1. If ∆G is negative, then the reaction is spontaneous and proceeds in the forward direction.
If ∆G is positive, then reaction is considered non- spontaneous. instead, as reverse reaction would have a negative ∆G, the products of the forward reaction shall be converted to the reactants. If ∆G is 0, reaction has achieved equilibrium. At this point, there is no longer any free energy to drive the reaction.
2. ∆G⊖ = -2.303RT log K
= -2.303 x 8.134 x 300 x log K
= -2.303 x 8.134 x 300 x log 8
= 5187.5 mol-1