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Home » Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.
Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.
CBSE | Chemistry | Class 11 | NCERT | Some Basic Concepts of Chemistry
Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.

Percentage of Fe by mass = 69.9% [As said previously]

By mass, 30.1 percent of O2 is present. [As said previously]

Relative moles of Fe in iron oxide:

= (69.9)x(55.85}/

= 1.25

Relative moles of O in iron oxide:

= (30.1)(16.00)/

= 1.88

Simplest molar ratio of Fe to O:

= 1.25: 1.88

= 1: 1.5

approx 2: 3

As a result, the empirical formula for iron oxide is Fe2 O3.

 

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