The density of Hg is 13.6g/cm^3. How many Hg atoms are present in 10.0cm^3 of Hg?
I think the size of an atom is 6.22 x 10^23. The answer is 4.08 x 10^23. I need help getting to the answer.
13.6 g Hg/cm^3 * 10 cm^3 The cm^3 cancels out and you get 136 g Hg.
136 g Hg * 200.59 g Hg/ 1 mol Hg = 0.68 mol Hg.
0.68 mol Hg * 6.02*10^23 atoms Hg/ 1 mol Hg= 4.08*10^23 atoms Hg
I did your other one.
Two minor problems with the answer ffrom Ana.
136 x (1 mol/200.59) = 0.68 mole [the fraction is the reciprocal is problem 1) and the second is I would have carried the number out to 0.678 since you are allowed 3 significant figures.)
Then 0.678 x 6.022 x 10^23 = ??
Thankyou both very much.
To find the number of Hg atoms in 10.0 cm^3 of Hg, we need to use the concept of Avogadro's number (6.022 x 10^23 atoms/mol) and the molar mass of Hg. Here's how to get to the answer step by step:
1. The given information is the density of Hg, which is 13.6 g/cm^3. Density is defined as mass per unit volume. So, we can figure out the mass of Hg in 10.0 cm^3 by multiplying the volume by the density:
Mass = Volume x Density
Mass = 10.0 cm^3 x 13.6 g/cm^3
Mass = 136 g.
So, we have 136 grams of Hg.
2. To calculate the number of moles of Hg, we need the molar mass of Hg, which is 200.59 g/mol. We can find the moles using the formula:
Moles = Mass / Molar Mass
Moles = 136 g / 200.59 g/mol
Moles = 0.678 mol.
Thus, we have 0.678 moles of Hg.
3. Finally, we can use Avogadro's number to find the number of Hg atoms. We know that 1 mole of any substance contains 6.022 x 10^23 particles (atoms, molecules, etc.). So, we can calculate the number of Hg atoms using the following conversion factor:
Number of Hg atoms = Moles of Hg x Avogadro's number
Number of Hg atoms = 0.678 mol x (6.022 x 10^23 atoms/mol)
Number of Hg atoms ≈ 4.08 x 10^23 atoms.
Therefore, there are approximately 4.08 x 10^23 Hg atoms present in 10.0 cm^3 of Hg.