Answer :

In 100.5 grams of water, there are approximately 6.70 × 10^24 atoms of hydrogen.

In 1 mole of water (H2O), there are 2 moles of hydrogen atoms (H). The molar mass of water is approximately 18.015 g/mol. To determine the number of moles of water, we divide the given mass by the molar mass:

moles of water = mass of water / molar mass of water

moles of water =[tex]100.5 g / 18.015 g/mol ≈ 5.57 moles[/tex]

Since the molar ratio between water and hydrogen is 2:1, we multiply the number of moles of water by 2 to find the number of moles of hydrogen:

[tex]moles of hydrogen = 2 * moles of water ≈ 11.14 moles[/tex]

Finally, we use Avogadro's number[tex](6.022 × 10^23 atoms/mol)[/tex] to convert the moles of hydrogen to the number of atoms of hydrogen:

number of atoms of hydrogen = moles of hydrogen * Avogadro's number

number of atoms of hydrogen =[tex]11.14 moles * 6.022 × 10^23 atoms/mol ≈ 6.70 × 10^24 atoms[/tex]

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Final answer:

There are approximately 6.72 x 1024 hydrogen atoms in 100.5g of water. This is calculated by first determining the number of water molecules and then multiplying by 2 (as each water molecule contains 2 hydrogen atoms).

Explanation:

To determine the number of hydrogen atoms in 100.5g of water (H2O), we first need to know how many molecules of water (H2O) are present. The formula to calculate the number of molecules in a sample is given by:

  1. Number of molecules = mass/molar mass

The molar mass of water is approximately 18.015 g/mol. So, 100.5g of water contains approximately:

  1. 100.5g ÷ 18.015 g/mol ≈ 5.58 mol.

Since Avogadro's number is 6.022 x 1023 molecules/mol, the total number of water molecules is calculated as:

  1. 5.58 mol x 6.022 x 1023 molecules/mol ≈ 3.36 x 1024 molecules.

Remember, each water (H2O) molecule contains 2 hydrogen atoms. Therefore, the total number of hydrogen atoms is:

  1. 3.36 x 1024 molecules x 2 hydrogen atoms/molecule ≈ 6.72 x 1024 hydrogen atoms.

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