   Chapter 2, Problem 93PS

Chapter
Section
Textbook Problem

A compound containing xenon and fluorine was prepared by shining sunlight on a mixture of Xe (0.526 g) and excess F2 gas. If you isolate 0.678 g of the new compound, what is its empirical formula?

Interpretation Introduction

Interpretation:

The empirical formula of the given product is to be determined if 0.526g of Xe is react with excess F2 to form the product.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Equation for number moles from mass and molar mass,

Numberofmoles=MassingramsMolarmass

Explanation

The mass of the product is given that 0.678g.

The mass of the xenon (Xe) in product is given that 0.526g.

So, the mass of fluorine in product is,

0.678g0.526g=0.152g

Equation for number of moles from mass and molar mass is,

Numberofmoles=MassingramsMolarmass

Therefore,

The number of moles of Xe is,

Numberofmoles=0.526g131.29g/mol=0

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