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ChemistryChemistry: An Atoms First Approach2nd Edition
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Vitamin A has a molar mass of 286.4 g/mol and a general molecular formula of C x H y E, where E is an unknown element. If vitamin A is 83.86% C and 10.56% H by mass, what is the molecular formula of vitamin A?

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 5, Problem 149AE
Textbook Problem
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Vitamin A has a molar mass of 286.4 g/mol and a general molecular formula of CxHyE, where E is an unknown element. If vitamin A is 83.86% C and 10.56% H by mass, what is the molecular formula of vitamin A?

Interpretation Introduction

Interpretation: The molar mass and the general molecular of vitamin A is given as CxHyE , where E is an unknown element. The molecular formula of the given vitamin A is to be stated.

Concept introduction: The number of moles of a substance is calculated by the formula,

Number of moles=Given mass of the substanceAtomic mass of the substance

To determine: The molecular formula of the given vitamin A.

Explanation of Solution

Given

The molar mass of vitamin A is 286.4 g/mol .

The mass percent of carbon is 83.86 % .

The mass percent of hydrogen is 10.56 % .

The mass of the given vitamin A is 286.4 g/mol .

Therefore, the mass of carbon =83.86 % of 286.4 g=(83.86100×286.4) g≈240 g

The mass of hydrogen =10.56 % of 286.4 g=(10.56100×286.4) g≈30 g

The mass of element E =(286.4−(Mass of carbon+Mass of hydrogen)) g=(286.4−240−30) g≈16 g

The calculated mass of the element E corresponds to 1 mol of oxygen (O) .

The atomic mass of carbon is 12 g/mol .

The atomic mass of hydrogen is 1 g/mol .

The atomic mass of oxygen is 16 g/mol

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