Question

CHEM HELP!

using the average atomic mass, calculate the number of atoms present in 1.2 mL of liquid mercury.
(Density=13.6g/mL)

Answer 1

So let's convert this amount of mL to grams:

`(13.6g)/(1mL)*1.2mL=16.32g`

Then we need to convert to moles using the molar weight found on the periodic table for mercury (Hg):

`(1mole)/(200.59g)*16.32g=8.135*10^(-2)mol`

Then we need to convert moles to atoms using Avogadro's number:

`(6.022*10^(23)atoms)/(1mole) *[8.135*10^(-2)mol]=4.90*10^(22)atoms`

So now we know that in 1.2 mL of liquid mercury, there are
`4.90*10^(22)atoms` present.