Consider an ice cube with a volume of 0.50 cup. (1 cup = 240.0 mL, density of ice = 0.9167 g/mL). How many water molecules (molar mass = 18.015 g/mol) are present in this ice cube?

3.86x10^24 molecules

Explanation:

From the question given, the following data were obtained:

Volume of ice = 0.5cup

1 cup = 240mL

0.5cup = 0.5 x 240 = 120mL

Density of ice = 0.9167 g/mL

molar mass of water = 18.015g/mol

First let us calculate the mass of ice. This is illustrated below:

Density = Mass /volume

Mass = Density x volume

Mass = 0.9167 x 120

Mass of ice = 110.004g = Mass of water

From Avogadro's hypothesis, we understood that 1mole of any substance contains 6.02x10^23 molecules. This means that 1mole of water will also contain 6.02x10^23 molecules.

1mole of water = 18.015g

If 1 mole (18.015g) contains 6.02x10^23 molecules,

Therefore, 110.004g of water will contain = (110.004x6.02x10^23)/18.015 = 3.86x10^24 molecules

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.

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