If the density of mercury is 13.53g/cm^3 and you have 62.5 cm^3 of mercury, how many: grams of mercury do you have? moles of mercury do you have? atoms of mercury do you have?

The answer to your question is below

Explanation:

Data

density = 13.53 g/cm³

volume = 62.5 cm³

mass = ?

moles = ?

atoms = ?

Process

1.- Calculate the mass of mercury

formula

density = mass/volume

-Solve for mass

mass = density x volume

-Substitution

mass = 13.53 x 62.5

-Result

mass = 845.63 grams

2.- Calculate the moles of mercury

Atomic mass = 200.6 g

              200.6 g of mercury 1 mol

              845.63 g of mercury  x

                   x = (845.63 x 1) / 200.6

                   x = 4.22 moles of mercury

3.- Calculate the number of atoms

               1 mol  6 .023 x 10 ²³ atoms

             4.22 moles   x

                 x = (4.22 x 6.023 x 10²³) / 1

                x = 2.54 x 10²³ atoms

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer