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At constant pressure, V1T1 = V2T2. Initial: V1 = 4L, T1 = 300K, V2 = 6L, T2 = ?. T2 = T1×V2V1 = 300×64 = 450K. Back to 4L: T3 = T2×V3V2 = 450×46 = 300K (original temperature).
Ref: NCBI Bookshelf, Ideal Gas Law: P1V1/T1 = P2V2/T2.
Gases expand much more than solids and liquids due to their higher coefficient of volume expansion, which is temperature-dependent and significantly larger (Section 10.5). As per NCERT, applying relevant law/formula with correct units and sign convention leads to Coefficient of volume expansion. This satisfies dimensional consistency and physical conditions given, so option D is scientifically correct.
Ref: NCBI Bookshelf, Ideal Gas Law: P1V1/T1 = P2V2/T2.
Work done: w = -PΔ V = -2 × 0.5 × 101.325 = -101.325 J . Given q = 1200 J , Δ U = q + w = 1200 - 101.325 = 1098.68 ≈ 1098.7 J .
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
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