   # Elemental sulfur (1.256 g) is combined with fluorine, to give a compound with the formula SF x , a very stable, colorless gas. If you have isolated 5.722 g of SF x , what is the value of x ? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 2, Problem 94PS
Textbook Problem
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## Elemental sulfur (1.256 g) is combined with fluorine, to give a compound with the formula SFx, a very stable, colorless gas. If you have isolated 5.722 g of SFx, what is the value of x?

Interpretation Introduction

Interpretation:

The value of x of the given product SFx is to be determined if 1.256g  of S is react with F2 to form the 5.722g of 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 of Solution

The mass of the product SFx is given that 5.722g

The mass of the sulfur (S) in product is given that 1.256g

So, the mass of fluorine in product is,

5.722g1.256g=4.466g

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

Numberofmoles=MassingramsMolarmass

Therefore,

The number of moles of S is,

Numberofmoles=1.256g32g/mol=0

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