how many particle units are in 150 grams of salt

Lussy04

2 min read

·

24-01-2025

1

0

Share

Salt, or sodium chloride (NaCl), is a common household item. But have you ever wondered how many individual particles make up a seemingly small amount, like 150 grams? Let's explore the fascinating world of molar mass and Avogadro's number to find the answer.

Understanding Moles and Avogadro's Number

Before we dive into the calculation, we need to understand some fundamental chemistry concepts. A mole (mol) is a unit representing a specific number of particles, just like a dozen represents 12 items. This number is Avogadro's number, approximately 6.022 x 10²³ particles per mole.

Calculating the Number of Moles in 150 Grams of Salt

To figure out how many particle units are in 150 grams of salt, we first need to determine the number of moles present. This requires knowing the molar mass of NaCl.

• Finding the Molar Mass of NaCl: The molar mass is the mass of one mole of a substance. We find this by adding the atomic masses of sodium (Na) and chlorine (Cl) from the periodic table. Sodium's atomic mass is approximately 23 g/mol, and chlorine's is approximately 35.5 g/mol. Therefore, the molar mass of NaCl is 23 + 35.5 = 58.5 g/mol.

• Calculating Moles: Now, we can use the molar mass to calculate the number of moles in 150 grams of salt:

  Moles = (Mass of salt) / (Molar mass of NaCl) = 150 g / 58.5 g/mol ≈ 2.56 moles

Determining the Number of Particle Units

Now that we know there are approximately 2.56 moles of NaCl in 150 grams, we can use Avogadro's number to find the total number of particle units (formula units, in this case, since salt is an ionic compound):

Number of particle units = (Number of moles) x (Avogadro's number) = 2.56 mol x 6.022 x 10²³ units/mol ≈ 1.54 x 10²⁴ units

The Answer: Approximately 1.54 x 10²⁴ Particle Units

Therefore, there are approximately 1.54 x 10²⁴ formula units of sodium chloride (NaCl) in 150 grams of table salt. That's an incredibly large number! This calculation demonstrates the vastness of the scale at which atoms and molecules interact.

Further Considerations: Ionic vs. Covalent Compounds

It's important to note that this calculation assumes perfect crystalline salt. In reality, some impurities may be present. Also, the term "particle unit" is slightly nuanced. For ionic compounds like NaCl, the particles are formula units, representing the simplest ratio of ions in the crystal lattice. For covalent compounds, the particle units would be molecules.

This calculation highlights the importance of understanding molar mass and Avogadro's number in chemistry. These concepts are essential for various applications, from stoichiometry calculations to determining the concentration of solutions.