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The density of potassium, which has the BCC structure, is 0.855 g/cmÂ³. The atomic weight of potassium is 39.09 g/mol. Please answer the questions below:
a) How many atoms per BCC cell? (3 points)
b) What is the coordination number for BCC cubic structure? (3 points)
c) Determine the packing fraction of BCC (potassium). (5 points)
d) Find the lattice parameter of potassium. (3 points)
e) Find the atomic radius of potassium. (3 points)
(Assuming cubic cell dimensions are “a” and atom radius is “r”)
Q2.
a) Please specify the circle coordinate for a cubic unit cell. (3 points)
b) Please sketch the following plane and direction within a cubic unit cell. (3 points each)

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02:21

The density of potassium, which has the BCC structure, is 0.855 g/cmÂ³. The atomic weight of potassium is 39.09 g/mol. Calculate (a) the lattice parameter: A = 5.289E-8 cm. Format: x.xxxxE-8 cm. (b) the atomic radius of potassium: 1.331E-8 cm. Format: x.xxxxE-8 cm.

03:00

1. The metal potassium crystallizes in a body-centered cubiclattice. If the density of potassium is 0.856 g/cm3, what is theunit cell edge length?a. 533 pmb. 41.7 pmc. 157.0 pmd. 33.1 pme. 423 pm2. Palladium crystallizes with a face-centered cubic unit cell.If the edge length of the unit cell is 387 pm, what is the radiusof a palladium atom in picometers?a. 137 pmb. 548 pmc. 1090 pmd. 316 pme. 48.4 pm

01:47

Potassium has BCC structure with nearest neighbour distance $(2.5 \times \sqrt{3}) \dot{A}$. Its density will be $\left(\mathrm{K}=39, N_{\mathrm{A}}=6 \times 10^{23}\right)$(a) $1.040 \mathrm{~kg} / \mathrm{m}^{3}$(b) $104 \mathrm{~kg} / \mathrm{m}^{3}$(c) $520 \mathrm{~kg} / \mathrm{m}^{3}$(d) $1040 \mathrm{~kg} / \mathrm{m}^{3}$

01:32

The element potassium has a molar mass of 39.098 grams/mole andcrystallizes in a BCC unit cell with a density of 0.856g/cm3. Calculate the radius in pm of a K atom.

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