Question
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 ]
MHT CET
Chemistry
Thermodynamics (C)
2026
MHT CET 2026 (11 April Shift 1)
MHT CET Chemistry Question (2026) — Solution
Options
- A. -5.744 kJ
- B. -5.123 kJ
- C. -6.514 kJ
- D. -4.981 kJ
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 ( P_1 P_2 ) Given: n = 1 mol R = 8.314 J K ^ -1 mol ^ -1 T = 300 K P_1 = 10 bar P_2 = 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
Related: Chemistry — Thermodynamics (C) · All PYQ Banks