Hello everyone, here is the problem i have:
The element nickel crystallizes in a face-centered cubic crystal, with a0 = 3.5238 pm. The atomic weight is 58.69 g/mol. Avogadro’s number is 6.02214×10^23mol-1. What is the calculated density of Ni, in g/cm3?
The Answer given is: 8.909g/cm^3
Here is my work:
1. Convert a0 from picometers to centimeters
3.5238 pm x 1cm/10^10pm = 3.5238 x 10^-10 cm
2. Cube a0 to get volume in cm^3
(3.5238 x 10^-10 cm)^3 = 4.375 x 10 ^ -29 cm^3
3. Calculate mass of the sample
Because its a face centered cube:
4(58.69 g/mol)
_____________ = 3.89 x 10^-22 g
6.02214×1023mol-1
4. Since D = m/v
D = (3.89 x 10^-22 g)/(4.375 x 10 ^ -29 cm^3) = 8909423.353 g/ cm^3
Im getting the right values but the decimal point seems to be shifted a bit too far....
Can anyone take a look at what i did wrong?
Thanks.