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Acid-catalysed hydrolysis of ethyl acetate in dilute aqueous solution, , is bimolecular but is found to follow first order kinetics. The reason is that

  1. Awater acts as a catalyst and does not appear in the rate law
  2. Bthe concentration of ethyl acetate remains constant during the reaction
  3. Cthe acid is consumed in the reaction
  4. Dwater is present in such large excess that its concentration remains practically constant

Answer: D

The true rate law is rate = . Since (about 55 M) changes negligibly, is constant and rate = , so the reaction is pseudo first order.
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