Empirical formula of an oxide

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In summary, the empirical formula of an oxide is the simplest whole number ratio of its constituent elements. It is determined through experimental analysis and can be the same as the molecular formula if the compound contains only one type of atom. The difference between empirical and molecular formula is that the former represents the simplest ratio while the latter represents the actual number of atoms in a molecule. The empirical formula of an oxide does not change with different experimental conditions.
  • #1
DarkPhoenix
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Homework Statement



An oxide of chlorine was analysed. A 0.366 g sample was found to contain 0.224 g of oxygen.

Calculate the empirical formula of this oxide.


The Attempt at a Solution



Cl = 0.366/35.5 = 0.10

O = 0.224/16 = 0.014
 
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  • #2
The mass of chlorine is not 0.366 it's 0.366-0.224=0.142
 
  • #3


The empirical formula of this oxide would be ClO. This can be determined by dividing the molar mass of each element by their respective masses in the compound. In this case, the ratio between chlorine and oxygen is approximately 1:1, indicating that the empirical formula is ClO. This result can also be supported by the fact that Cl and O are both nonmetals and typically form covalent compounds, which often have simpler empirical formulas. Further analysis and experimentation may be needed to determine the molecular formula of this oxide.
 

1. What is the empirical formula of an oxide?

The empirical formula of an oxide is the simplest whole number ratio of its constituent elements. It represents the relative number of atoms of each element present in the compound.

2. How is the empirical formula of an oxide determined?

The empirical formula of an oxide is determined through experimental analysis, specifically by finding the mass or percentage composition of each element in the compound.

3. Can the empirical formula of an oxide be the same as its molecular formula?

Yes, the empirical formula of an oxide can be the same as its molecular formula if the compound contains only one type of atom. However, if the compound contains more than one type of atom, the empirical formula will be different from the molecular formula.

4. What is the difference between empirical formula and molecular formula?

The empirical formula represents the simplest whole number ratio of elements in a compound, while the molecular formula represents the actual number of atoms of each element in a molecule of the compound.

5. Can the empirical formula of an oxide change with different experimental conditions?

No, the empirical formula of an oxide is a fixed ratio determined by the elemental composition of the compound and does not change with different experimental conditions.

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