Chapter 3, Problem 166CWP

### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404

Chapter
Section

### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404
Textbook Problem

# A compound with molar mass 180.1 g/mol has the following composition by mass: C 40.0% H 6.70% O 53.3% Determine the empirical and molecular formulas of the compound.

Interpretation Introduction

Interpretation: The empirical and molecular formula for the compound of given molar mass is to be stated.

Concept introduction: The molecular formula of an element defines the total number of atoms present in a molecule and the empirical formula of an element is defined as the simplest formula that express the percentage composition of the element.

To determine: The empirical and molecular formula of the given compound.

Explanation

Explanation

Given

The molar mass of the compound is 180.1Â g/mol .

The mass of the compound is considered to be 100Â g .

The mass percent of carbon is 40.0% .

The mass percent of hydrogen is 6.70% .

The mass percent of oxygen is 53.3% .

Therefore, the mass of the compound is considered to be 100Â g .

So, the mass of carbon is 40.0Â g .

The mass of hydrogen is 6.70Â g .

The mass of oxygen is 53.3Â g .

The molar mass of carbon is 12â€‰g/mol .

The molar mass of hydrogen is 1â€‰g/mol .

The molar mass of oxygen is 16Â g/mol .

The number of moles is calculated by the formula,

Numberâ€‰ofâ€‰moles=Givenâ€‰massMolarâ€‰mass

Substitute the value of the given mass and the molar mass, to calculate the number of moles of carbon and hydrogen, in the above equation.

For carbon,

Numberâ€‰ofâ€‰molesâ€‰ofâ€‰carbon=Givenâ€‰massMolarâ€‰mass=40â€‰g12â€‰g/mol=3.33â€‰mol

For hydrogen,

Numberâ€‰ofâ€‰molesâ€‰ofâ€‰hydrogen=Givenâ€‰massMolarâ€‰mass=6.70â€‰g1â€‰g/mol=6.70â€‰mol

For oxygen,

Numberâ€‰ofâ€‰molesâ€‰ofâ€‰oxygen=Givenâ€‰massMolarâ€‰mass=53.3â€‰g16â€‰g/mol=3

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