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Question Bank: Thermodynamics
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FAQs on Question Bank: Thermodynamics
| 1. What's the difference between enthalpy and internal energy in thermodynamics? |  |
Ans. Enthalpy (H) is the total heat content of a system at constant pressure, while internal energy (U) represents the total energy stored within molecules. The relationship is H = U + PV. Enthalpy measures heat released or absorbed during chemical reactions, making it essential for calculating energy changes in exothermic and endothermic processes studied in CBSE Class 11 Chemistry.
| 2. How do I know if a reaction is spontaneous using Gibbs free energy? | |
Ans. A reaction is spontaneous when Gibbs free energy (ΔG) is negative. The formula ΔG = ΔH - TΔS shows that spontaneity depends on enthalpy change, entropy change, and temperature. When ΔG < 0, the reaction proceeds forward naturally; when ΔG > 0, it's non-spontaneous. This concept helps predict whether chemical processes occur automatically or require external energy input.
| 3. Why is entropy important in thermodynamics and how does it relate to disorder? | |
Ans. Entropy (S) quantifies the degree of randomness and disorder in a system. The second law of thermodynamics states that entropy of the universe always increases during spontaneous processes. Higher entropy means particles are more disorganised; lower entropy indicates an organised state. Understanding entropy changes helps explain why certain reactions favour products and why energy transformations are never 100% efficient.
| 4. What does the first law of thermodynamics actually mean for chemical reactions? | |
Ans. The first law states that energy cannot be created or destroyed, only converted from one form to another: ΔU = q + w (change in internal energy equals heat absorbed plus work done). In chemical reactions, this means total energy before and after remains constant. Breaking and forming bonds releases or absorbs energy, but the total energy of an isolated system remains unchanged, fundamental to understanding reaction mechanisms.
| 5. How can I quickly identify exothermic versus endothermic reactions in exam questions? | |
Ans. Exothermic reactions release heat (ΔH negative, products have lower energy than reactants), while endothermic reactions absorb heat (ΔH positive, products have higher energy). Look for keywords: combustion, neutralisation, and freezing are typically exothermic; melting, evaporation, and decomposition are endothermic. Recognising these patterns and using ΔH sign conventions helps answer thermodynamic questions accurately during NEET preparation and board examinations.
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Document Description: Question Bank: Thermodynamics for NEET 2026 is part of Chemistry Class 11 preparation. The notes and questions for Question Bank: Thermodynamics have been prepared according to the NEET exam syllabus. Information about Question Bank: Thermodynamics covers topics like and Question Bank: Thermodynamics Example, for NEET 2026 Exam. Find important definitions, questions, notes, meanings, examples, exercises and tests below for Question Bank: Thermodynamics.
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