anonymous
  • anonymous
ASAP PLEASE What is the mass, in grams, of a sample of 1.20 × 1022 atoms of mercury (Hg)? Show your work or explain the steps that you used to determine your answer.
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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jamiebookeater
  • jamiebookeater
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thomaster
  • thomaster
Do you know the molar mass of mercury?
anonymous
  • anonymous
No :(
thomaster
  • thomaster
Have a look at this Image. You're at number of particles. Can you figure out what the first step is?
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anonymous
  • anonymous
._. The image is confusing me even more.
anonymous
  • anonymous
Could you write down the formula for me?
thomaster
  • thomaster
It's not a formula. It's like a path. In order to go from atoms of mercury to mass, you first have to convert atoms to mol. To do this, you have to divide the number of atoms by avogadro's number (6.022*10^23)
anonymous
  • anonymous
how do i do that though? Like how do i divide 1.20 × 1022 by 6.022*10^23?
anonymous
  • anonymous
@thomaster
thomaster
  • thomaster
with a calculator of course
thomaster
  • thomaster
\(\LARGE\dfrac{1.20*10^{22}}{6.022*10^{23}}\)
thomaster
  • thomaster
then you will have the amount of moles mercury. Next step is to multiply with the molar mass of mercury. You can find it in any periodic table.

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