An ideal gas undergoes an isothermal change of volume. The initial and final yolumes are given to be 1 litre and 2.7 litres respectively. If in this process the entropy per mole changes from S1 to S2 The value of differences S2-S1, is nearest to (R is the universal gas constant)

Two moles of an ideal gas undergo an irreversible isothermal expansion fromVa=100 liters to Vb=300 liters at T=300K.(a)  What is the entropy change for this process?(b) What is the Gibbs free energy change?(c) Is this process spontaneous or not? Explain your answer.

When a metal bar is temporarily connected between a hot reservoir at Th and a cold reservoir at Tc, the energy transferred by heat from the hot reservoir to the cold reservoir is Qh. In this irreversible process, find expressions for the change in entropy of the following. (Use any variable or symbol stated above as necessary.) (a) the hot reservoir ΔSh =    (b) the cold reservoir ΔSc =    (c) the Universe ΔSU =

A box contains 100 gas molecules all released on the left side of the box. What is the initial entropy of all the gas molecules on one side? You can calculate the number of microstates (left/right distribution of molecules) possible by the equation W = N! / ( nL! * nR!,) where N is the total number of molecules and nL is the number on the left and nR is the number on the right. What is the entropy of the most disorganized distribution of gas molecules?

What is the change in entropy (in J/deg) when a 235- g piece of ice melts to water at 0 degrees Celcius?