2nd Law of Thermodynamics I understand that the 2nd law of thermodynamics roughly states that, if you have a body (or a gas in a chamber) that is hot at one end and cold on the other, the heat will always flow from the hot to the cold part and to get the opposite effect, one has to put energy in from the outside (through a machine or something).
Now, I don't understand why this fact cannot be explained just through probabilities (of the velocities of the gas molecules, say). 
It would seem to me that it is simply very, very, very unlikely that faster moving molecules all end up in (approximately) one spot at any time.
But from all the fuzz about the 2nd law, I'm led to believe that there has to be more behind it than probability. So where am I wrong? Why is the second law beyond probability? How is the 2nd law tested? (so that one can rule out simple probability?)
ps.: I haven't yet had a course on probability theory. So my understanding of it is limited.
 A: It's very, very unlikely that heat should flow from cold to hot, for values of "very very unlikely" involving extremely large powers of ten. We're talking monkeys-with-typewriters-writing-Shakespeare kind of unlikely.
There's a very good, largely nonmathematical discussion of the second law and entropy in Sean Carroll's From Eternity to Here, which discusses entropy in detail in the context of the "arrow of time." It's a very good treatment of the subject, and well worth reading.
A: I also found that with modern computers with about a days effort, I could write a 2D kinetic particle simulation code. Collide two particles, and conservation of energy and momentum leaves only a single undetrmined quantity, which I simply set by using a random number generator. Throw in a few hundred or thousand particles, and you can see how the system evolves, and what sort of statistical properties emerge. This allows someone who isn't really good at math, but good at programming to design numerical experiments. I postulate that if these tools had been available when the subject was first researched that if would have developed much quicker.
A: I assure you, it is all probability AND statistics.
Well you see when you say "a gas is at 300 Kelvin", then it does not mean all the molecules in the gas are "at 300 Kelvin", it rather states an average. It represents the total behavior of the gas compared to anything at any other temperature. So there are actually molecules with more kinetic energy, and those with less kinetic energy, interacting with each other and the environment they are in, however due to the massive number of collisions and interactions, the result with highest probability(i.e. same temperature box&gas stays at the same temperature) is the macroscopic outcome.
Probability, combined with statistics is a very powerful tool to represent macroscopic nature, and I suggest you to take probabilistic maths and statistical thermodynamics courses to further investigate such issues.
A: I belief that when the 2nd law of thermodynamics is stated carefully in the right way it becomes a total no-brainer, i.e., just plain obvious. 
The only concept you have to know about is that of macro- and micro-states:
A micro-state is a state that characterizes position/velocity of each and every molecule in your gas, or, more general, the exact state of the system.
A macro state is a collection of many micro-states that share a common characteristic. For example, there are many ways you can arrange the molecules of a gas and still have the same volume, temperature and pressure. The number of micro-states that make up a given macro-state is called multiplicity
The 2nd law of thermodynamics simply states that over the course of time, multiplicity will increase: Macro-states with more micro-states are more probable than macro-states with fewer micro-states.
A: The second law of thermodynamics is about more than probability because physics does not discriminate between the past and the future. It's called Loschmidt's Paradox, and it remains unresolved.
A: To show that you can't change a gas in a closed container that's a uniform temperature to a nonuniform temperature without an external source of Gibbs free energy, you have to assume the second law of thermodynamics from which the zeroth law follows. According to Has the zeroth law of thermodynamics ever been proven?, the zeroth law probably hasn't been proven. Two gases can never be immiscible with each other because any two gases will mix in any proportion. If you have a gas and two immiscible liquids all in contact with one another in an isolated system and the zeroth law turns out to be false, maybe the gas and the two liquids will never form a thermal equilibrium and heat will be flowing in circles between the gas and the two liquids.
