Each of the vessels 1 and 2 contain 2.0 moles of gaseous helium. The ratio of the vessel volumes is V₂/V₁ = 2.0, and the ratio of the absolute temperatures of helium in them is T₁/T₂ = 2.0. Assuming i

Question

Each of the vessels 1 and 2 contain 2.0 moles of gaseous helium. The ratio of the vessel volumes is V₂/V₁ = 2.0, and the ratio of the absolute temperatures of helium in them is T₁/T₂ = 2.0. Assuming ideal behaviour, find the difference of gas entropies in these vessels, S₂ − S₁. (ln 2 = 0.7)

TestHub · Accepted Answer

S₂ − S₁ = nCᵥ,ₘ ln(T₂/T₁) + nR ln(V₂/V₁) = 2 × (3R/2) × (−ln 2) + 2R ln 2 = 2R ln 2 (1 − 1.5) = −R ln 2 = −2 × 0.7 = −1.4 cal/K. Matches (a).

Chemistry - Thermodynamics - II Question with Solution | TestHub

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