To find how many grams are in $5.033 \times 10^{24}$ atoms of oxygen, we can follow these steps:

1. Find the molar mass of oxygen:
   Oxygen has a molar mass of approximately 16 grams per mole (g/mol).

2. Use Avogadro's number:
   Avogadro's number is $6.022 \times 10^{23}$ atoms per mole. This tells us how many atoms are in 1 mole of oxygen.

3. Convert atoms to moles:
   To convert the given number of atoms to moles, divide the number of atoms by Avogadro's number:
   $\text{Moles of oxygen} = \frac{5.033 \times 10^{24} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}}$

4. Convert moles to grams:
   Once we know how many moles we have, we can multiply by the molar mass (16 g/mol) to find the mass in grams.

Let's calculate this:

$\text{Moles of oxygen} = \frac{5.033 \times 10^{24}}{6.022 \times 10^{23}} \approx 8.36 \text{ moles}$

Now, multiply by the molar mass:

$\text{Mass of oxygen} = 8.36 \text{ moles} \times 16 \text{ g/mol} = 133.76 \text{ grams}$

Thus, $5.033 \times 10^{24}$ atoms of oxygen weigh approximately 133.76 grams.

Would you like more details or have any questions?

Here are 5 related questions for further understanding:

1. How would the mass change for a different number of atoms?
2. What is the role of Avogadro's number in these calculations?
3. How do you convert from grams to atoms of a substance?
4. Why is the molar mass of oxygen 16 g/mol?
5. How does the concept of moles help in chemistry?

Tip: Always make sure to use the correct molar mass depending on the element's molecular form, like O$_2$ for molecular oxygen.