ThermodynamicsHard
Question
Each of the vessels 1 and 2 contain 1.2 moles of gaseous helium. The ratio of the volume of vessels is V2/V1 = 2.0, and the ratio of the absolute temperature of helium in them is T1/T2 = 2.0. Assuming the gas to be ideal, find the difference of gas entropies in these vessels, S2 – S1 (ln 2 = 0.7).
Options
A.0.84 cal/K
B.4.2 cal/K
C.−0.84 cal/K
D.−4.2 cal/K
Solution
$S_{2} - S_{1} = n.C_{V,m}.\ln\frac{T_{2}}{T_{1}} + nR.\ln\frac{V_{2}}{V_{1}}$
$1.2 \times \frac{3R}{2} \times \ln\frac{1}{2} + 1.2 \times R \times \ln 2 = - 0.84\text{ Cal/K}$
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