how many atoms are in 15.2 grams of lithium

Lussy04

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22-01-2025

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Lithium, a silvery-white alkali metal, finds uses in batteries, ceramics, and even as a mood stabilizer in medicine. But have you ever wondered about the sheer number of atoms packed into even a small amount of this element? Let's calculate just how many atoms are present in 15.2 grams of lithium. This will involve a journey through the world of moles and Avogadro's number.

Understanding the Fundamentals: Moles and Avogadro's Number

Before we begin our calculation, let's grasp two essential concepts:

• Moles: A mole (mol) is a fundamental unit in chemistry, representing a specific number of particles (atoms, molecules, ions, etc.). This number is Avogadro's number.

• Avogadro's Number: This constant, approximately 6.022 x 10²³, signifies the number of entities (atoms in our case) in one mole of a substance.

Think of a mole as a convenient way to count incredibly large numbers of tiny particles, just as we use dozens to count eggs.

Calculating the Number of Lithium Atoms

Here's a step-by-step guide to determine the number of atoms in 15.2 grams of lithium:

Step 1: Find the molar mass of lithium.

The periodic table reveals lithium's atomic mass as approximately 6.94 grams per mole (g/mol). This means one mole of lithium weighs 6.94 grams.

Step 2: Convert grams to moles.

We have 15.2 grams of lithium. To convert this to moles, we use the molar mass:

Moles of lithium = (15.2 g) / (6.94 g/mol) ≈ 2.19 moles

Step 3: Use Avogadro's number to find the number of atoms.

Now, we'll use Avogadro's number to determine the number of atoms in 2.19 moles of lithium:

Number of atoms = (2.19 moles) * (6.022 x 10²³ atoms/mol) ≈ 1.32 x 10²⁴ atoms

Therefore, there are approximately 1.32 x 10²⁴ atoms in 15.2 grams of lithium. That's a truly massive number!

Further Exploration: The Significance of this Calculation

This seemingly simple calculation has broader implications. Understanding how to convert mass to the number of atoms is crucial in various fields:

• Chemistry: Stoichiometry relies heavily on this conversion to predict the quantities of reactants and products in chemical reactions.

• Materials Science: It's essential for understanding the properties of materials at the atomic level. The number of atoms influences everything from conductivity to strength.

• Nuclear Physics: Calculations involving radioactivity and nuclear reactions often involve converting mass to the number of atoms.

This seemingly simple calculation underscores the vastness of the atomic world and the power of chemistry's fundamental concepts. By understanding moles and Avogadro's number, we can bridge the gap between the macroscopic world of grams and the microscopic world of atoms.