A solid substance has a density of 12 g/mL. A cube made out of this substance has 1 mm edge length. If the atomic mass of the substance is 120.0 g/mol, calculate how many moles of the substance are in this cube.

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A solid substance has a density of 12 g/mL. A cube made out of this substance has 1 mm edge length. If the atomic mass of the substance is 120.0 g/mol, calculate how many moles of the substance are in this cube.

Chemistry
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first find the volume of the cube, then find the mass with the density, finally convert the mass to moles
How do you find the volume?
|dw:1442365426768:dw|

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Other answers:

So do you find the mass by using the density formula?
yep
you'll have to convert the volume (or the density) to match the units
I'm trying to work it out and getting confused.
\[\sf \rho = \frac{m}{v} \\ \rho = 120~\frac{g}{mL}~,~~v =(1mm)^3 \] \[\sf 1~mm^3 ~\times~ \left(\frac{1~cm}{1~mm}\right)^3~\times~\frac{1~mL}{1~cm^3} =~1~mL\] \[\sf \frac{120~g}{mL} =\frac{m}{1~mL}~\implies m = 120~g\]
When I see a value or conversion factor, I typically try to associate it with an appropriate formula
you made a mistake, 1 cm = 10 mm, so: \(\sf \large 1~mm^3 ~\times~ \left(\frac{1~cm}{10~mm}\right)^3~\times~\frac{1~mL}{1000~cm^3} =~0.001~mL\)
...it was a typo <_<
suuuuure it was :P
A+ for effort
Um...which way is it?
The way @aaronq wrote.
Thanks
Would it be 1000 or 100 for cm^3?
Alright. I was wondering why there was an extra 0
Thanks for the help!
Ok that was my fault. I had it backwards. \[\sf 1~mm^3 \times\left(\frac{1~cm}{10~mm}\right)^3~\times~ \frac{1~mL}{1~cm^3} =~1.0~\times~10^{-3}~mL \]Thats what it should be. There should be no 1000.
So once we have this, create a ratio: \[\sf \frac{120~g}{1~mL} = \frac{m}{1.0~\times~10^{-3}~mL} \implies m=~(120 \cdot 1.0~\times~10^{-3})g\]
i made a mistake too..it's supposed to be: \(\sf \large 1~mm^3 ~\times~ \left(\frac{1~cm}{10~mm}\right)^3~\times~\frac{1~cm^3}{1000~mm^3} =0.001~cm^3=~0.001~mL\)
it is 1000, 10^3= 1000 no?

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