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anonymous
 one year ago
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.
anonymous
 one year ago
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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aaronq
 one year ago
Best ResponseYou've already chosen the best response.1first find the volume of the cube, then find the mass with the density, finally convert the mass to moles

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0How do you find the volume?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0So do you find the mass by using the density formula?

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1you'll have to convert the volume (or the density) to match the units

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I'm trying to work it out and getting confused.

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2\[\sf \rho = \frac{m}{v} \\ \rho = 120~\frac{g}{mL}~,~~v =(1mm)^3 \] \[\sf 1~mm^3 ~\times~ \left(\frac{1~cm}{1~mm}\right)^3~\times~\frac{1~mL}{1~cm^3} =~1~mL\] \[\sf \frac{120~g}{mL} =\frac{m}{1~mL}~\implies m = 120~g\]

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2When I see a value or conversion factor, I typically try to associate it with an appropriate formula

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1you made a mistake, 1 cm = 10 mm, so: \(\sf \large 1~mm^3 ~\times~ \left(\frac{1~cm}{10~mm}\right)^3~\times~\frac{1~mL}{1000~cm^3} =~0.001~mL\)

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2...it was a typo <_<

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Um...which way is it?

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2The way @aaronq wrote.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Would it be 1000 or 100 for cm^3?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Alright. I was wondering why there was an extra 0

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Thanks for the help!

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2Ok 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.

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.2So once we have this, create a ratio: \[\sf \frac{120~g}{1~mL} = \frac{m}{1.0~\times~10^{3}~mL} \implies m=~(120 \cdot 1.0~\times~10^{3})g\]

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1i made a mistake too..it's supposed to be: \(\sf \large 1~mm^3 ~\times~ \left(\frac{1~cm}{10~mm}\right)^3~\times~\frac{1~cm^3}{1000~mm^3} =0.001~cm^3=~0.001~mL\)

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1it is 1000, 10^3= 1000 no?
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