Ch.2 - Atoms & Elements

Problem 36

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Chapter 2, Problem 36

The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces 45.1 g of sodium upon decomposition. How much fluorine (in grams) forms?

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Key Concepts

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

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for solving problems involving mass ratios and conversions between different substances.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. In the context of sodium fluoride (NaF), knowing the molar masses of sodium (Na) and fluorine (F) is crucial for determining the mass of fluorine produced when a specific mass of sodium is decomposed.

Mass Ratio

The mass ratio is a comparison of the mass of one substance to the mass of another substance in a compound. In sodium fluoride, the mass ratio of sodium to fluorine is given as 1.21:1, indicating that for every 1.21 grams of sodium, there is 1 gram of fluorine. This ratio is vital for calculating the amount of fluorine produced from a known mass of sodium, as it provides a direct relationship between the two elements.

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Related Practice

An automobile gasoline tank holds 42 kg of gasoline. When the gasoline burns, 168 kg of oxygen is consumed, and carbon dioxide and water are produced. What is the total combined mass of carbon dioxide and water that is produced?

Textbook Question

Two samples of carbon tetrachloride are decomposed into their constituent elements. One sample produces 38.9 g of carbon and 448 g of chlorine, and the other sample produces 14.8 g of carbon and 134 g of chlorine. Are these results consistent with the law of definite proportions? Explain your answer.

Upon decomposition, one sample of magnesium fluoride produces 1.65 kg of magnesium and 2.57 kg of fluorine. A second sample produces 2.72 kg of magnesium. How much fluorine (in grams) does the second sample produce?

Textbook Question

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.

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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