Final answer:
To convert the given number of atoms of mercury to grams, we need to use the molar mass of mercury and Avogadro's number. First, convert atoms to moles by dividing by Avogadro's number. Then, convert moles to grams using the molar mass of mercury.
Step-by-step explanation:
To determine the number of grams of mercury in 5.3x1024 atoms of mercury, we need to convert the given number of atoms to grams using the molar mass of mercury. The molar mass of mercury is 200.59 g/mol. This means that one mole of mercury contains 200.59 grams. To convert atoms to moles, we divide the given number of atoms by Avogadro's number, which is 6.022x1023 atoms/mol.
First, let's find the number of moles of mercury in 5.3x1024 atoms:
5.3x1024 atoms / 6.022x1023 atoms/mol = 8.806 mol
Next, we can use the molar mass of mercury to convert moles to grams:
8.806 mol * 200.59 g/mol = 1765.5 g
Therefore, there are 1765.5 grams of mercury in 5.3x1024 atoms of mercury.
Learn more about converting atoms to grams using the molar mass of an element