NCERT Class XI Chemistry Equilibrium Solutions

© examsnet.com
Question : 18
Total: 73
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as :
CH3COOH(l)+C2H5OH(l)CH3COOC2H5(l)+H2O(l)
(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?
Solution:  
(i) Qc =
[CH3COOC2H5][H2O]
[CH3COOH][C2H5OH]

(ii) CH3COOH+C5H5OHCH2COOC2H5+H2O
Initially
nCH3COOH = 1.00 ; nC2H5OH = 0.180 and nCH3COOC2H5 = nh2O = 0
At equilibrium :
nCH3COOH = (1.00 − 0.171) = 0.829, nC2H5OH = (0.180 − 0.171) = 0.009
nCH3COOC2H5 = nH2O = 0.171
K =
[CH3COOC2H5][H2O]
[CH3COOH][C2H5OH]
=
(0.171)(0.171)
(0.829)(0.009)
= 3.919
(iii) CH3COOH+C2H5OHCH3COOC2H5+H2O
Initial
nCH3COOH = 1.00 mol, nC2H5OH = 0.500 mol , nCH3COOC2H5 = nH2O = 0
At equilibrium,
nCH3COOH = (1.00 - 0.214) = 0.786 mol,
nC2H5OH = (0.500 - 0.214) = 0.286 mol,
nCH3COOC2H5 = 0.214 and nH2O = 0.214
Qc =
[CH3COOC2H5][H2O]
[CH3COOH][C2H5OH]
=
(0.214)(0.214)
(0.786)(0.286)
= 0.2037
As Qc < K, the equilibrium has not reached. The reaction tends to proceed right, towards products.
© examsnet.com
Go to Question: