How many atoms of mercury are present in

3.2 cubic centimeters of liquid mercury?
The density of mercury is 13.55 g/cc.

mass Hg = volume x density.

Substitute and solve for mass Hg.

Convert mass Hg in grams to moles. moles = grams/molar mass.

Remember 1 mole of Hg contains 6.022E23 atoms Hg..

0.3645564

To determine the number of atoms of mercury present in 3.2 cubic centimeters of liquid mercury, we need to use the density of mercury and convert it to the number of moles of mercury. Then, using Avogadro's number, we can calculate the number of atoms.

Here's a step-by-step breakdown to find the answer:

Step 1: Convert the volume of mercury to grams.
Given density of mercury = 13.55 g/cc
Volume of liquid mercury = 3.2 cc

To find the mass of mercury, we can use the formula:
Mass = Density * Volume

Mass of mercury = 13.55 g/cc * 3.2 cc = 43.36 grams

Step 2: Convert the mass of mercury to moles.
To find the number of moles of mercury, we need to know its molar mass. The molar mass of mercury is 200.59 g/mol.

To calculate the number of moles, we can use the formula:
Moles = Mass / Molar mass

Moles of mercury = 43.36 g / 200.59 g/mol ≈ 0.216 moles

Step 3: Convert the moles of mercury to atoms.
Avogadro's number states that there are 6.022 x 10^23 atoms in one mole of any substance.

To calculate the number of atoms, we can use the formula:
Atoms = Moles * Avogadro's number

Atoms of mercury = 0.216 moles * 6.022 x 10^23 atoms/mol ≈ 1.301 x 10^23 atoms

Therefore, there are approximately 1.301 x 10^23 atoms of mercury present in 3.2 cubic centimeters of liquid mercury.