I learned about the equilibrium constant. Now, I've seen that the equilibrium constant of burning is extremely small $(K \ll 1)$. here, I have a question. you see, $K$ is still NOT 0, which means that the forward reactions happen at least a tiny bit. Then, shouldn't we see some parts of anything burning at least a little bit?
shouldn't I be able to observe this tiny bit of combustion happening at room temperature? if $K$ is extremely small but not 0, I don't understand it.

In general, I've always wondered why we don't see small amounts of reactions happening spontaneously since the equilibrium constant isn't 0.

There's the concept of a "threshold energy", but it seems a bit arbitrary and not well-defined.
Even if the concentration of product is extremely low compared to the reactants, shouldn't we observe something? Am I missing something?

Comment: The fact that there will always be some small reaction happening doesn't mean that you will see it or be able to detect it. The equilibrium constant $K$ is the ratio of the reaction rates of the forward and reverse reactions under equilibrium conditions. In the case of reactions with $K \ll 1$, the reverse reaction is much faster