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 2.16QP
To determine
Calculate the density of iron.
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Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight of 55.85 g/mol. Compute its theoretical density.
7.87
g/cm³
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.
A pure titanium cube has an edge length of 2.74 inin . How many titanium atoms does it contain? Titanium has a density of 4.50g/cm34.50g/cm3.
Express your answer in atoms to three significant figures.
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, civil-engineering and related others by exploring similar questions and additional content below.Similar questions
- Calculate 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 BCC metal with an atomic mass of 63.5 g/mole and atomic radius of 0.128 nm.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
- Two hypothetical metals are created with different elements that have thesame 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_forwardCalculate 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 63.55g/molarrow_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
- 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_forwardNumber 1arrow_forwardDraw a bar diagram on your sketch paper based on the table below and determine the non-carbon hardness (permanent hardness) in mg/L of CaCO3. Atomic weight Equivalent weight or molecular Concentration (mg/L) meq/L concentration (mg/meq) weight (g/mol) 100 Ca2+ 40 150 mg/L as CaCO3 150/50=3 (g/mol)/2(eq/mol)=50 Mg2+ 24 100 mg/L as CACO3 100/50=2 Na+ 23 46 mg/L K+ 39 39 mg/L HCO3 61 225 mg/L as CaCO3 225/50=4.5 SO42- 96 72 mg/L CI 35.5 71 mg/L O 25 mg/L of CaCO3 O 50 mg/L of CaCO3 O 100 mg/L of CaCO3 O 150 mg/L of CaCO3arrow_forward
- Calculate 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_forwardConsidering an alloy of the two soluble components A and B described by a phase diagram Figure P2.31, determine the masses of the alloy that are in the liquid and solid phases at a given temperature if the total mass of the alloy is 100 g, component B represents 60% of the alloy, 25% of the liquid is component B, and 70% of solid is component B.arrow_forwardUsing the information available in Table 2.3, calculate the density of molyb-denum given that it has an atomic mass of 95.94 g/mole.arrow_forward
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