An acid-base reaction proceeds predominantly in the direction that forms the weaker acid and the weaker base. Based on this principle, which of the following reactions is thermodynamically feasible in the forward direction?

Step-by-step solution

For an acid-base equilibrium to be favored in the forward direction, the reactant acid must be stronger than the product acid. We compare the acidity of the hydrocarbons based on the hybridization of the carbon atom holding the acidic proton ( sp > sp^2 > sp^3 ). In the first option, the reactant acid is ethene ( sp^2 ) and the product acid is ethyne ( sp ). Since ethyne is a stronger acid than ethene, the backward reaction is favored. In the second option, the reactant acid is propyne ( sp ) and the product acid i