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JEE Main202622 January 2026Morning ShiftChemistryThermodynamics (C)Actual

Match the List-I with List-II ( array |c|l|c|c| & List-I (Thermodynamic Process) & & List-II & & & (Magnitude in kJ) A. & array l Work done in reversible, isothermal expansion of 2 mol ideal gas from 2 , dm ^3 to 20 , dm ^3 at 300 , K array & I. & 4 B. & array l Work done in irreversible isothermal expansion of 1 mol ideal gas from 1 , m ^3 to 3 , m ^3 at 300 , K against constant pressure 3 , kPa array & II. & 11.5 C

Options

  1. AA-II, B-III, C-I, D-IV
  2. BA-III, B-II, C-IV, D-I
  3. CA-II, B-I, C-III, D-IV
  4. DA-I, B-II, C-III, D-IV

Correct answer

A. A-II, B-III, C-I, D-IV

Step-by-step solution

Calculate each thermodynamic quantity: A. Reversible isothermal expansion (2 mol, 2→20 dm³, 300 K): W = nRT (V₂/V₁) = 2 8.314 300 (10) = 2 8.314 300 2.303 = 11,481 J ≈ 11.5 kJ → II B. Irreversible isothermal expansion (1 mol, 1→3 m³, 3 kPa constant pressure): W = P_ ext V = 3000 (3-1) = 6000 J = 6 kJ → III C. Adiabatic expansion (1 mol, T = -320 K, C_V = 3 2 R ): U = nC_V| T| = 1 3 2 8.314 320 = 3,991 J ≈ 4 kJ → I D. Enthalpy change (1 mol, T = 337 K, C_p = 5 2 R ): H = nC_p T = 1 5 2 8.314 337 = 7,016 J ≈ 7 kJ → I

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