Answer :

Final answer:

To find the number of oxygen atoms in 163 g of aluminum sulfate, calculate the moles of aluminum sulfate, determine moles of oxygen by multiplying with 12 (from the formula), and use Avogadro's number to convert moles to atoms, resulting in approximately 3.44 × 10^24 oxygen atoms.

Explanation:

To determine how many oxygen atoms are in 163 g of aluminum sulfate, we first need to know the molar mass of aluminum sulfate, which is the sum of the molar masses of all the atoms in its formula, Al2(SO4)3. The molar mass consists of 2 moles of aluminum (Al), 3 moles of sulfur (S), and 12 moles of oxygen (O) atoms. Using the periodic table, we find the molar mass of aluminum sulfate to be about 342.15 g/mol.

Next, using the molar mass, we calculate the number of moles of aluminum sulfate in 163 g:

(163 g Al2(SO4)3) / (342.15 g/mol) = 0.476 moles of Al2(SO4)3

Since each mole of aluminum sulfate contains 12 moles of oxygen, we multiply 0.476 moles of aluminum sulfate by 12 to get the total moles of oxygen:

0.476 moles Al2(SO4)3 × 12 moles O = 5.712 moles O

Finally, we use Avogadro's number (6.022 × 1023 atoms/mol) to convert moles of oxygen to atoms:

5.712 moles O × (6.022 × 1023 atoms/mol) = 3.44 × 1024 oxygen atoms

Therefore, there are approximately 3.44 × 1024 oxygen atoms in 163 g of aluminum sulfate.

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