Molar Mass of Silver Nitrate

Oct 13, 2025 by miodeya.com 46 views

Understanding the Problem

To solve this problem, we need to calculate the number of molecules in 65 g of silver nitrate (AgNO3). This requires us to use the concept of molar mass and Avogadro's number.

Molar Mass of Silver Nitrate

The molar mass of silver nitrate (AgNO3) can be calculated by adding the atomic masses of silver (Ag), nitrogen (N), and three oxygen atoms (O). The atomic masses are:

Silver (Ag): 107.868 g/mol
Nitrogen (N): 14.007 g/mol
Oxygen (O): 16.00 g/mol

The molar mass of silver nitrate is:

107.868 g/mol (Ag) + 14.007 g/mol (N) + 3(16.00 g/mol) (O) = 169.87 g/mol

Calculating the Number of Moles

To calculate the number of moles of silver nitrate in 65 g, we can use the formula:

Number of moles = Mass of substance / Molar mass

Number of moles = 65 g / 169.87 g/mol = 0.383 mol

Calculating the Number of Molecules

To calculate the number of molecules, we can use Avogadro's number (6.022 x 10^23 molecules/mol). We can multiply the number of moles by Avogadro's number to get the number of molecules:

Number of molecules = Number of moles x Avogadro's number = 0.383 mol x 6.022 x 10^23 molecules/mol = 2.3046 x 10^23 molecules

Conclusion

Therefore, the correct answer is B. 2.3046 x 10^23.

Understanding the Significance

This problem demonstrates the importance of understanding the concept of molar mass and Avogadro's number in chemistry. By calculating the number of moles and molecules, we can gain a deeper understanding of the properties and behavior of substances at the molecular level.

Real-World Applications

This concept is crucial in various fields, such as:

Chemical engineering: Understanding the number of molecules in a given mass of a substance is essential in designing and optimizing chemical processes.
Materials science: The number of molecules in a material can affect its properties, such as strength, conductivity, and optical properties.
Pharmaceuticals: The number of molecules in a drug can impact its efficacy, stability, and bioavailability.

Common Mistakes

When solving this problem, it's essential to:

Use the correct molar mass: Make sure to use the correct molar mass of silver nitrate.
Calculate the number of moles correctly: Use the formula: Number of moles = Mass of substance / Molar mass.
Use Avogadro's number correctly: Multiply the number of moles by Avogadro's number to get the number of molecules.

Q: What is the molar mass of silver nitrate (AgNO3)?

A: The molar mass of silver nitrate (AgNO3) is 169.87 g/mol, which is calculated by adding the atomic masses of silver (Ag), nitrogen (N), and three oxygen atoms (O).

Q: How do I calculate the number of moles of silver nitrate in a given mass?

A: To calculate the number of moles of silver nitrate in a given mass, you can use the formula:

Number of moles = Mass of substance / Molar mass

For example, if you have 65 g of silver nitrate, the number of moles would be:

Number of moles = 65 g / 169.87 g/mol = 0.383 mol

Q: What is Avogadro's number, and how is it used to calculate the number of molecules?

A: Avogadro's number is 6.022 x 10^23 molecules/mol, which is a constant that represents the number of molecules in one mole of a substance. To calculate the number of molecules, you can multiply the number of moles by Avogadro's number:

Number of molecules = Number of moles x Avogadro's number = 0.383 mol x 6.022 x 10^23 molecules/mol = 2.3046 x 10^23 molecules

Q: What are some common mistakes to avoid when calculating the number of molecules?

A: Some common mistakes to avoid when calculating the number of molecules include:

Using the wrong molar mass of silver nitrate
Calculating the number of moles incorrectly
Using Avogadro's number incorrectly
Not converting units correctly

Q: Why is it important to understand the concept of molar mass and Avogadro's number?

A: Understanding the concept of molar mass and Avogadro's number is crucial in various fields, such as:

Chemical engineering: Understanding the number of molecules in a given mass of a substance is essential in designing and optimizing chemical processes.
Materials science: The number of molecules in a material can affect its properties, such as strength, conductivity, and optical properties.
Pharmaceuticals: The number of molecules in a drug can impact its efficacy, stability, and bioavailability.

Q: Can I use this concept to calculate the number of molecules in other substances?

A: Yes, you can use this concept to calculate the number of molecules in other substances by following the same steps:

Calculate the molar mass of the substance
Calculate the number of moles of the substance
Multiply the number of moles by Avogadro's number to get the number of molecules

Q: What are some real-world applications of this concept?

A: Some real-world applications of this concept include:

Designing and optimizing chemical processes
Developing new materials with specific properties
Creating new pharmaceuticals with improved efficacy and stability

Q: Can I use this concept to solve problems in other areas of chemistry?

A: Yes, you can use this concept to solve problems in other areas of chemistry, such as:

Stoichiometry: Understanding the concept of molar mass and Avogadro's number is essential in solving stoichiometry problems.
Thermodynamics: Understanding the concept of molar mass and Avogadro's number is crucial in understanding thermodynamic properties, such as entropy and free energy.

By understanding the concept of molar mass and Avogadro's number, you can solve a wide range of problems in chemistry and apply this knowledge to real-world applications.