how many atoms are present in a sample of water molecules with a mass of 1.800g
mols H2O = grams/molar mass
1 mol contains 6.02E23 molecules.
There are no LONE but there are three single atoms/single molecule. Can you take it from there.
To determine the number of atoms present in a sample of water molecules, you need to understand the concept of moles and Avogadro's number.
1. Calculate the number of moles of water molecules:
- Water's molar mass (H2O) = 18.015 g/mol (2 hydrogen atoms + 1 oxygen atom)
- Moles = Mass / Molar Mass
- Moles = 1.800 g / 18.015 g/mol = 0.0999 mol (rounded to four decimal places)
2. Use Avogadro's number to calculate the number of atoms:
- Avogadro's number (NA) = 6.022 x 10^23 atoms/mol
- Number of atoms = Moles x NA
- Number of atoms = 0.0999 mol x 6.022 x 10^23 atoms/mol = 6.02 x 10^22 atoms (rounded to three significant figures)
Therefore, there are approximately 6.02 x 10^22 atoms in a sample of water molecules with a mass of 1.800g.