Textbook Question
Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. a. methyl butyrate (component of apple taste and smell): C 58.80%, H 9.87%, O 31.33%
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Ch.3 - Molecules, Compounds & Chemical Equations
Chapter 3, Problem 93
What is the empirical formula of nitrogen chloride given that a 0.77 mg sample of nitrogen reacts with chlorine to form 6.61 mg of the chloride?
Verified step by step guidance1
Determine the mass of chlorine in the compound by subtracting the mass of nitrogen from the total mass of the nitrogen chloride: \(6.61 \text{ mg} - 0.77 \text{ mg}\).
Convert the mass of nitrogen (0.77 mg) to moles using the molar mass of nitrogen (14.01 g/mol).
Convert the mass of chlorine (calculated in step 1) to moles using the molar mass of chlorine (35.45 g/mol).
Calculate the mole ratio of nitrogen to chlorine by dividing the moles of each element by the smallest number of moles calculated in steps 2 and 3.
Use the mole ratio to determine the empirical formula by expressing the ratio as the smallest whole numbers.
Related Practice
Textbook Question
Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. b. vanillin (responsible for the taste and smell of vanilla): C 63.15%, H 5.30%, O 31.55%
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Textbook Question
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Textbook Question
A 45.2-mg sample of phosphorus reacts with selenium to form 131.6 mg of the selenide. Determine the empirical formula of phosphorus selenide.
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Textbook Question
From the given empirical formula and molar mass, find the molecular formula of each compound. a. C6H7N, 186.24 g/mol
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Textbook Question
From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. a. C4H9, 114.22 g/mol
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