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A metal crystallizes in a body-centered cubic structure (edge length = 47/13) and has a density...
A metal crystallizes in a body-centered cubic structure (edge length = 4/3) and has a density of 12.9 g/cm2. If the radius of the metal atom is 128 pm, what is the molar mass of the metal in g/mol? Express your answer using 3 significant figures. Question 30 5 pts Consider the reaction: 2 ICI (g) <-->l2(g) + Cl2 (g). Its equilibrium constant is K-0.0122 (T-298K) A reaction mixture at T=298K initially contains Pici-Pci, = P1, -0.100atm. What is the...
Metal x crystallizes in a face-centered cubic (close-packed) structure. The edge length of the unit cell was found by x-ray diffraction to be 383.9 pm. The density of x is 20.95 . Calculate the mass of an x atom, and use Avogadro’s number to calculate the molar weight of Metal X crystallizes in a face-centered cubic (close-packed) structure. The edge length of the unit cell was found by x-ray diffraction to be 383.9 pm. The density of X is 20.95...
3. (4 points) A metal crystallizes in a face centered cubic structure and has a density of 11.9 g/cm. If the radius of the metal atom is 138 pm, what is the identity of the metal? P ( i)x (138Yio) 5.9H CX1013 (5.9466X 10 Cm 7.07 X107S 7.07 X103 6.02 2 x 103 -S
1. Vanadium crystallizes in a body-centered cubic lattice, and the length of the edge of a unit cell is 305 pm. what is the density of V?
Iron crystallizes in a body-centered cubic lattice. Calculate the density of Fe if the edge of a unit cell is 307 pm. A. 12.8 g/cm3 B. 6.40 x 106 g/cm3 C. 8.26 g/cm3 D. answer not listed E. 8.72 g/cm3 F. 7.84 g/cm3 G. 6.41 g/cm3
Gold crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?407 pm204 pm288 pm333 pm
Barium metal (d = 3.51 g/cm³) has a body-centered cubic structure. Calculate the edge length of a unit cell. (1 m = 10¹² pm)
Barium metal (d = 3.51 g/cm³) has a body-centered cubic structure. Calculate the edge length of a unit cell. (1 m = 10¹² pm)
An unknown element crystallizes in a face-centered cubic lattice and it has a density of 1.45 g/cmº. The edge of its unit cell is 4.52 x10-8 cm and there are 4 atoms in one cell. Calculate the molar mass of the atom. 20.2 g/mol 9.59 g/mol 80.8 g/mol Oo 13.9 none of the answers given are correct
Iridium crystallizes in a face-centered cubic unit cell that has an edge length of 3.833 Å. The atom in the center of the face is in contact with the corner atoms, as shown in the drawing. Part A Calculate the atomic radius of an iridium atom. Express your answer using four significant figures. Part B Calculate the density of iridium metal. (Figure 1) Express your answer using four significant figures.