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2. The mass percent of water in a hydrate of FESO4 is 45.35%. What is the formula of the hydrate?

2. The mass percent of water in a hydrate of FESO4 is 45.35%. What is the formula of the hydrate?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question:** The mass percent of water in a hydrate of FeSO₄ is 45.35%. What is the formula of the hydrate? --- **Explanation:** This question asks you to determine the formula of a hydrate based on the given mass percent of water in the compound. A hydrate is a compound that contains water molecules within its crystal structure, and the formula is typically written as \( FeSO₄ \cdot xH₂O \), where \( x \) represents the number of water molecules per formula unit of FeSO₄. To solve this problem, you would: 1. **Calculate the Molar Masses:** - Determine the molar mass of FeSO₄. - Determine the molar mass of H₂O. 2. **Calculate the Amount of Water:** - Use the given mass percent to find out how many grams of water corresponds to the 100 grams of the hydrate. 3. **Determine the Number of Water Molecules (x):** - Use the molar masses and given percentages to calculate the value of \( x \), which tells you how many water molecules are associated with each formula unit of FeSO₄ in the hydrate. This analysis helps determine the precise stoichiometry of the hydrate in question.
Transcribed Image Text:**Question:** The mass percent of water in a hydrate of FeSO₄ is 45.35%. What is the formula of the hydrate? --- **Explanation:** This question asks you to determine the formula of a hydrate based on the given mass percent of water in the compound. A hydrate is a compound that contains water molecules within its crystal structure, and the formula is typically written as \( FeSO₄ \cdot xH₂O \), where \( x \) represents the number of water molecules per formula unit of FeSO₄. To solve this problem, you would: 1. **Calculate the Molar Masses:** - Determine the molar mass of FeSO₄. - Determine the molar mass of H₂O. 2. **Calculate the Amount of Water:** - Use the given mass percent to find out how many grams of water corresponds to the 100 grams of the hydrate. 3. **Determine the Number of Water Molecules (x):** - Use the molar masses and given percentages to calculate the value of \( x \), which tells you how many water molecules are associated with each formula unit of FeSO₄ in the hydrate. This analysis helps determine the precise stoichiometry of the hydrate in question.
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