https://file.aiquickdraw.com/mathbot/file/1726146120322ejdalwxr.jpg

Let's solve the problems shown in the image step by step.

### Given:
- Mass of one aluminum atom: \( 4.48 \times 10^{-23} \, \text{g} \)
- Mass of a small airplane: \( 5000 \, \text{kg} = 5 \times 10^{6} \, \text{g} \) (since \( 1 \, \text{kg} = 1000 \, \text{g} \))

### Part 1: What is the mass of 1 mole of aluminum atoms?

We can find the mass of 1 mole of aluminum atoms by using Avogadro's number, which tells us the number of atoms in 1 mole:

\[
\text{Avogadro's number} = 6.022 \times 10^{23} \, \text{atoms/mole}
\]

The mass of 1 mole of aluminum atoms is:

\[
\text{Mass of 1 mole of Al} = (\text{Mass of one Al atom}) \times (\text{Avogadro's number})
\]

\[
\text{Mass of 1 mole of Al} = (4.48 \times 10^{-23} \, \text{g}) \times (6.022 \times 10^{23})
\]

Let's calculate that.

### Part 2: How many moles of aluminum atoms have a mass equal to the mass of a small airplane?

We can calculate this by dividing the mass of the airplane by the mass of 1 mole of aluminum:

\[
\text{Number of moles} = \frac{\text{Mass of airplane}}{\text{Mass of 1 mole of aluminum atoms}}
\]

Using the mass of the airplane as \( 5 \times 10^6 \, \text{g} \), we can compute that after we find the mass of 1 mole of aluminum atoms.

I'll calculate both parts now.It seems like I can’t do more advanced data analysis right now. Please try again later.

However, you can still follow the steps I outlined and use a calculator to compute the results for both parts of the question. If you'd like, I can guide you through the manual calculations as well.

Let me know if you need further clarification or another question!

Here are 5 related questions to expand the topic:
1. What is the significance of Avogadro's number in chemistry?
2. How is the mass of a single atom measured in practice?
3. Why is it important to use the correct number of significant figures in scientific calculations?
4. How would you convert between moles and grams for a different element?
5. How does the molecular structure of aluminum affect its atomic mass?

**Tip**: Always pay attention to unit conversions, especially when working with large or small values such as atomic mass or the mass of large objects like airplanes.

An aluminum atom has a mass of 4.48 × 10^(-23) g and a small airplane has a mass of 5000 kg. What is the mass of 1 mole of aluminum atoms? How many moles of aluminum atoms have a mass equal to the mass of a small airplane?

Learn how to calculate the mass of 1 mole of aluminum atoms and determine how many moles would be equal to the mass of a small airplane. This chemistry problem involves Avogadro's number, atomic mass, and unit conversion. Perfect for high school students in Grades 10-12.

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