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:T50a,{"@context":"https://schema.org","@type":"Quiz","name":"Mht Cet 2023 Solid State PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/mht-cet/questions/2023/chemistry/solid-state/jaoe38c1lr50yx90","educationalLevel":"Entrance exam preparation","about":"Mht Cet / Chemistry / Solid State","hasPart":{"@type":"Question","name":"Mht Cet 2023 Solid State PYQ with Solution","text":"Calculate the density of metal having molar mass 210 \\mathrm{~g} \\mathrm{~mol}^{-1} that forms simple cubic unit cell. \\left(\\mathrm{a}^3 \\cdot \\mathrm{N}_{\\mathrm{A}}=21.5 \\mathrm{~cm}^3 \\mathrm{~mol}^{-1}\\right)","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"A"},"comment":{"@type":"Comment","text":"The density (ρ) of a simple cubic unit cell is calculated using: \\rho = \\frac{Z \\cdot M}{a^3 \\cdot N_A} Where: Z = Number of atoms per unit cell (1 for simple cubic) M = Molar mass of the metal (g/mol) a = Edge length of the unit cell (cm) N_A = Avogadro's Number (6.022 x 10²³ mol⁻¹) Finding the Edge Length (a): a^3 = \\frac{21.5 \\mathrm{~cm}^3 \\mathrm{~mol}^{-1}}{N_A} a^3 = \\frac{21.5 \\mathrm{~cm}^3 \\mathrm{~mol}^{-1}}{6.022 \\times 10^{23} \\mathrm{~mol}^{-1}} a^3 = 3.57 \\times 10^{-23} \\mathrm{..."}}}18:T419,

The density (ρ) of a simple cubic unit cell is calculated using:

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

Where:

$Z$ = Number of atoms per unit cell (1 for simple cubic)

$M$ = Molar mass of the metal (

Solid State

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