What Is the Equilibrium Constant for the Following Reaction $\rightleftharpoons$ HCO₂^-(aq) + HCN(aq)
and Does the Reaction Favor the Formation

What is the equilibrium constant for the following reaction,
HCO₂H(aq) + CN^-(aq) $\rightleftharpoons$ HCO₂^-(aq) + HCN(aq)
And does the reaction favor the formation of reactants or products? The acid dissociation constant, K_a, for HCO₂H is 1.8 × 10^-4 and the acid dissociation constant for HCN is 4.0 × 10^-10.

A) K = 1.00. The reaction favors neither the formation of reactants nor products.
B) K = 2.2 × 10^-6. The reaction favors the formation of products.
C) K = 2.2 × 10^-6. The reaction favors the formation of reactants.
D) K = 4.5 × 10⁵. The reaction favors the formation of products.
E) K = 4.5 × 10⁵. The reaction favors the formation of reactants.