How Many Grams Of $H_2O$ Are Present In $6.022 \times 10^{23}$ Molecules Of $ H 2 O H_2O H 2 ​ O [/tex]?

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Introduction

In chemistry, understanding the relationship between the number of molecules and the mass of a substance is crucial for various calculations and applications. The given problem involves determining the mass of water (H2O) present in a specific number of molecules. To solve this, we need to use the concept of Avogadro's number and the molar mass of water.

Understanding Avogadro's Number

Avogadro's number is a fundamental constant in chemistry, representing the number of particles (atoms or molecules) in one mole of a substance. It is defined as 6.022 × 10^23 particles per mole. This number is used to relate the number of particles to the amount of substance in moles.

Calculating the Number of Moles

To find the number of moles of water present in 6.022 × 10^23 molecules, we can use Avogadro's number. Since Avogadro's number represents the number of particles in one mole, we can divide the given number of molecules by Avogadro's number to find the number of moles.

# Import necessary modules
import math

molecules = 6.022 * (1023)
avogadro_number = 6.022 * (1023)



moles = molecules / avogadro_number


print(moles)

Molar Mass of Water

The molar mass of water (H2O) is the sum of the atomic masses of its constituent atoms: hydrogen (H) and oxygen (O). The atomic mass of hydrogen is approximately 1 g/mol, and the atomic mass of oxygen is approximately 16 g/mol. Therefore, the molar mass of water is 18 g/mol (2 × 1 + 16).

Calculating the Mass of Water

Now that we have the number of moles and the molar mass of water, we can calculate the mass of water present in 6.022 × 10^23 molecules. We can use the formula: mass = number of moles × molar mass.

# Define variables
moles = 1  # From previous calculation
molar_mass = 18  # g/mol


mass = moles * molar_mass


print(mass)

Conclusion

In this article, we have calculated the mass of water present in 6.022 × 10^23 molecules of H2O. We first used Avogadro's number to find the number of moles, and then we used the molar mass of water to calculate the mass. The result shows that the mass of water present in 6.022 × 10^23 molecules is 18 g.

Frequently Asked Questions

  • What is Avogadro's number?
    • Avogadro's number is a fundamental constant in chemistry, representing the number of particles (atoms or molecules) in one mole of a substance.
  • How do I calculate the number of moles from a given number of molecules?
    • You can divide the given number of molecules by Avogadro's number to find the number of moles.
  • What is the molar mass of water?
    • The molar mass of water is 18 g/mol, which is the sum of the atomic masses of its constituent atoms: hydrogen and oxygen.

References

Further Reading

  • Chemistry: The Central Science. (2019). 14th ed. Pearson Education.
  • Atkins, P. W., & De Paula, J. (2018). Physical Chemistry. 10th ed. Oxford University Press.

Introduction

In our previous article, we explored the concept of Avogadro's number and its application in calculating the mass of water present in a specific number of molecules. In this article, we will address some frequently asked questions related to this topic and provide additional insights to help you better understand the relationship between molecules and mass.

Q&A

Q: What is Avogadro's number, and why is it important in chemistry?

A: Avogadro's number is a fundamental constant in chemistry, representing the number of particles (atoms or molecules) in one mole of a substance. It is defined as 6.022 × 10^23 particles per mole. Avogadro's number is essential in chemistry because it allows us to relate the number of particles to the amount of substance in moles.

Q: How do I calculate the number of moles from a given number of molecules?

A: To calculate the number of moles from a given number of molecules, you can divide the given number of molecules by Avogadro's number. This will give you the number of moles of the substance.

Q: What is the molar mass of water, and how is it calculated?

A: The molar mass of water is 18 g/mol, which is the sum of the atomic masses of its constituent atoms: hydrogen and oxygen. The atomic mass of hydrogen is approximately 1 g/mol, and the atomic mass of oxygen is approximately 16 g/mol.

Q: How do I calculate the mass of a substance from its number of molecules?

A: To calculate the mass of a substance from its number of molecules, you need to follow these steps:

  1. Calculate the number of moles from the given number of molecules using Avogadro's number.
  2. Multiply the number of moles by the molar mass of the substance to get the mass.

Q: What is the difference between the number of molecules and the number of moles?

A: The number of molecules represents the actual number of particles in a substance, while the number of moles represents the amount of substance in a unit called a mole. Avogadro's number allows us to relate the number of molecules to the number of moles.

Q: Can I use Avogadro's number to calculate the mass of any substance?

A: Yes, you can use Avogadro's number to calculate the mass of any substance, as long as you know the molar mass of the substance.

Q: What are some real-world applications of Avogadro's number?

A: Avogadro's number has numerous real-world applications in chemistry, including:

  • Calculating the mass of substances in chemical reactions
  • Determining the amount of substance in a sample
  • Understanding the properties of materials at the molecular level

Conclusion

In this article, we have addressed some frequently asked questions related to the relationship between molecules and mass. We have also provided additional insights to help you better understand the concept of Avogadro's number and its application in chemistry. By mastering this concept, you will be able to calculate the mass of substances with ease and apply it to real-world problems.

Frequently Asked Questions

  • What is Avogadro's number, and why is it important in chemistry?
  • How do I calculate the number of moles from a given number of molecules?
  • What is the molar mass of water, and how is it calculated?
  • How do I calculate the mass of a substance from its number of molecules?
  • What is the difference between the number of molecules and the number of moles?

References

Further Reading

  • Chemistry: The Central Science. (2019). 14th ed. Pearson Education.
  • Atkins, P. W., & De Paula, J. (2018). Physical Chemistry. 10th ed. Oxford University Press.