Materials for Civil and Construction Engineers (4th Edition)
4th Edition
ISBN: 9780134320533
Author: Michael S. Mamlouk, John P. Zaniewski
Publisher: PEARSON
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Chapter 2, Problem 2.20QP
To determine
Calculate the density of aluminum.
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Express your answer in atoms to three significant figures.
Calculate the radius of the copper atom, given that copper has an FCC crystal structure, a density of 8.89 g/cm3, and an atomic mass of 63.55 g/mole.
Chapter 2 Solutions
Materials for Civil and Construction Engineers (4th Edition)
Ch. 2 - Define elastic and plastic behaviors at the micro...Ch. 2 - Prob. 2.2QPCh. 2 - Prob. 2.3QPCh. 2 - Describe the order in which electrons fill the...Ch. 2 - Prob. 2.5QPCh. 2 - Why do atoms maintain specific separations?Ch. 2 - Prob. 2.7QPCh. 2 - Prob. 2.8QPCh. 2 - Prob. 2.9QPCh. 2 - Two hypothetical metals are created with different...
Ch. 2 - Prob. 2.11QPCh. 2 - Prob. 2.12QPCh. 2 - Prob. 2.13QPCh. 2 - Prob. 2.14QPCh. 2 - Prob. 2.15QPCh. 2 - Prob. 2.16QPCh. 2 - Prob. 2.17QPCh. 2 - Determine the density of a hypothetical BCC metal...Ch. 2 - Determine the density of a hypothetical FCC metal...Ch. 2 - Prob. 2.20QPCh. 2 - Prob. 2.21QPCh. 2 - Prob. 2.22QPCh. 2 - Prob. 2.23QPCh. 2 - Prob. 2.24QPCh. 2 - Prob. 2.25QPCh. 2 - Prob. 2.26QPCh. 2 - Prob. 2.27QPCh. 2 - Prob. 2.28QPCh. 2 - Prob. 2.29QPCh. 2 - Prob. 2.30QPCh. 2 - Prob. 2.31QPCh. 2 - Prob. 2.32QPCh. 2 - Prob. 2.33QPCh. 2 - Prob. 2.34QPCh. 2 - Prob. 2.35QPCh. 2 - Prob. 2.36QP
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- Question 6 (of 8) 6. The density of platinum is 21500 kg/m³ and that of aluminum is 2702 kg/m³. Find the ratio of the volume of 1.80 kg of platinum to the volume of 1.17 kg of aluminum.arrow_forwardUsing the information available in Table 2.3, calculate the volume of the unit cell of copper in cubic meters.arrow_forwardLead has one of the highest densities of all the pure metals at 11,240 kg/m^3. What is the density of Lead in units of Lin/in^3?arrow_forward
- The density (mass>volume) of aluminum is 5.26 slug/ft3. Determine its density in SI units. Use an appropriate prefix.arrow_forwardCalculate the volume of the unit cell of iron in cubic meters, given that iron has a body-center cubic crystal structure and an atomic radius of 0.124 nm.arrow_forwardDetermine the density of a hypothetical FCC metal with an atomic mass of 42.9 g/mole and atomic radius of 0.132 nm.arrow_forward
- At a temperature of 60°F, a 0.04 in. gap exists between the ends of the two bars shown in the figure. Bar (1) is an aluminum alloy [E=10000 ksi; v=0.32; a= 12.5 x10^-6/,°F] bar with a width of 3 in. and a thickness of 0.75 in. Bar (2) is a stainless steel [E= 28000 ksi; v=0.12; a=9.6x10^-6/°F] bar with a width of 2 in and a thickness of 0.75 in. The supports at A and C are rigid. Determine the normal stress in bar (1) at a temperature of 380°F. Answer in ksiarrow_forwardGiven that the density of aluminum is 5.26 slugs per cubic feet. Determine its density in SI units.arrow_forwardTwo hypothetical metals are created with different elements that have the same atomic mass (g/mole) and the same atomic radius. Metal A has a density of 9.50 g/cm3 and metal B has a density of 8.73 g/cm3. If one of these metals has a BCC lattice structure and the other has an FCC lattice structure, identify the structure that corresponds to each of one of them. Justify your answer.arrow_forward
- Question 18 True or false: A covalent bond in a molecule is tougher than a hydrogen bond. Select one: O True Falsearrow_forwardCalculate the radius of the aluminum atom, given that aluminum has an FCC crystal structure, a density of 2.70 Mg/m3 , and an atomic mass of 26.98 g/mole. Note that the APF for the FCC lattice structure is 0.74.arrow_forwardCopper has an atomic radius of 0.128 nm (1.28A°), an FCC crystal structure, and an atomic weight of 63.5 g/mol. Compute its theoretical density?arrow_forward
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