An amount of 2 mole of CO was in the small cubical container of length, () at . The gas was taken ou — Thermodynamics and Thermochemistry Chemistry Question
Question
An amount of 2 mole of CO was in the small cubical container of length, ($l = a$) at $57^\circ\text{C}$. 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?
Answer: A
💡 Solution & Explanation
Initial volume $V_1 = a^3$, final volume $V_2 = (2a)^3 = 8a^3$. The process is isothermal expansion. $\Delta S = n R \ln\left(\frac{V_2}{V_1}\right) = 2 \times 8.314 \times \ln(8) = 16.628 \times 2.079 = 34.58 \text{ J/K}$.
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