"How fast" and "how far" are answered by completely different things. A reaction can be overwhelmingly favorable at equilibrium and still be too slow to ever actually get there.
It feels natural to assume that a reaction which "wants" to happen — one with a large, favorable equilibrium constant — must also happen quickly. It doesn't follow. Whether a reaction proceeds to completion and how quickly it gets there are governed by two entirely separate branches of chemistry, calculated from entirely separate quantities, and a reaction can score at opposite extremes on each one at the same time. Diamond sitting on a table at room temperature is the standard proof: thermodynamics has already decided the outcome, and kinetics has decided you will never see it happen.