In the relationship between `deltag` and k for a given reaction, if `deltag` is negative, what is k?

Consider a hypothetical reaction:

A ↔ B

The change in free energy, ΔG can be related to the equilibrium constant K as:

ΔG = -RT ln K

i.e.   K = exp (-ΔG/RT)

When ΔG is negative, the exponential becomes positive which results in a high value of the equilibrium constant (K).  More and more of the reactants get converted into products and the reaction tends to be spontaneous.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.