Tony Stark was investigating the properties of the Vibranium in Captain America's Shield. He found that Vibranium formed a cubic closest packed (ccp) structure with a edge length of 197.3 pm and density of 31.20 g cm ³. Determine the molar mass of Vibranium in g mol 1. Report your answer to 2 decimal places. Your Answer: Answer units

Tony Stark was investigating the properties of the Vibranium in Captain America's Shield. He found that Vibranium formed a cubic closest packed (ccp) structure with a edge length of 197.3 pm and density of 31.20 g cm ³. Determine the molar mass of Vibranium in g mol 1. Report your answer to 2 decimal places. Your Answer: Answer units

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 150CP: Spinel is a mineral that contains 37.9% aluminum, 17.1% magnesium, and 45.0% oxygen, by mass, and...

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Spinel is a mineral that contains 37.9% aluminum, 17.1% magnesium, and 45.0% oxygen, by mass, and has a density of 3.57 g/cm3.The edge of the cubic unit cell measures 809 pm. How many of each type of ion are present in the unit cell?
What factors affect the viscosity of a substance? Which of the following substances, water (H2O), ethanol (CH3CH2OH), ethylene glycol (HOCH2CH2OH), and glycerol (HOCH2CH(OH)CH2OH), is expected to have the highest viscosity? Should viscosity of a substance be affected by temperature? Explain your answers.
The surface tension and viscosity of water at several different temperatures are given in this table. Water Surface Tension (mN/m) Viscosity (mPa s) 0 C 75.6 1.79 20 C 72.8 1.00 60 C 66.2 0.47 100 C 58.9 0.28 (a) As temperature increases, what happens to the surface tension of water? Explain why this occurs, in terms of molecular interactions and the effect of changing temperature. (b) As temperature increases, what happens to the viscosity of water? Explain why this occurs, in terms of molecular interactions and the effect of changing temperature.
Nanotechnology, or technology utilizing 1100 nm sized particles, has rapidly expanded in the past few decades, with potential applications ranging across far-reaching fields such as electronics, medicine, biomaterials, and consumer products, to name a few. One of the primary advantages of nanoparticles is the presence of large surface/mass ratios, resulting in enhanced surface activities compared to bulk materials. a Use the density of silver (10.49 g/cm3) to determine the number of Ag atoms in a spherical 20.-nm silver particle. b In the crystalline metallic environment, the measured radii of silver atoms has been measured to be 144 pm. Use this to calculate the atomic packing fraction of a 20.-nm silver particle. In other words, calculate the ratio of the volume taken up by Ag atoms to the volume of the entire nanoparticle. c Based on the result of part (b), silver conforms to which type of cubic crystal lattice? A simple cubic B body-centered cubic C face-centered cubic d A cubic Ag ingot having a mass of 5.0-g is processed to form a batch of 20.-nm Ag nanoparticles. Calculate the ratio of the surface area provided by the batch of nanoparticles to the surface area of the initial cube of Ag.
8.61 Distinguish between a block copolymer and a graft copolymer.
Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a compound based on this pattern?
Iridium metal, Ir, 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 iridium is 22.42 g/cm3. Calculate the mass of an iridium atom. Use Avogadros number to calculate the atomic mass of iridium.
Consider the three types of cubic units cells. (a) Assuming that the spherical atoms or ions in a primitive cubic unit cell just touch along the cubes edges, calculate the percentage of occupied space within the unit cell. (Recall that the volume of a sphere is (4/3)r3, where r is the radius of the sphere.) (b) Compare the percentage of occupied space in the primitive cell (pc) with the bcc and fcc unit cells. Based on this, will a metal in these three forms have the same or different densities? If different, in which is it most dense? In which is it least dense?
The solid-state structure of silicon is shown below. Unit cell for silicon (a) Describe this crystal as pc, bcc, or fcc. (b) What type of holes are occupied in the lattice? (c) How many Si atoms are there per unit cell? (d) Calculate the density of silicon in g/cm3 (given that the cube edge has a length of 543.1 pm). (e) Estimate the radius of the silicon atom. (Note: The Si atoms on the edges do not touch one another.)
The structures of some common crystalline substances are shown below. Show that the net composition of each unit cell corresponds to the correct formula of each substance.