16:I[8216,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"BackButton"] 17:I[1553,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"QuestionViewer"] 15:T513,{"@context":"https://schema.org","@type":"Quiz","name":"Mht Cet 2024 Solid State PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/mht-cet/questions/2024/chemistry/solid-state/m3txgof7","educationalLevel":"Entrance exam preparation","about":"Mht Cet / Chemistry / Solid State","hasPart":{"@type":"Question","name":"Mht Cet 2024 Solid State PYQ with Solution","text":"Calculate the volume of unit cell of an element having molar mass 27 \\mathrm{~g} \\mathrm{~mol}^{-1} that forms fcc unit cell. \\left[\\rho . \\mathrm{N}_{\\mathrm{A}}=16.0 \\times 10^{23} \\mathrm{~g} \\mathrm{~cm}^{-3} \\mathrm{~mol}^{-1}\\right]","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"B"},"comment":{"@type":"Comment","text":"The density (\\rho) of a unit cell is given by: \\rho = \\frac{Z \\times M}{N_A \\times a^3} where: Z is the number of atoms per unit cell. For a face-centered cubic (fcc) unit cell, Z = 4. M is the molar mass of the element (given as 27 g/mol). N_A is Avogadro's number (6.022 \\times 10^{23} \\text{ mol}^{-1}). a is the edge length of the unit cell. a^3 represents the volume of the unit cell. We are given that \\rho \\times N_A = 16.0 \\times 10^{23} \\text{ g cm}^{-3} \\text{ mol}^{-1}. We can rearrange..."}}}18:T460,

The density ($\rho$) of a unit cell is given by:

$$\rho = \frac{Z \times M}{N_A \times a^3}$$

where:

$Z$ is the number of atoms per unit cell. For a face-centered cubic (fcc) unit cell, $Z = 4$.

$M$

Solid State

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