Two moles of an ideal gas undergo free expansion from 10 L to 100 L at 300 K. The values of S_ system and S_ surroundings are (R is universal gas constant)

Step-by-step solution

For the free expansion of an ideal gas, the external pressure is zero, so the work done W = 0 . Since the process is isothermal at 300 K, the change in internal energy U = 0 . From the first law of thermodynamics, q = U - W = 0 . Since no heat is exchanged with the surroundings, the change in entropy of the surroundings is: S_ surroundings = q_ surr T = 0 Entropy is a state function, so the change in entropy of the system for an isothermal expansion is calculated using a reversible path between the same initial and