When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of and . in a certain experiment, 20.00 g iron metal was reacted with 11.53 g oxygen gas. after the experiment, the iron was totally consumed, and 3.78 g oxygen gas remained. calculate the amounts of and formed in this experiment?

Given:

initial mass of Fe = 20.0 g 
initial mass of oxygen gas = 11.53 g 
mass of oxygen remained = 3.78 g 

Solution:
The chemical reaction is expressed as:

4Fe + 3O2 --> 2Fe2O3 

We first calculate the oxygen that is used in the reaction,
Mass oxygen used = 11.53 g - 3.78 g = 7.75 g O2
Moles O2 = 7.75 g O2 ( 1 mol / 32 g ) = 0.2422 moles O2
Moles Fe2O3 produced = 0.2422 moles O2 ( 2 mol Fe2O3 / 3 moles O2 ) = 0.1615 mol Fe2O3
Mass Fe2O3 produced = 0.1615 mol Fe2O3 ( 159.7 g / 1 mol ) = 25.79 g Fe2O3

Therefore, the mass of ferrous oxide produced would be 45.79 g Fe2O3.

Atomicity occurs to prevent updates of the database occurring only partially, which can cause greater problems than rejecting the whole series outright.some are monatomic, diatomic, triatomic etc because it shows the number of atoms. for example, monatomic means it contains only one atom.