Zinc sulfide (zinc blende type, Z=4, molar mass 97.5 g mol^-1) has a unit cell edge of 541 pm. Use N_A = 6.022x10^23 mol^-1. Calculate the density in g cm^-3 (two decimals).

JEE Advanced levelNumerical answerDifficulty 3 of 3ss143

Zinc sulfide (zinc blende type, $Z = 4$ , molar mass $97.5 g mo l^{- 1}$ ) has a unit cell edge of $541 pm$ . Use $N_{A} = 6.022 \times 1 0^{23} mo l^{- 1}$ . Calculate the density in $g c m^{- 3}$ (two decimals).

Numerical answer type, answer in g/cm^3, tolerance 0.03.

Mass of the cell

= \frac{4 \times 97.5}{6.022 \times 1 0 ^{23}} = 6.476 \times 1 0^{- 22} g

. Volume

= (5.41 \times 1 0^{- 8})^{3} = 1.583 \times 1 0^{- 22} c m^{3}

ρ = 4.09 g c m^{- 3}