   Chapter 3, Problem 179CP

Chapter
Section
Textbook Problem

Consider a gaseous binary compound with a molar mass of 62.09 g/mol. When 1.39 g of this compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound. Assume water is the only product that contains hydrogen.

Interpretation Introduction

Interpretation: The molar mass of a binary compound is given. The formula of the binary compound is to be calculated from the given data.

Concept introduction: The binary compounds are those compounds that are composed of two different elements.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The number of moles is the ratio of mass of compound to its molar mass.

To determine: The formula of the binary compound.

Explanation

Given

The molar mass of gaseous binary compound is 62.09g/mol.

Combustion of 1.39 g of given compound produces 1.21g of water (H2O).

The molar mass of water (H2O) is 18.015 g/mol.

Formula

The number of moles is calculated by using the formula,

Numberofmoles=GivenmassMolarmass (1)

Substitute the values of mass and molar mass of binary compound in above equation.

Numberofmoles=GivenmassMolarmass=1.39g62.09g/mol=0.0224mol

Since, it is assumed that water is the only product that contains hydrogen (H); therefore, amount of hydrogen in water is equal to amount of hydrogen present in 1.39 g of given compound.

Substitute the values of mass and molar mass of water in equation (1).

Numberofmoles=GivenmassMolarmass=1

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