Decomposition of ammonia to nitrogen and hydrogen equation

1.	Decomposition of ammonia to nitrogen and hydrogen equation
Answer» In CHEMICAL kinetics , we learn that in a reversible reaction ,both the forward reaction and reverse reaction OCCUR at the same time. At equilibrium , the rates are the same. For example:Production of AMMONIA NH3 .During the production of ammonia both the forward & reverse reaction is present . 3H2(g)+N2(g)⟶2NH3(g)3HX2(g)+NX2(g)⟶2NHX3(g) forward reaction 2NH3(g)⟶3H2(g)+N2(g)2NHX3(g)⟶3HX2(g)+NX2(g) reverse reaction Now come to the Gibbs free energy. Under standard condition(298K) , it can be calculated that the reaction is forwardly favored (forward reaction is spontaneous,and thus the decomposition of NH3 is non-spontaneous). I UNDERSTAND H2 and N2 will produce more NH3.My question is at this situation will NH3 decompose into H2 and N2 to some EXTENT(though it is a non-spontaneous process)?.But chemical kinetics tells that both reaction(not necessarily same rate) have to be present to create equilibrium in future.

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