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To find how many molecules of water are present in a 5.65 mole sample of water, we can use Avogadro's number, which is \( 6.022 \times 10^{23} \) molecules per mole.

The calculation would be:

\[
\text{Number of molecules} = 5.65 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol}
\]

Now, performing the multiplication:

\[
\text{Number of molecules} = 3.4 \times 10^{24} \, \text{molecules}
\]

Thus, a 5.65 mole sample of water contains approximately \( 3.4 \times 10^{24} \) molecules.

Would you like a more detailed breakdown of the steps or further explanation? Here are some related questions:

1. How is Avogadro's number used in other chemical calculations?
2. What is the relationship between moles and mass in chemical reactions?
3. How do we convert between molecules and grams in a sample of a substance?
4. How does water's molar mass factor into calculations involving moles?
5. Can you explain the significance of Avogadro's constant in chemistry?

**Tip**: Always ensure you use proper significant figures based on the precision of your initial data (in this case, the mole value).

How many molecules of water are present in a 5.65 mole sample of water?

Learn how to calculate the number of molecules in a 5.65 mole sample of water using Avogadro's number. This problem involves multiplying the mole quantity by 6.022 × 10^23, resulting in approximately 3.4 × 10^24 molecules. Suitable for high school students studying chemistry.

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