Aqueous Solutions of Ammonia (NH₃)and Hydrogen Cyanide (HCN)react to Produce $\leftrightarrows$

Aqueous solutions of ammonia (NH₃) and hydrogen cyanide (HCN) react to produce ammonium cyanide,(NH₄CN) according to the following equilibrium reaction.NH₃(aq) + HCN(aq) $\leftrightarrows$ NH₄⁺(aq) + CN^-(aq)
Given the following equilibrium constants,which statement best describes the reaction once equilibrium is established? (K_w = 1.01 $\times$ 10^-14)
NH₄⁺ $~~~~~~~~$ K_a = 5.6 $\times$ 10^-10
HCN $~~~~~~~~$$~ ~$ K_a = 4.0 $\times$ 10^-10

A) The reaction is product favored.
B) The reaction is reactant favored.
C) The reaction is neither product nor reactant favored.