How many atoms are in 10.0 cm3 of mercury (at room temperature)?
mass Hg = volume Hg x density Hg
mols Hg = grams Hg/atomic mass Hg
Then you know 1 mol Hg contains 6.02E23 atoms.
To find the number of atoms in a given amount of substance, you need to use the Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol.
To determine the number of atoms in 10.0 cm3 of mercury, you need to follow these steps:
Step 1: Determine the molar mass of mercury (Hg). The molar mass of mercury is approximately 200.59 g/mol.
Step 2: Convert the volume of mercury from cm3 to liters. Since 1 cm3 is equal to 1 x 10^-6 liters, 10.0 cm3 of mercury is equal to 10.0 x 10^-6 liters.
Step 3: Calculate the number of moles of mercury. The number of moles can be determined using the formula:
moles = volume (in liters) / molar volume (22.4 L/mol at room temperature)
moles = 10.0 x 10^-6 / 22.4
Step 4: Calculate the number of atoms by multiplying the number of moles by Avogadro's number:
number of atoms = moles x Avogadro's number
number of atoms = (10.0 x 10^-6 / 22.4) x 6.022 x 10^23
After performing this calculation, you will have the number of atoms in 10.0 cm3 of mercury at room temperature.