To show that entropy is not the same thing as disorder (what people intuitively accept as disorder) my textbook gives an example of crystallization in a supersaturated solution. And it argues that since both temprature and disorder decrease the entropy must decrease also, but it does not. Hence giving a contradiction to the disorder interpretation: Unlike what the book says, in reality the entropy must decrease because no such system is truly isolated. Right? Also, doesn't the 2nd law say that entropy only tends to increase in an isolated system (it can decrease locally within an isolated system)? So, wouldn't stacking some coins would have sufficed as example? So why give this example in particular?