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MHT CET202611 April 2026Morning ShiftChemistryThermodynamics (C)Actual

Calculate the work done when 1 mole of an ideal gas is expanded reversibly and isothermally from initial pressure 10 bar to final pressure 1 bar at constant temperature 300 K. [ R = 8.314 J K ⁻¹ mol ⁻¹ ]

Options

  1. A-5.744 kJ
  2. B-5.123 kJ
  3. C-6.514 kJ
  4. D-4.981 kJ

Correct answer

A. -5.744 kJ

Step-by-step solution

For a reversible isothermal expansion of an ideal gas, the work done is given by the formula: W = -2.303 nRT ₁₀ ( P₁ P₂ ) Given: n = 1 mol R = 8.314 J K ⁻¹ mol ⁻¹ T = 300 K P₁ = 10 bar P₂ = 1 bar Substituting the values into the formula: W = -2.303 1 8.314 300 ₁₀ ( 10 1 ) W = -2.303 2494.2 1 W = -5744.14 J W = -5.744 kJ

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