Given the following standard potentials in basic solution

and assuming that a reversible reaction can be established on a suitable catalyst, calculate E^⦵, Δ_rG^⦵, and K for the reductions of

(a) CrO₄²⁻ 

(b) [Cu(NH₃)₂]⁺ in basic solution. Comment on why Δ_rG^⦵ and K are so different between the two cases despite the values of E^⦵ being so similar.

CrO2 (aq) + 4HO(l) + 3e Cr(OH), (s) + 5OH- (aq) E = -0.11 V [Cu(NH)](aq) + eCu(s) + 2NH (aq) E* = -0.10 V