### The overall change in Entropy

Posted: **Wed Feb 14, 2018 12:26 am**

by **Sophia Kim 1C**

In section 9.10 in the textbook it states that since deltaU = q+w it follows that q rev must be greater than q irrev because only than can the sums of q and w be the same for the two paths. Can someone explain what that means?

### Re: The overall change in Entropy [ENDORSED]

Posted: **Wed Feb 14, 2018 9:56 am**

by **Chem_Mod**

Not only does q_{rev} need to be greater than q_{irrev} but also for w_{rev} must be greater than w_{irrev}. Note that here we mean greater in absolute terms, you must consider the signs depending on whether work is done by or work is done on the system. This is simply because following the reversible path gives you the maximum amount of work a system can do or have done on it.

Since the change in internal energy U is a state function, it should be same for whether an irreversible or reversible path was taken. Try solving for q and w in the reversible and irreversible case between the same two states of a gas (T, V, n, P) to confirm this and develop your intuition.