Final answer:
There are approximately 3.34 x 10²⁵ water molecules in a 1.00-liter bottle of water, with the given density of 1.00 g/mL. This is calculated by finding the mass of the water, determining the number of moles, and then using Avogadro's number to find the molecule count.
Step-by-step explanation:
To calculate the number of water molecules in a 1.00-liter bottle of water using its density, we will first find the mass of the water and then use Avogadro's number to find the number of molecules.
- Firstly, we identify that the density of water is 1.00 g/mL. Since there are 1000 mL in 1 L, the mass of water in a 1.00-liter bottle is 1000 g (1 kg).
- Now we use the molecular weight of water (H₂O), which is approximately 18.015 g/mol, to find the number of moles in 1000 g of water. We divide the mass of water by the molar mass: 1000 g / 18.015 g/mol ≈ 55.50 moles.
- Next, we use Avogadro's number, which is 6.022 x 10²³, to calculate the number of molecules in those moles: 55.50 moles x 6.022 x 10²³ molecules/mol = 3.34 x 10²⁵ water molecules.
Therefore, there are approximately 3.34 x 10²⁵ water molecules in a 1.00-liter bottle of water, given the density of water is 1.00 g/mL.