Ch.2 - Atoms, Molecules, and Ions

Problem 14a3

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Chapter 2, Problem 14a3

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (a) Calculate the mass of fluorine per gram of iodine in Compound 3.

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Determine the mass of iodine and fluorine in Compound 3 from the data provided. For Compound 3, the mass of iodine is 9.41 grams and the mass of fluorine is 9.86 grams.

Set up the ratio of the mass of fluorine to the mass of iodine for Compound 3. This ratio can be calculated using the formula: \( \text{Ratio} = \frac{\text{Mass of Fluorine}}{\text{Mass of Iodine}} \).

Substitute the values into the formula: \( \text{Ratio} = \frac{9.86 \, \text{g}}{9.41 \, \text{g}} \).

Calculate the ratio by dividing the mass of fluorine by the mass of iodine. This will give you the mass of fluorine per gram of iodine in Compound 3.

The result from the calculation will provide the mass of fluorine per gram of iodine, which is a measure of how much fluorine is present relative to iodine in the compound.

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Key Concepts

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

Mass Ratio

The mass ratio is a comparison of the mass of one substance to the mass of another substance. In this context, it refers to the mass of fluorine relative to the mass of iodine in a compound. This ratio is crucial for understanding the composition of the compound and can be calculated by dividing the mass of fluorine by the mass of iodine.

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, which is essential for calculating mass ratios in compounds, as seen in the question.

Compound Composition

Compound composition refers to the specific elements and their proportions that make up a chemical compound. Understanding the composition is vital for analyzing the properties and behavior of the compound, including how to calculate the mass of one element per unit mass of another, as required in the problem.

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Matter Composition

Related Practice

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 35.20 g O

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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Textbook Question

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (a) Calculate the mass of fluorine per gram of iodine in Compound 1 and 2.

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Textbook Question

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (b) How do the numbers in part (a) support the atomic theory?

Which of the subatomic particles in an atom does not have a charge (and was therefore the last to be discovered)?

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