Determining the Molecular Formula

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Introduction

In chemistry, empirical and molecular formulas are two essential concepts used to describe the composition of chemical compounds. An empirical formula represents the simplest whole-number ratio of atoms of each element present in a compound, while a molecular formula shows the actual number of atoms of each element in a molecule of the compound. In this article, we will explore whether C$_2$_H$_2$$ is an empirical formula and determine the molecular formula if a sample of the compound has a molar mass of 78.114 g/mol.

What is an Empirical Formula?

An empirical formula is a chemical formula that shows the simplest whole-number ratio of atoms of each element present in a compound. It is a way to represent the composition of a compound in a concise and simplified manner. Empirical formulas are often used to describe the composition of compounds that have a simple ratio of atoms of each element.

Is C$_2$_H$_2$$ an Empirical Formula?

To determine if C$_2$_H$_2$$ is an empirical formula, we need to check if it represents the simplest whole-number ratio of atoms of each element present in the compound. In this case, the formula C$_2$_H$_2$$ indicates that there are 2 carbon atoms and 2 hydrogen atoms present in the compound. This ratio is already in its simplest form, so C$_2$_H$_2$$ is indeed an empirical formula.

What is a Molecular Formula?

A molecular formula is a chemical formula that shows the actual number of atoms of each element present in a molecule of a compound. It is a more detailed representation of the composition of a compound than an empirical formula. Molecular formulas are often used to describe the composition of compounds that have a more complex ratio of atoms of each element.

Determining the Molecular Formula

To determine the molecular formula of a compound, we need to know its molar mass. The molar mass of a compound is the sum of the atomic masses of all the atoms present in a molecule of the compound. In this case, we are given that the molar mass of the compound is 78.114 g/mol.

Calculating the Molecular Formula

To calculate the molecular formula, we need to divide the molar mass of the compound by the molar mass of the empirical formula unit. The molar mass of the empirical formula unit C$_2$_H$_2$$ is 14.026 g/mol (2 x 12.011 g/mol for carbon + 2 x 1.008 g/mol for hydrogen).

Molecular mass of the compound = 78.114 g/mol Molar mass of the empirical formula unit = 14.026 g/mol

To calculate the molecular formula, we divide the molecular mass of the compound by the molar mass of the empirical formula unit:

Molecular formula = (Molecular mass of the compound / Molar mass of the empirical formula unit) x Empirical formula unit

Molecular formula = (78.114 g/mol / 14.026 g/mol) x C$_2$_H$_2$$

Molecular formula = 5.57 x C$_2$_H$_2$$

Since we cannot have a fraction of a molecule, we round up to the nearest whole number to get the molecular formula:

Molecular formula = 6C$_2$_H$_2$$

Conclusion

In conclusion, C$_2$_H$_2$$ is an empirical formula that represents the simplest whole-number ratio of atoms of each element present in the compound. To determine the molecular formula, we need to know the molar mass of the compound, which is 78.114 g/mol. By dividing the molar mass of the compound by the molar mass of the empirical formula unit, we get a multiplier of 5.57, which we round up to 6 to get the molecular formula 6C$_2$_H$_2$$. This molecular formula represents the actual number of atoms of each element present in a molecule of the compound.

References

IUPAC (1997). Nomenclature of Organic Chemistry. IUPAC Recommendations and Preferred Names 1993.
Lide, D. R. (2005). CRC Handbook of Chemistry and Physics. CRC Press.
Atkins, P. W., & De Paula, J. (2006). Physical Chemistry. Oxford University Press.
Frequently Asked Questions (FAQs) about Empirical and Molecular Formulas ====================================================================

Q: What is the difference between an empirical formula and a molecular formula?

A: An empirical formula represents the simplest whole-number ratio of atoms of each element present in a compound, while a molecular formula shows the actual number of atoms of each element in a molecule of the compound.

Q: How do I determine if a given formula is an empirical formula?

A: To determine if a given formula is an empirical formula, you need to check if it represents the simplest whole-number ratio of atoms of each element present in the compound. If the ratio is already in its simplest form, then it is an empirical formula.

Q: What is the significance of empirical formulas in chemistry?

A: Empirical formulas are significant in chemistry because they provide a concise and simplified way to represent the composition of a compound. They are often used to describe the composition of compounds that have a simple ratio of atoms of each element.

Q: How do I calculate the molecular formula of a compound?

A: To calculate the molecular formula of a compound, you need to know its molar mass. You then divide the molar mass of the compound by the molar mass of the empirical formula unit to get a multiplier. You then multiply the empirical formula unit by the multiplier to get the molecular formula.

Q: What is the relationship between empirical and molecular formulas?

A: The empirical formula is a factor of the molecular formula. The molecular formula is a multiple of the empirical formula.

Q: Can an empirical formula be a molecular formula?

A: Yes, an empirical formula can be a molecular formula if the ratio of atoms of each element present in the compound is already in its simplest form.

Q: How do I determine the molar mass of a compound?

A: To determine the molar mass of a compound, you need to know the atomic masses of all the atoms present in the compound. You then add up the atomic masses to get the molar mass.

Q: What is the significance of molecular formulas in chemistry?

A: Molecular formulas are significant in chemistry because they provide a more detailed representation of the composition of a compound than empirical formulas. They are often used to describe the composition of compounds that have a more complex ratio of atoms of each element.

Q: Can a molecular formula be an empirical formula?

A: No, a molecular formula cannot be an empirical formula because it shows the actual number of atoms of each element present in a molecule of the compound, while an empirical formula shows the simplest whole-number ratio of atoms of each element present in the compound.

Q: How do I convert an empirical formula to a molecular formula?

A: To convert an empirical formula to a molecular formula, you need to know the molar mass of the compound. You then divide the molar mass of the compound by the molar mass of the empirical formula unit to get a multiplier. You then multiply the empirical formula unit by the multiplier to get the molecular formula.

Q: What is the relationship between the empirical formula and the molecular formula?

A: The empirical formula is a factor of the molecular formula. The molecular formula is a multiple of the empirical formula.

Conclusion

In conclusion, empirical and molecular formulas are two essential concepts in chemistry that provide a concise and simplified way to represent the composition of a compound. Empirical formulas show the simplest whole-number ratio of atoms of each element present in a compound, while molecular formulas show the actual number of atoms of each element present in a molecule of the compound. By understanding the relationship between empirical and molecular formulas, you can determine the molecular formula of a compound and gain a deeper understanding of its composition.