Enter your answer to 3 significant figures.  If the atomic radius of palladium is 0.137 nm, calculate the volume of its unit cell in cubic nanometers.  Hint: you will need the crystal structure of palladium. I got 0.058 the first time and it was wrong

A pure metallic solid has an atomic radius of 1.9 Angstrom, an FCC crystal structure and has a density of 9.72 g/ml. Calculate its molar mass in g/mol. Round your answer to 0 decimal places Please answer the question ASAP. I need the answer in 35min. Thank you.

Rhodium has a density of 12.41 g/cm3 and crystallizes with the face-centered cubic unit cell. Calculate the radius of a rhodium atom in cm. Please input your answer in scientific notation using the format 5.9x10^7 (do not include any spaces). Do not include units in your answer. type your answer...

At room temperature, the edge length of the cubic unit cell in elemental silicon is 5.431 Å, and the density of silicon at the same temperature is 2.328 g cm-3 . Each cubic unit cell contains eight silicon atoms. Using only these facts, perform the following operations.(a) Calculate the volume (in cubic centimeters) of one unit cell.(b) Calculate the mass (in grams) of silicon present in a unit cell.(c) Calculate the mass (in grams) of an atom of silicon.(d) The mass of an atom of silicon is 28.0855 u. Estimate Avogadro’s number to four significant figures.

Tungsten B is a solid phase of tungsten still unknown to science. The only difference between it and ordinary tungsten is that Tungsten B forms a crystal with an fcc unit cell and a lattice constant a=0.387 nm. Calculate the density of Tungsten B. Round your answer to 3 significant digits. 0 g cm 3 x10 Ś

Number 1-8

PLEASE double and triple check your answers and help me with all the parts. There are two parts attached as 2 screenshots.

KCl has the same crystal structure as NaCl (fcc). a) Calculate the volume  of the unit cell for KCl, given that the ionic radii are K+ = 152 pm and Cl- = 167 pm. b) Compute the density of KCl.  Show your work.   Note: pc: 1 atom/unit cell bcc: 2 atoms/unit cell fcc: 4 atoms/unit cell  1 pm = 1 x 10-10 cm Primitive Cubic (pc): 2 x (atomic radius) = edge Face-Centered Cubic: 4 x (atomic radius) = edge x √2 = face diagonal Body-Centered Cubic: 4 x (atomic radius) = edge x √3 = body diagonal   Mass of 1 formula unit (ex. NaCl) x # of formula units per unit cell (ex. 4) = mass of unit cell Mass of unit cell ÷ unit cell volume ( ex. = edge3 for NaCl) = density

Assume the edge length of the unit cell for tantalum is 331 pm. Calculate the volume of this unit cell in cm³. Remember, there are 1.00x10¹⁰ pm per 1.00 cm. Calculate the mass in grams of this unit cell. Submit an answer with three significant figures. (Molar mass of tantalum = 180.95 g/mol) Calculate the density of this unit cell in g/cm³.

A hypothetical metal has a tetragonal unit cell for which the lattice parameters (in nm) are a=b=0.550, c=0.673 and all angles are 90 degrees. If there are 5 atoms per unit cell and the atomic packing factor is 0.63, determine the atomic radius in nm. Use 3.14 for pi. Give your answer to 3 decimal places. I got 0.197 the first time and it was incorrect.