Chemistry - Thermodynamics - I Question with Solution | TestHub
ChemistryThermodynamics - IIsothermal Process/Isobaric/IsochoricMedium2 minQB
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The equation of state for one mole of a gas is PV = RT + BP, where B is a constant, independent of temperature. The internal energy of fixed amount of gas is function of temperature only. If one mole of the above gas is isothermally expanded from 12 L to 22 L at constant external pressure of 1 bar at 400 K, then the change in enthalpy of the gas is approximately (B = 2 L/mol)
Options:
Answer:
C
Solution:
Δ U = 0 (isothermal, U = f(T)), so Δ H = Δ(PV) = Δ(RT + BP) = B Δ P. From V = RT/P + B: P1 = RT/(V1 - B), with RT = 0.083 × 400 = 33.2 L-bar, P1 = 33.2/10 = 3.32 bar and P2 = 33.2/20 = 1.66 bar. Δ P = -1.66 bar, Δ H = 2 × (-1.66) = -3.32 L-bar = -332 J. Matches (c).
Stream:JEESubject:ChemistryTopic:Thermodynamics - ISubtopic:Isothermal Process/Isobaric/Isochoric
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