ThermodynamicsHard
Question
An amount of 2 mole of CO was in the small cubical container of length (l = a) at 57°C. The gas was taken out completely from the small container and put into large container (l = 2a) at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal gas?
Options
A.34.58 J/K
B.– 34.58 J/K
C.−11.53 J/K
D.+11.53 J/K
Solution
$\Delta S = nR.\ln\frac{V_{2}}{V_{1}} = 2 \times 8.314 \times \ln\frac{(2a)^{3}}{a^{3}} = 34.58\text{ J/K}$
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