   # In a reaction, 2.04 g of vanadium combined with 1.93 g of sulfur to give a pure compound. What is the empirical formula of the product? ### 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 138GQ
Textbook Problem
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## In a reaction, 2.04 g of vanadium combined with 1.93 g of sulfur to give a pure compound. What is the empirical formula of the product?

Interpretation Introduction

Interpretation: The empirical formula of the given compound should be determined by using the given data that 2.04g of Vanadium combined with 1.93g of Sulfur should be determined.

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

Given

In the compound two elements are there namely vanadium and sulfur.

The mass and molar mass of vanadium involved in the reaction is 2.04g and 50.94g/mol respectively.

The mass and molar mass of sulfur involved in the reaction is 1.93g and 32.065g/mol respectively.

Equation for number moles from mass and molar mass is,

Numberofmoles=MassingramsMolarmass

Therefore, the number of moles of vanadium is,

Numberofmoles=2.04g50.94g/mol=0.04004mol

The number of moles of sulfur is,

Numberofmoles=1.93g32.065g/mol=0

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