Question

Refer to the reaction performed in the Homogeneous Equilibrium Experiment:

Acetic Acid + Ethanol <--> Ethylacetate + water

A student mixes the following volumes together in a reaction flask:
-HCl 0.00mL
-Acetic Acid 1.00 mL
-Ethanol 1.00mL
-Ethylacetate 4.00 mL
-Water 0.00 mL

Which of the following is true concerning the equilibrium reaction under study?

a) The reaction will shift to the right
b) The reaction is at equilibrium
c) The reaction will shift to the left
d) The reaction will not occur
e) None of the above

Answer 1

Ans. Le Chatelier’s principle states “if a dynamic equilibrium is disturbed by changing the conditions (Concentration, Volume, Pressure, temperature, etc.), the position of equilibrium shifts to counteract the change to reestablish an equilibrium”.

# HCl is not involved in equilibrium terms. [HCl] is also 0.0. So, ignore HCl.

#. Water is generally not involved in equilibrium term. However, water is a product in this reaction. If the reaction takes place, there must be formation of water molecules for the equilibrium to be established.

# To establish equilibrium, the reaction mixture must also produce some water. To produce water molecules, the reaction must proceed to the right.

Therefore, correct option is A. The reaction will shift to the right.

# Option B. Incorrect. The reaction is NOT at equilibrium because there is no water molecules added to the reaction mixture.

Option C. Incorrect. See XA.

Option D. Incorrect. The reaction will occur because the required reactants are provided in the reaction mixture and the reaction must proceed to the right to attain equilibrium.