen to osmium in the given compounds. By dividing the mass of oxygen by the mass of osmium for each compound, we can compare these ratios to see if they form a simple whole number ratio, which is essential for validating the law.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. Understanding stoichiometry is crucial for analyzing the composition of compounds and determining how different elements combine in fixed ratios, which is fundamental to applying the Law of Multiple Proportions.

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Stoichiometry Concept

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Related Practice

Open Question

Two samples of sodium chloride are decomposed into their constituent elements. One sample produces 6.98 g of sodium and 10.7 g of chlorine, and the other sample produces 11.2 g of sodium and 17.3 g of chlorine. Are these results consistent with the law of definite proportions? Explain your answer.

Textbook Question

The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces 28.8 g of sodium upon decomposition. How much fluorine (in grams) forms?

Upon decomposition, one sample of magnesium fluoride produces 1.65 kg of magnesium and 2.57 kg of fluorine. A second sample produces 1.32 kg of magnesium. How much fluorine (in grams) does the second sample produce?

Palladium forms three different compounds with sulfur. The mass of sulfur per gram of palladium in each compound is listed here. Show that these masses are consistent with the law of multiple proportions. Compound Grams S per Gram Pd A 0.603 B 0.301 C 0.151

Sulfur and oxygen form both sulfur dioxide and sulfur trioxide. When samples of these are decomposed, the sulfur dioxide produces 3.49 g oxygen and 3.50 g sulfur, while the sulfur trioxide produces 6.75 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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Textbook Question

Sulfur and fluorine form several different compounds including sulfur hexafluoride and sulfur tetrafluoride. Decomposition of a sample of sulfur hexafluoride produces 4.45 g of fluorine and 1.25 g of sulfur, while decomposition of a sample of sulfur tetrafluoride produces 4.43 g of fluorine and 1.87 g of sulfur. Calculate the mass of fluorine per gram of sulfur for each sample and show that these results are consistent with the law of multiple proportions.

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