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Answer :
There are approximately 1.11 x 10^22 atoms of mercury in 1.37 mL of mercury. to calculate the number of atoms, we need to first determine the mass of 1.37 mL of mercury using its density.
Density is defined as mass per unit volume, so we can calculate the mass of 1.37 mL of mercury as:
mass = density x volume
mass = 13.5 g/mL x 1.37 mL
mass = 18.495 g
Next, we need to convert the mass of mercury into the number of atoms. To do this, we use the molar mass of mercury, which is 200.59 g/mol. We can calculate the number of moles of mercury as:
moles = mass / molar mass
moles = 18.495 g / 200.59 g/mol
moles = 0.0922 mol
Finally, we can convert moles of mercury into the number of atoms using Avogadro's number, which is 6.022 x 10^23 atoms/mol:
number of atoms = moles x Avogadro's number
number of atoms = 0.0922 mol x 6.022 x 10^23 atoms/mol
number of atoms = 1.11 x 10^22 atoms
Therefore, there are approximately 1.11 x 10^22 atoms of mercury in 1.37 mL of mercury.
Learn more about mercury here:
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