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Calculate the density of CsCl. Use 169pm as the radius of Cs+.
rCs+= 169pm
length= 2*169= 338pm= 3.38*10^-8
v= l^3= (3.38*10^-8)^3 = 3.86*10^-23
m= 2* 168.36 g/mol / 6.022*10^23 = 5.59*10^-24g
d= m/v
d= 5.59*10^-24g/ 3.86*10^-23
d= 14.48 g/cm^3
BUT the correct answer is 4.24 g/cm^3. I can't figure out my mistake I've done it several times
rCs+= 169pm
length= 2*169= 338pm= 3.38*10^-8
v= l^3= (3.38*10^-8)^3 = 3.86*10^-23
m= 2* 168.36 g/mol / 6.022*10^23 = 5.59*10^-24g
d= m/v
d= 5.59*10^-24g/ 3.86*10^-23
d= 14.48 g/cm^3
BUT the correct answer is 4.24 g/cm^3. I can't figure out my mistake I've done it several times
Answers
Answered by
smiley
How did you get that answer then?
Answered by
bfdslf
You used the cation radius when calculating volume rather than the anion radius.
Answered by
Bhag Singh
Side of cube(unit cell) is root(3)×a=4r.
You are using 2r
Thats wrong.
You are using 2r
Thats wrong.
Answered by
vasu
Actually you have to use 4r=/3.a for volume then you get 1095.8 kg/m3 for one atom. and one unit cell has 4 cation (cs+) and 1 anion (cl-) and you have multiply 4x1x1095.8 = 4380 kg/m3.