Ch.2 - Atoms, Molecules, and Ions

Problem 13a1

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Chapter 2, Problem 13a1

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. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 17.60 g O

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Determine the mass of nitrogen given for the reaction, which is 30.82 grams.

Identify the mass of oxygen that reacts with the nitrogen in the first compound, which is 17.60 grams.

Calculate the mass ratio of oxygen to nitrogen for the compound by dividing the mass of oxygen by the mass of nitrogen.

Use the formula: Mass ratio = \( \frac{\text{mass of oxygen}}{\text{mass of nitrogen}} \).

Plug in the values: Mass ratio = \( \frac{17.60 \, \text{g}}{30.82 \, \text{g}} \) to find the mass of oxygen per gram of nitrogen in the first compound.

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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 calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how much oxygen reacts with a given mass of nitrogen in this scenario.

Mass Ratio

The mass ratio is a comparison of the mass of one substance to the mass of another substance in a chemical reaction. In this case, it refers to the mass of oxygen per gram of nitrogen. Calculating this ratio helps in understanding the composition of the compounds formed and is crucial for analyzing the different amounts of oxygen that react with a fixed mass of nitrogen.

Chemical Compounds

Chemical compounds are substances formed when two or more elements chemically bond together in fixed proportions. The different amounts of oxygen reacting with nitrogen in this question indicate the formation of various nitrogen-oxygen compounds, each with distinct properties. Recognizing how these compounds differ based on their elemental ratios is key to interpreting the results of the experiment.

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Chemical Properties

Related Practice

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed into its elements, yielding 0.273 g of carbon and 0.727 g of oxygen. If a sample of a different compound decomposes into 0.429 g of carbon and 0.571 g of oxygen, what is its ratio of the mass of O to C? (c) According to Dalton's atomic theory, what is the empirical formula of the second compound?

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Textbook Question

Sodium reacts with oxygen in air to form two compounds: sodium oxide and sodium peroxide. In forming sodium oxide, 23.0 g of sodium combines with 8.0 g of hydrogen. In forming sodium peroxide, 23.0 g of sodium combines with 16.0 g of oxygen. (a) What are the mass ratios of oxygen in the two compounds?

Textbook Question

Sodium reacts with oxygen in air to form two compounds: sodium oxide and sodium peroxide. In forming sodium oxide, 23.0 g of sodium combines with 8.0 g of hydrogen. In forming sodium peroxide, 23.0 g of sodium combines with 16.0 g of oxygen. (b) What fundamental law does this experiment demonstrate?

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Textbook Question

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. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. 30.82 g N and 88.00 g O