Question

HC2H3O2(aq) + CN-1(aq) ↔ HCN(aq) + C2H3O2-1(aq)

The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information?

Answer 1

The equilibrium constant of 3.7 x 10^4 indicates that the forward reaction is favored, meaning the products HCN and C2H3O2-1 are favored over the reactants HC2H3O2 and CN-1.

Step-by-step explanation:

The equilibrium constant of 3.7 x 10^4 indicates that the forward reaction is favored. When the equilibrium constant is greater than 1, it means that the products are favored at equilibrium. In this case, the products HCN and C2H3O2-1 are favored over the reactants HC2H3O2 and CN-1.

Answer 2

The reaction favors the formation of HCN(aq) and C₂H₃O₂₋₁ (aq) at equilibrium, as their product concentrations are higher than the reactant concentrations.

Step-by-step explanation:

The given reaction is a chemical equilibrium represented by the equation:

HC₂H₃O₂(aq) + CN₋₁(aq) ↔ HCN(aq) + C₂H₃O₂₋₁(aq)

The equilibrium constant (Kc) for this reaction is 3.7 x 104.

From this information, we can conclude that the reaction favors the formation of HCN(aq) and C₂H₃O₂₋₁(aq) at equilibrium, as their product concentrations are higher than the reactant concentrations.