The Atomic Mass Of Nitrogen Is 14.01, Hydrogen Is 1.01, Sulfur Is 32.07, And Oxygen Is 16.00. What Is The Molar Mass Of Ammonium Sulfate $\[\left[(NH_4)_2SO_4\right]?\\]A. $\[63.09 \, \text{g}\\] B. $\[84.17 \, \text{g}\\]

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Introduction

In chemistry, the molar mass of a compound is a crucial parameter that helps us understand its properties and behavior. The molar mass is the mass of one mole of a substance, expressed in units of grams per mole (g/mol). In this article, we will calculate the molar mass of ammonium sulfate, a compound with the chemical formula (NH4)2SO4.

Understanding the Atomic Mass

Before we dive into the calculation, let's review the atomic masses of the elements involved:

  • Nitrogen (N) has an atomic mass of 14.01 g/mol
  • Hydrogen (H) has an atomic mass of 1.01 g/mol
  • Sulfur (S) has an atomic mass of 32.07 g/mol
  • Oxygen (O) has an atomic mass of 16.00 g/mol

Calculating the Molar Mass of Ammonium Sulfate

To calculate the molar mass of ammonium sulfate, we need to sum the atomic masses of all the atoms in the compound. The formula (NH4)2SO4 indicates that there are two ammonium ions (NH4+) and one sulfate ion (SO42-).

Let's break down the calculation:

  • Ammonium ions (NH4+): Each ammonium ion consists of one nitrogen atom, four hydrogen atoms, and four oxygen atoms. The atomic masses of these atoms are:
    • Nitrogen (N): 14.01 g/mol
    • Hydrogen (H): 1.01 g/mol (4 times)
    • Oxygen (O): 16.00 g/mol (4 times)
  • Sulfate ion (SO42-): The sulfate ion consists of one sulfur atom and four oxygen atoms. The atomic masses of these atoms are:
    • Sulfur (S): 32.07 g/mol
    • Oxygen (O): 16.00 g/mol (4 times)

Step-by-Step Calculation

Now, let's calculate the molar mass of ammonium sulfate step by step:

  1. Ammonium ions (NH4+):
    • Nitrogen (N): 14.01 g/mol
    • Hydrogen (H): 4 x 1.01 g/mol = 4.04 g/mol
    • Oxygen (O): 4 x 16.00 g/mol = 64.00 g/mol
    • Total mass of one ammonium ion: 14.01 + 4.04 + 64.00 = 82.05 g/mol
    • Since there are two ammonium ions, the total mass of both ions is: 2 x 82.05 = 164.10 g/mol
  2. Sulfate ion (SO42-):
    • Sulfur (S): 32.07 g/mol
    • Oxygen (O): 4 x 16.00 g/mol = 64.00 g/mol
    • Total mass of the sulfate ion: 32.07 + 64.00 = 96.07 g/mol
  3. Total molar mass of ammonium sulfate:
    • Total mass of both ammonium ions: 164.10 g/mol
    • Total mass of the sulfate ion: 96.07 g/mol
    • Total molar mass of ammonium sulfate: 164.10 + 96.07 = 260.17 g/mol

Conclusion

The molar mass of ammonium sulfate is 260.17 g/mol. This value is not among the options provided in the question. However, we can see that the closest option is 84.17 g/mol, which is significantly lower than the actual molar mass. This discrepancy highlights the importance of accurate calculations in chemistry.

Discussion

The calculation of the molar mass of ammonium sulfate is a straightforward process that involves summing the atomic masses of all the atoms in the compound. However, the result may vary depending on the accuracy of the atomic masses used. In this article, we used the standard atomic masses of the elements involved.

The molar mass of a compound is a fundamental property that has numerous applications in chemistry and other fields. Understanding how to calculate the molar mass of a compound is essential for solving problems and making predictions about its behavior.

References

  • CRC Handbook of Chemistry and Physics (2022)
  • IUPAC Standard Atomic Weights (2022)

Appendix

The following table summarizes the atomic masses of the elements involved in the calculation:

Element Atomic Mass (g/mol)
Nitrogen (N) 14.01
Hydrogen (H) 1.01
Sulfur (S) 32.07
Oxygen (O) 16.00

Q: What is the molar mass of ammonium sulfate?

A: The molar mass of ammonium sulfate is 260.17 g/mol.

Q: Why is the molar mass of ammonium sulfate important?

A: The molar mass of a compound is a fundamental property that has numerous applications in chemistry and other fields. Understanding how to calculate the molar mass of a compound is essential for solving problems and making predictions about its behavior.

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

A: To calculate the molar mass of a compound, you need to sum the atomic masses of all the atoms in the compound. You can use the standard atomic masses of the elements involved, which can be found in reference books or online resources.

Q: What are the atomic masses of the elements involved in the calculation of the molar mass of ammonium sulfate?

A: The atomic masses of the elements involved in the calculation of the molar mass of ammonium sulfate are:

  • Nitrogen (N): 14.01 g/mol
  • Hydrogen (H): 1.01 g/mol
  • Sulfur (S): 32.07 g/mol
  • Oxygen (O): 16.00 g/mol

Q: Why is the calculation of the molar mass of a compound important in chemistry?

A: The calculation of the molar mass of a compound is important in chemistry because it helps us understand the properties and behavior of the compound. For example, the molar mass of a compound can be used to determine its density, boiling point, and melting point.

Q: Can I use the molar mass of a compound to determine its chemical formula?

A: No, the molar mass of a compound cannot be used to determine its chemical formula. The chemical formula of a compound is determined by the number and type of atoms present in the compound, not by its molar mass.

Q: How do I determine the chemical formula of a compound?

A: To determine the chemical formula of a compound, you need to analyze the compound's composition and identify the number and type of atoms present. This can be done using various techniques, such as spectroscopy, chromatography, and mass spectrometry.

Q: What are some common applications of the molar mass of a compound?

A: The molar mass of a compound has numerous applications in chemistry and other fields, including:

  • Determining the density of a compound
  • Calculating the boiling point and melting point of a compound
  • Understanding the chemical reactivity of a compound
  • Determining the chemical formula of a compound
  • Calculating the amount of a compound required for a reaction

Q: Where can I find more information about the molar mass of a compound?

A: You can find more information about the molar mass of a compound in reference books, online resources, and scientific journals. Some popular resources include the CRC Handbook of Chemistry and Physics, the IUPAC Standard Atomic Weights, and the National Institute of Standards and Technology (NIST) WebBook.

Q: What are some common mistakes to avoid when calculating the molar mass of a compound?

A: Some common mistakes to avoid when calculating the molar mass of a compound include:

  • Using incorrect atomic masses
  • Failing to account for the number of atoms present in the compound
  • Not using the correct units (e.g., g/mol)
  • Not rounding the result to the correct number of significant figures

Q: How can I practice calculating the molar mass of a compound?

A: You can practice calculating the molar mass of a compound by working through examples and exercises in your textbook or online resources. You can also try calculating the molar mass of different compounds and comparing your results to the actual values.