Question

The density of water is 1.00 g/ml at 4°c. how many water molecules are present in 2.36 ml of water at this temperature?

Answer 1

To find the number of water molecules in 2.36 mL of water at 4°C, calculate the mass of water using its density, convert that mass to moles using the molar mass of water, and then multiply by Avogadro's number to get the molecule count.

Step-by-step explanation:

The question involves calculating the number of water molecules in a given volume of water using the density of water and Avogadro's number. First, we find the mass of water using the density (1.00 g/mL) and volume (2.36 mL), which gives us 2.36 g of water. Next, we convert grams to moles by dividing by the molar mass of water (approximately 18.015 g/mol). Finally, we multiply the number of moles by Avogadro's number (6.022×10²³ particles/mol) to find the number of molecules.

Using these steps:
Mass = Density × Volume = 1.00 g/mL × 2.36 mL = 2.36 g
Moles = Mass / Molar Mass = 2.36 g / 18.015 g/mol
Molecules = Moles × Avogadro's Number

Answer 2

Mass of 1 ml of water 1 g as density of water 1.00 g/ml at 4° C. So, mass of 2.36 ml of water
`(1)/(2.36)` g= 0.423 g.

Molecular mass of water is 18 g which indicates 18 g water contains 6.023 X
`10^(23)` number of water molecules. So, 0.423 g of water contains
`(6.023 X 10^(23) X 0.423 )/(18)  g` = 0.141 X
`10^(23)` number of water molecules= 1.41 X
`10^(22)` number of water molecules.