Sarthaks APP
+1 vote
3.1k views
in Chemistry by (29.7k points)

Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as: 

(i) Write the concentration ratio (reaction quotient), Qc, for this reaction (note: water is not in excess and is not a solvent in this reaction) 

(ii) At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant. 

(iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. Has equilibrium been reached? 

1 Answer

+1 vote
by (128k points)
selected by
 
Best answer

(i) Reaction quotient, 

(ii) Let the volume of the reaction mixture be V. Also, here we will consider that water is a solvent and is present in excess. 

The given reaction is

Therefore, equilibrium constant for the given reaction is: 

(iii) Let the volume of the reaction mixture be V. 

Sarthaks APP

Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students.

Categories

...