Understanding the Atomic Mass of Phosphorus

Oct 13, 2025 by orovajewels.com 111 views

The periodic table is a powerful tool in chemistry that allows us to identify the elements, their properties, and their relationships with each other. One of the key pieces of information that the periodic table provides is the atomic mass of each element. In this article, we will use the periodic table to determine the number of atoms of phosphorus (P) in a sample that has a mass of 172.90 g.

Understanding the Atomic Mass of Phosphorus

The atomic mass of phosphorus is 30.97 g/mol. This means that one mole of phosphorus atoms has a mass of 30.97 g. To determine the number of atoms of phosphorus in a sample, we need to know the mass of the sample and the atomic mass of phosphorus.

Calculating the Number of Moles of Phosphorus

To calculate the number of moles of phosphorus in the sample, we can use the following formula:

moles = mass / atomic mass

In this case, the mass of the sample is 172.90 g, and the atomic mass of phosphorus is 30.97 g/mol. Plugging these values into the formula, we get:

moles = 172.90 g / 30.97 g/mol = 5.59 mol

Calculating the Number of Atoms of Phosphorus

Now that we know the number of moles of phosphorus, we can calculate the number of atoms of phosphorus using Avogadro's number. Avogadro's number is 6.022 x 10^23 atoms/mol. This means that one mole of atoms contains 6.022 x 10^23 atoms.

To calculate the number of atoms of phosphorus, we can multiply the number of moles of phosphorus by Avogadro's number:

atoms = moles x Avogadro's number = 5.59 mol x 6.022 x 10^23 atoms/mol = 3.36 x 10^24 atoms

Conclusion

In this article, we used the periodic table to determine the number of atoms of phosphorus in a sample that has a mass of 172.90 g. We first calculated the number of moles of phosphorus using the mass of the sample and the atomic mass of phosphorus. Then, we calculated the number of atoms of phosphorus using Avogadro's number. The result is 3.36 x 10^24 atoms.

Answer

The correct answer is C. 3.36 x 10^24 atoms.

Why is this important?

Understanding the number of atoms in a sample is crucial in chemistry. It allows us to determine the amount of substance present, which is essential in many chemical reactions. Additionally, knowing the number of atoms in a sample can help us understand the properties of the substance, such as its reactivity and its behavior in different conditions.

Real-world applications

The ability to determine the number of atoms in a sample has many real-world applications. For example, in the field of materials science, knowing the number of atoms in a material can help us understand its properties and behavior. This can be useful in designing new materials with specific properties, such as strength, conductivity, or optical properties.

In the field of medicine, understanding the number of atoms in a sample can help us develop new treatments and therapies. For example, knowing the number of atoms in a molecule can help us design new drugs that target specific receptors or enzymes.

Conclusion

In the previous article, we discussed how to determine the number of atoms of phosphorus in a sample using the periodic table. However, we understand that you may still have some questions about this topic. In this article, we will address some of the most frequently asked questions about determining the number of atoms of phosphorus.

Q: What is the atomic mass of phosphorus?

A: The atomic mass of phosphorus is 30.97 g/mol.

Q: How do I calculate the number of moles of phosphorus in a sample?

A: To calculate the number of moles of phosphorus in a sample, you can use the following formula:

moles = mass / atomic mass

For example, if the mass of the sample is 172.90 g, you can plug this value into the formula along with the atomic mass of phosphorus (30.97 g/mol) to get:

moles = 172.90 g / 30.97 g/mol = 5.59 mol

Q: What is Avogadro's number, and how do I use it to calculate the number of atoms of phosphorus?

A: Avogadro's number is 6.022 x 10^23 atoms/mol. This means that one mole of atoms contains 6.022 x 10^23 atoms. To calculate the number of atoms of phosphorus, you can multiply the number of moles of phosphorus by Avogadro's number:

atoms = moles x Avogadro's number = 5.59 mol x 6.022 x 10^23 atoms/mol = 3.36 x 10^24 atoms

Q: What are some real-world applications of determining the number of atoms of phosphorus?

A: Determining the number of atoms of phosphorus has many real-world applications, including:

Materials science: Knowing the number of atoms in a material can help us understand its properties and behavior.
Medicine: Understanding the number of atoms in a molecule can help us design new drugs that target specific receptors or enzymes.
Environmental science: Determining the number of atoms of phosphorus in a sample can help us understand the impact of phosphorus on the environment.

Q: What are some common mistakes to avoid when determining the number of atoms of phosphorus?

A: Some common mistakes to avoid when determining the number of atoms of phosphorus include:

Using the wrong atomic mass of phosphorus.
Failing to convert the mass of the sample from grams to moles.
Not using Avogadro's number to calculate the number of atoms of phosphorus.

Q: How can I practice determining the number of atoms of phosphorus?

A: You can practice determining the number of atoms of phosphorus by working through sample problems or using online resources such as calculators or interactive simulations. You can also try using different values for the mass of the sample and the atomic mass of phosphorus to see how the number of atoms of phosphorus changes.

Conclusion

In conclusion, determining the number of atoms of phosphorus is an important concept in chemistry that has many real-world applications. By understanding the atomic mass of phosphorus and Avogadro's number, you can calculate the number of atoms of phosphorus in a sample. We hope that this article has helped to answer some of your questions about determining the number of atoms of phosphorus.