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:T504,{"@context":"https://schema.org","@type":"Quiz","name":"Mht Cet 2025 Thermodynamics PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/mht-cet/questions/2025/chemistry/thermodynamics/merjlz2l","educationalLevel":"Entrance exam preparation","about":"Mht Cet / Chemistry / Thermodynamics","hasPart":{"@type":"Question","name":"Mht Cet 2025 Thermodynamics PYQ with Solution","text":"Calculate the entropy change of surrounding if 2 moles of \\mathrm{H}_2 and 1 mole of \\mathrm{O}_2 gas combine to form 2 moles of liquid water by releasing 525 kJ heat to surrounding at constant pressure and at 300 K .","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"B"},"comment":{"@type":"Comment","text":"Given: q = 525~\\text{kJ} heat is released (exothermic process, so q = -525~\\text{kJ}) T = 300~\\text{K} Pressure is constant. Step 1: Entropy change of surroundings (\\Delta S_{\\text{surroundings}}) is calculated by: \\Delta S_{\\text{surroundings}} = \\frac{q_{\\text{surroundings}}}{T} Since heat is released by the system, the same amount of heat is gained by the surroundings. So, q_{\\text{surroundings}} = +525~\\text{kJ} = 525,000~\\text{J} Step 2: Substitute the values: \\Delta S_{\\text{surroundings}..."}}}18:T427,

Given:

$q = 525~\text{kJ}$ heat is released (exothermic process, so $q = -525~\text{kJ}$)
$T = 300~\text{K}$
Pressure is constant.

Step 1: Entropy change of surroundings

Thermodynamics

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