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The work done by the system W (taken as positive when the system does work on the surroundings) for the isothermal reversible expansion of 1 mole of an ideal gas, from an initial pressure of 1.0 bar…

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The work done by the system W (taken as positive when the system does work on the surroundings) for the isothermal reversible expansion of 1 mole of an ideal gas, from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at constant temperature of 273 K is
  1. −5227 J
  2. +5227 J
  3. +4880 J
  4. −4880 J

Answer and explanation

Correct answer: B - +5227 J
Wby system=nRTln⁡(P1/P2)=1×8.314×273×ln⁡10=1×8.314×273×2.303≈5227W_{\text{by system}} = nRT\ln(P_1/P_2) = 1 \times 8.314 \times 273 \times \ln 10 = 1 \times 8.314 \times 273 \times 2.303 \approx 5227 J. With work done by the system counted as positive, W=+5227W = +5227 J.

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