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:T4fa,{"@context":"https://schema.org","@type":"Quiz","name":"Mht Cet 2024 Liquid Solution PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/mht-cet/questions/2024/chemistry/liquid-solution/m4cwcr7k","educationalLevel":"Entrance exam preparation","about":"Mht Cet / Chemistry / Liquid Solution","hasPart":{"@type":"Question","name":"Mht Cet 2024 Liquid Solution PYQ with Solution","text":"Calculate the molar mass of solute when 4 g of it dissolved in 1 \\mathrm{dm}^3 solvent has osmotic pressure 2 atm at 300 K . [R \\left[=0.082 \\mathrm{~dm}^3 \\mathrm{~atm} \\mathrm{~K} \\mathrm{~mol}^{-1}\\right]","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"A"},"comment":{"@type":"Comment","text":"To determine the molar mass of the solute, the van't Hoff equation for osmotic pressure can be used, which is given by: \\Pi = \\frac{n}{V}RT where: \\Pi is the osmotic pressure (2 atm), n is the number of moles of solute, V is the volume of the solution in liters (1 dm^3 = 1 L), R is the universal gas constant (0.082 dm^3 atm K^{-1} mol^{-1}), T is the temperature in Kelvin (300 K). Rearranging the formula to find n, the number of moles: n = \\frac{\\Pi V}{RT} Substitute the values into the equatio..."}}}18:T51d,

To determine the molar mass of the solute, the van't Hoff equation for osmotic pressure can be used, which is given by:

$$ \Pi = \frac{n}{V}RT $$

where:

$\Pi$ is the osmotic pressure (2 atm),

$n$ is the number of moles of so

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