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Vladimir [108]
2 years ago
11

Titanium has an HCP unit cell for which the ratio of the lattice parameters c/a is 1.58. If the radius of the Ti atom is 0.1445

nm, (a) determine the unit cell volume, and (b) calculate the density of Ti and compare it with the literature value
Chemistry
1 answer:
Karolina [17]2 years ago
8 0

The unit cell volume of the crystal is V_c = 9.9084*10^-^2^3 cm^3 / unit cell 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

<h3>Unit Cell Volume</h3>

The unit cell volume can be calculated as

V_c = 6R^2c\sqrt{3}\\

let's substitute the values into the formula

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

The unit cell volume of the crystal is V_c = 9.9084*10^-^2^3 cm^3 / unit cell

<h3>Density of Ti</h3>

The density of titanium can be calculated as

\rho = \frac{nA}{V_c N_a}

  • n = 6 for hcp
  • A = 46.88 g/mol
  • Na = Avogadro's number

let's substitute the values into the formula

\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

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;

brainly.com/question/6610542

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Discussion:

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8 0
1 year ago
What is the pressure of a gas that began at 38 torr, and 500L and is changed to occupy a volume of 677 L?
qwelly [4]

Answer:

P₂ = 28.5 torr

Explanation:

Given data:

Initial pressure = 38 torr

Initial volume = 500 L

Final volume = 677 L

Final pressure = ?

Solution:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = Initial volume

P₂ = Final pressure

V₂ = Final volume

Now we will put the vales in formula.

P₁V₁ = P₂V₂

P₂ = P₁V₁ /V₂

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P₂ = 28.5 torr

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