How many water molecules are in a 10.0g sample of water?

First you need the molar mass of water(H2O).

Given that oxygen is 16 g mole^-1 and hydrogen is 1 g mole^-1 the molar mass of water is 18 g mole^-1.

Next we need the number of moles of water that 10.0 g represents (N) which we get from

N=10.0 g / 18 g mole^-1

as one mole contains 6x10^23 molecules then

Nx6x10^23 is the number of molecules.

To determine the number of water molecules in a 10.0g sample of water, we need to use the concept of molar mass and Avogadro's number.

1. The molar mass of water (H2O) is approximately 18.015 g/mol.
2. Calculate the number of moles of water in the given sample using the formula:

Moles = Mass / Molar mass

Moles = 10.0 g / 18.015 g/mol

3. Solve for the number of water molecules by multiplying the number of moles by Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol.

Number of water molecules = Moles × Avogadro's number

Number of water molecules = (10.0 g / 18.015 g/mol) × (6.022 x 10^23 molecules/mol)

The final calculation will give you the number of water molecules in the 10.0g sample.

To determine the number of water molecules in a 10.0g sample of water, we need to use the concept of moles and Avogadro's number.

First, we need to convert the mass of the water sample from grams to moles. To do this, we divide the mass by the molar mass of water, which is approximately 18.015 g/mol.

10.0g ÷ 18.015 g/mol = 0.555 mol (rounded to three decimal places)

Next, we use Avogadro's number, which is 6.022 x 10^23 molecules/mol, to convert from moles to molecules.

0.555 mol x (6.022 x 10^23 molecules/mol) = 3.34 x 10^23 molecules

Therefore, in a 10.0g sample of water, there are approximately 3.34 x 10^23 water molecules.

3.34x10^23