Discover the best answers at Westonci.ca, where experts share their insights and knowledge with you. Explore a wealth of knowledge from professionals across different disciplines on our comprehensive platform. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.
Sagot :
The unit cell volume of the crystal is [tex]V_c = 9.9084*10^-^2^3 cm^3 / unit cell[/tex] and the density of titanium is calculated as 4.71g/cm^3 while the literature value is 4.5 g/cm^3
Data;
- radius = 0.1445 nm
- c/a = 1.58
- A = 46.88 g/mol
Unit Cell Volume
The unit cell volume can be calculated as
[tex]V_c = 6R^2c\sqrt{3}\\[/tex]
let's substitute the values into the formula
[tex]V_c = 6 * (1.445*10^-^8)^2 * 1.58 8 * a * \sqrt{3} \\a = 2R\\V_c = 6 * (1.445*10^-^8)^2 * 1.58* 2 * 1.445*10^-^8 * \sqrt{3}\\ V_c = 9.984*10^-^2^3 cm^3 / unit cell[/tex]
The unit cell volume of the crystal is [tex]V_c = 9.9084*10^-^2^3 cm^3 / unit cell[/tex]
Density of Ti
The density of titanium can be calculated as
[tex]\rho = \frac{nA}{V_c N_a}[/tex]
- n = 6 for hcp
- A = 46.88 g/mol
- Na = Avogadro's number
let's substitute the values into the formula
[tex]\rho = \frac{nA}{V_c Na}\\ \rho = \frac{6*46.88}{9.9084*10^-^2^3* 6.023*10^2^3} \\\rho = 4.71 g/cm^3[/tex]
The density of titanium is calculated as 4.71g/cm^3 while the literature value is 4.5 g/cm^3
Learn more on crystal lattice here;
https://brainly.com/question/6610542
Thanks for using our service. We aim to provide the most accurate answers for all your queries. Visit us again for more insights. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. We're glad you visited Westonci.ca. Return anytime for updated answers from our knowledgeable team.
