# How many cubic centimeters would you need to have 1 mole of aluminum?

is a value that can compared to particles (molecules and atoms), volume and mass.

The mole is equal ##6.02 x 10^23## molecules, which is known as Avogadro’s number. The mole is equal to 22.4 Liters of gas at standard temperature and pressure (STP). And, the mole is equal to the molar mass (gfm) of the element or molecule.

The element aluminum has a molar mass of 26.99 amu. Therefore, a 1 mole sample of aluminum would have a mass of 26.99 grams.

Once we know the mass of the mole of aluminum we can use the to calculate the volume. The density equation is ##D = m/v##, where D = density, m = mass and v = volume.

The standard density of aluminum is ##2.70 g/(cm^3)##,

##D = m/v## and ##v = m/D##

D = ##2.70 g/(cm^3)##
m = ##26.99 g##
v = ???

##v = (26.99 g)/(2.70 g/(cm^3))##

##v = 9.99 cm^3##

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