how many atoms are in 2.9 moles of lithium

Lussy04

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22-01-2025

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Ever wondered about the sheer number of tiny particles making up even a small amount of matter? Let's delve into the fascinating world of atoms and moles, using lithium as our example. We'll calculate exactly how many atoms are present in 2.9 moles of lithium.

Understanding Moles and Avogadro's Number

Before we tackle the calculation, let's clarify some fundamental concepts. A **mole (mol)** is a fundamental unit in chemistry. It's a specific amount of a substance, containing a fixed number of particles (atoms, molecules, ions, etc.). That fixed number is **Avogadro's number**, approximately 6.022 x 10²³ particles per mole.

Think of it like a dozen: a dozen eggs always means 12 eggs. Similarly, a mole of any substance always contains Avogadro's number of particles.

Calculating the Number of Lithium Atoms

Now, let's calculate the number of atoms in 2.9 moles of lithium (Li). We'll use Avogadro's number as our conversion factor.

1. Start with the given amount: 2.9 moles of lithium
2. Use Avogadro's number as a conversion factor: 6.022 x 10²³ atoms/mol
3. Set up the calculation: 2.9 mol Li x (6.022 x 10²³ atoms Li / 1 mol Li)
4. Perform the calculation: The "mol Li" units cancel out, leaving us with the number of atoms. The result is approximately 1.746 x 10²⁴ atoms of lithium.

The Answer: A Huge Number!

Therefore, there are approximately 1.746 x 10²⁴ atoms in 2.9 moles of lithium. That's an incredibly large number – a testament to the incredibly small size of individual atoms!

Why is this Calculation Important?

Understanding how to convert moles to the number of atoms is crucial in various aspects of chemistry. It allows us to:

• Determine the number of reacting particles in chemical reactions.
• Calculate the mass of a substance given the number of moles or atoms.
• Relate macroscopic properties (like mass) to microscopic properties (like the number of atoms).

Further Exploration: Moles and Other Elements

The same principle applies to calculating the number of atoms in any given number of moles of any element. Just remember to use Avogadro's number as your conversion factor. Try calculating the number of atoms in different amounts of other elements to solidify your understanding!

For example, you could explore how many atoms are in 1 mole of gold (Au), or 0.5 moles of oxygen (O₂) – remembering that oxygen exists as a diatomic molecule (O₂), meaning you'd need to account for that in your calculation.

Understanding Avogadro's number and mole calculations is a cornerstone of chemistry. Mastering these concepts opens up a deeper understanding of the fundamental building blocks of matter.