What Is The Empirical Formula For A Compound If A Sample Contains 1.0 G Of S And 1.5 G Of O?A. $SO$ B. $SO_3$ C. $S_2O_2$ D. $S_2O_3$

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Introduction

In chemistry, determining the empirical formula of a compound is crucial in understanding its composition and properties. The empirical formula represents the simplest whole-number ratio of atoms of each element present in the compound. In this article, we will explore how to find the empirical formula of a compound given the mass of its constituent elements.

Understanding the Empirical Formula

The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. It is usually expressed as a chemical formula, with the subscripts representing the number of atoms of each element. For example, the empirical formula of water is H2O, indicating that one molecule of water contains two hydrogen atoms and one oxygen atom.

Calculating the Number of Moles of Each Element

To determine the empirical formula of a compound, we need to calculate the number of moles of each element present in the sample. We can do this by dividing the mass of each element by its atomic mass.

Calculating the Number of Moles of Sulfur (S)

The atomic mass of sulfur (S) is 32.07 g/mol. To calculate the number of moles of sulfur, we divide the mass of sulfur (1.0 g) by its atomic mass (32.07 g/mol).

moles_S = mass_S / atomic_mass_S
moles_S = 1.0 g / 32.07 g/mol
moles_S = 0.0312 mol

Calculating the Number of Moles of Oxygen (O)

The atomic mass of oxygen (O) is 16.00 g/mol. To calculate the number of moles of oxygen, we divide the mass of oxygen (1.5 g) by its atomic mass (16.00 g/mol).

moles_O = mass_O / atomic_mass_O
moles_O = 1.5 g / 16.00 g/mol
moles_O = 0.0938 mol

Determining the Simplest Whole-Number Ratio

To determine the empirical formula, we need to find the simplest whole-number ratio of atoms of each element present in the compound. We can do this by dividing the number of moles of each element by the smallest number of moles.

Finding the Smallest Number of Moles

The smallest number of moles is 0.0312 mol (moles of S).

Determining the Ratio of Sulfur to Oxygen

To determine the ratio of sulfur to oxygen, we divide the number of moles of each element by the smallest number of moles (0.0312 mol).

ratio_S = moles_S / smallest_moles
ratio_S = 0.0312 mol / 0.0312 mol
ratio_S = 1

ratio_O = moles_O / smallest_moles
ratio_O = 0.0938 mol / 0.0312 mol
ratio_O = 3

Writing the Empirical Formula

Based on the ratio of sulfur to oxygen (1:3), we can write the empirical formula of the compound as SO3.

Conclusion

In conclusion, the empirical formula of a compound can be determined by calculating the number of moles of each element present in the sample, finding the simplest whole-number ratio of atoms of each element, and writing the empirical formula based on the ratio. In this article, we have demonstrated how to find the empirical formula of a compound given the mass of its constituent elements.

Frequently Asked Questions

  • What is the empirical formula of a compound?
  • How do I calculate the number of moles of each element present in a sample?
  • How do I determine the simplest whole-number ratio of atoms of each element present in a compound?
  • What is the significance of the empirical formula in chemistry?

References

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling
  • Chemistry: The Central Science, by Theodore L. Brown

Further Reading

  • Empirical Formula: Definition, Calculation, and Examples
  • Determining the Empirical Formula of a Compound
  • Calculating the Number of Moles of Each Element Present in a Sample

Related Topics

  • Chemical Formulas and Equations
  • Stoichiometry and Chemical Reactions
  • Atomic Mass and Molar Mass

Keywords

  • Empirical Formula
  • Chemical Composition
  • Stoichiometry
  • Atomic Mass
  • Molar Mass
  • Chemical Reactions
  • Chemical Equations

Introduction

In our previous article, we discussed how to determine the empirical formula of a compound given the mass of its constituent elements. In this article, we will address some of the most frequently asked questions related to empirical formulas.

Q&A

Q: What is the empirical formula of a compound?

A: The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound.

Q: How do I calculate the number of moles of each element present in a sample?

A: To calculate the number of moles of each element, you need to divide the mass of each element by its atomic mass.

Q: How do I determine the simplest whole-number ratio of atoms of each element present in a compound?

A: To determine the simplest whole-number ratio, you need to divide the number of moles of each element by the smallest number of moles.

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

A: The empirical formula is significant in chemistry because it represents the simplest whole-number ratio of atoms of each element present in a compound, which is essential in understanding the properties and behavior of the compound.

Q: Can I use the empirical formula to determine the molecular formula of a compound?

A: Yes, you can use the empirical formula to determine the molecular formula of a compound. The molecular formula is a representation of the actual number of atoms of each element present in a molecule of the compound.

Q: How do I convert the empirical formula to the molecular formula?

A: To convert the empirical formula to the molecular formula, you need to multiply the subscripts of the empirical formula by a factor that represents the actual number of molecules of the compound.

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

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

Q: Can I use the empirical formula to determine the percentage composition of a compound?

A: Yes, you can use the empirical formula to determine the percentage composition of a compound. The percentage composition is the percentage by mass of each element present in the compound.

Q: How do I calculate the percentage composition of a compound using the empirical formula?

A: To calculate the percentage composition, you need to multiply the mass of each element by its percentage composition and then divide by the total mass of the compound.

Conclusion

In conclusion, the empirical formula is a crucial concept in chemistry that represents the simplest whole-number ratio of atoms of each element present in a compound. By understanding the empirical formula, you can determine the molecular formula, percentage composition, and other important properties of a compound.

Frequently Asked Questions

  • What is the empirical formula of a compound?
  • How do I calculate the number of moles of each element present in a sample?
  • How do I determine the simplest whole-number ratio of atoms of each element present in a compound?
  • What is the significance of the empirical formula in chemistry?
  • Can I use the empirical formula to determine the molecular formula of a compound?
  • How do I convert the empirical formula to the molecular formula?
  • What is the difference between the empirical formula and the molecular formula?
  • Can I use the empirical formula to determine the percentage composition of a compound?
  • How do I calculate the percentage composition of a compound using the empirical formula?

References

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling
  • Chemistry: The Central Science, by Theodore L. Brown

Further Reading

  • Empirical Formula: Definition, Calculation, and Examples
  • Determining the Empirical Formula of a Compound
  • Calculating the Number of Moles of Each Element Present in a Sample

Related Topics

  • Chemical Formulas and Equations
  • Stoichiometry and Chemical Reactions
  • Atomic Mass and Molar Mass

Keywords

  • Empirical Formula
  • Chemical Composition
  • Stoichiometry
  • Atomic Mass
  • Molar Mass
  • Chemical Reactions
  • Chemical Equations