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

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

b. examine and describe cells