   Chapter 3, Problem 166CWP

Chapter
Section
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 180.1 g/mol .

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

So, the mass of carbon is 40.0 g .

The mass of hydrogen is 6.70 g .

The mass of oxygen is 53.3 g .

The molar mass of carbon is 12g/mol .

The molar mass of hydrogen is 1g/mol .

The molar mass of oxygen is 16 g/mol .

The number of moles is calculated by the formula,

Numberofmoles=GivenmassMolarmass

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,

Numberofmolesofcarbon=GivenmassMolarmass=40g12g/mol=3.33mol

For hydrogen,

Numberofmolesofhydrogen=GivenmassMolarmass=6.70g1g/mol=6.70mol

For oxygen,

Numberofmolesofoxygen=GivenmassMolarmass=53.3g16g/mol=3

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