   # To find the formula of a compound composed of iron and carbon monoxide, Fe x (CO) yx , the compound is burned in pure oxygen to give Fe 2 O 3 and CO 2 . if you burn 1.959 g of Fe x (CO) y and obtain 0.799 g of Fe 2 O 3 and 2.200 g of CO 2 , what is the empirical formula of Fe x (CO) y ? ### 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 4, Problem 38PS
Textbook Problem
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## To find the formula of a compound composed of iron and carbon monoxide, Fex(CO)yx, the compound is burned in pure oxygen to give Fe2O3 and CO2. if you burn 1.959 g of Fex(CO)y and obtain 0.799 g of Fe2O3 and 2.200 g of CO2, what is the empirical formula of Fex(CO)y?

Interpretation Introduction

Interpretation:

The empirical formula of Fex(CO)y should be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Amount of substance (in mole) can be calculated by using the following equation,

Numberofmole=GivenmassofthesubstanceMolarmass

• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).

### Explanation of Solution

When 1.959g of given sample is burned in oxygen, 0.799g of Fe2O3 and 2.200gofCO2 will obtain.

The reaction can be represented as

Fex(CO)yFe2O3+CO2

From the given masses the amount of Fe2O3 andCO2 can be calculated.

Thus, amount of Fe2O3 andCO2 isolated from the combustion of given compound are,

0.799gFe2O3×1molFe2O3159.69gFe2O3=0.0050molFe2O32.200gCO2×1molCO244.010gCO2=0.0499molCO2

For every mole of Fe2O3 isolated, 2molofFe must have been present in the given compound.

So,

0

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