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From the image you uploaded, the problem involves calculating the mass of one mole of aluminum atoms, given that:

- The mass of one aluminum atom is \( 4.48 \times 10^{-23} \, \text{g} \).
- You are asked to find the mass of 1 mole of aluminum atoms.

### Key concepts:
- **Avogadro's number**: The number of atoms in one mole of any substance is \( 6.022 \times 10^{23} \, \text{atoms/mol} \).

### Solution:

To find the mass of 1 mole of aluminum atoms, multiply the mass of a single atom by Avogadro's number:

\[
\text{Mass of 1 mole of aluminum atoms} = \text{Mass of 1 atom} \times \text{Avogadro's number}
\]

\[
\text{Mass} = (4.48 \times 10^{-23} \, \text{g}) \times (6.022 \times 10^{23} \, \text{atoms/mol})
\]

Let's compute this.The mass of 1 mole of aluminum atoms is approximately **26.98 g**. 

Your previous answer was 26.9 g, but rounding it to two decimal places (based on significant digits) gives **26.98 g**, which should be the correct answer.

Would you like further details on the significant digits or any other questions?

Here are five related questions you might consider:
1. What are the rules for determining significant digits?
2. How does Avogadro's number relate to moles in chemistry?
3. Can you explain the concept of atomic mass and how it is measured?
4. How is the mass of a single atom determined experimentally?
5. What other examples involve using Avogadro's number for different elements?

**Tip:** When working with significant digits, always ensure your final answer reflects the precision of the given values.

An aluminum atom has a mass of 4.48 x 10^-23 g and a small airplane has a mass of 5000 kg. Use this information to answer the question: What is the mass of 1 mole of aluminum atoms?

Learn how to calculate the mass of 1 mole of aluminum atoms using the mass of a single atom and Avogadro's number. This problem involves significant figures and scientific notation, suitable for high school chemistry students.

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