Chemistry, asked by Arshaquemirash9923, 1 year ago

An element with molar mass 2.7 x 10kg mol from a cubic unit cell with edge length 405 pm. If its density is 2.7 x 10 3 , what is the nature of the cubic unit cell?

Answers

Answered by ltsmeAliya
0

Answer:

Four atoms of the element are present per unit cell.

Hence, the unit cell is face-centred cubic (fcc) or cubic close-packed (ccp).  

Explanation:

It is given that density of the element, d = 2.7 × 10³ kg m^{-3}  

Molar mass, M = 2.7 × 10^{-2} kg mol^{-1}

Edge length, a = 405 pm = 405 × 10^{-12} m    = 4.05 × 10^{-10} m

Avogadro’s number, NA = 6.022 × 10^{23} mol^{-1}

Applying the relation,

d= \frac{z.M}{a^{3}.N_{A}  }

z= \frac{d.a^{3}N_{A}  }{M}

z = 2.7 × 10³ kg m^{-3} × (4.05 × 10^{-10} m)³ ×6.022 × 10^{23} mol^{-1}  ÷ 2.7 × 10^{-2} kg mol^{-1}

z = 4.004

z = 4

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