Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Joules23 on January 28, 2007, 10:18:53 PM
-
Solid tantalum is made up of repeating unit cells that are cubes, with edges of length 330.29 picometers. Each unit cell contains two tantalum atoms. Solid tantalum has a density of 16.654 g/cm^3. Calculate Avogadros number using this data. V=a^3
1 mole Ta = 180.9479g Ta = ? atoms Ta
i know im supposed to get 6.022e23 , but im not getting that, let me know what im doing wrong.
1 mole Ta=1 mole Ta (180.9479g/1 mole)(1cm^3/16.654g)((10e-2)^3/1cm^3)(1 molecule/3.3029e-24m^3)
= 3.2896e21
-
Your units are wrong. And you are also not including the number of atoms in each unit cell.
N = (n*m)/(p*v)
N= avagardos number
n = number of atoms in smallest unit cell
m=molar mass
p=density
v=volume
Note, your molar mass and density are in grams and cm^3. This means you must either convert both of those into meters and kilograms, or convert the picometers into centimeters.
-
Here is how I would work out the problem.
First, convert density to g/pm^3
(16.654g/cm^3)x(1cm^3/10^30pm^3) = 1.6654x10^-32 g/pm^3
Then, calculate weight of a unit cell by multiplying density by volume
(1.6654x10^-32 g/pm^3) x (330.29pm)^3 = 6 x 10^-22 g / unit cell
Since there are two atoms in the unit cell, weight of one atom is 3 x 10^-22 g
Finally, 180.949g / Avogadro's No. = weight of an atom = 3 x 10^-22g
Solve the equation and there you go.
-
thanks for that, it really helped me
i have one more question regarding Avogardros number:
Use the density of steric acid, the volme of a molecule and 1 mole=284g to calculate Avogadros number.
Density of steric acid = .1g/L
Volume of molecule = 8.89 x 10^-26 L
DxVxA=284g
(.1)(8.89x10^-26)A=284g
A=3.19x10^28
But according to my computer print out im supposed to get 3.4x10^24, what am i doing wrong?
-
Density of steric acid = .1g/L
density is wrong
-
wow yea.. your right, now i feel dumb, thanks