   Chapter 9, Problem 17CR ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
94 views

# A compound was analyzed and was found to have the following percent composition by mass: sodium, 43.38%; carbon, 11.33%; oxygen, 45.29%. Determine the empirical formula of the compound.

Interpretation Introduction

Interpretation:

The empirical formula of the compound having 43.38% of sodium, 11.33% of carbon and 45.29% of oxygen should be determined.

Concept Introduction:

The formula of the chemical compound in which atoms are present in simple positive integer ratio is said to be empirical formula. This formula only gives the proportions of the elements but doesn’t give the actual number of atoms present in the compound.

Explanation

First, calculate how many grams of each element present in 100 g of compound.

Compound has 43.38% of sodium implies there is 43.38 g of sodium per 100.00 g of compound. Similarly, compound has 11.33% of carbon and 45.29% of oxygen implies there is 11.33 g of carbon per 100.00 g of compound and 45.29 g of oxygen per 100.00 g of compound.

Calculate the number of moles of sodium, carbon and oxygen:

Number of moles of sodium = Given massMolar mass

Molar mass of sodium = 22.99 g/mol

Number of moles of sodium = 43.38 g22.99 g/mol=1.886 mol

Number of moles of carbon = Given massMolar mass

Molar mass of carbon = 12.01 g/mol

Number of moles of carbon =  11.33 g12.01 g/mol=0.94 mol

Number of moles of oxygen = Given massMolar mass

Molar mass of oxygen = 16

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