NCERT Class XI Chemistry Equilibrium Solutions
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Question : 18
Total: 73
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as :
C H 3 C O O H ( l ) + C 2 H 5 O H ( l ) ⇌ C H 3 C O O C 2 H 5 ( l ) + H 2 O ( l )
(i) Write the concentration ratio (reaction quotient),Q c , 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?
(i) Write the concentration ratio (reaction quotient),
(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) Q c =
(ii)C H 3 C O O H + C 5 H 5 O H ⇌ C H 2 C O O C 2 H 5 + H 2 O
Initially
n C H 3 C O O H = 1.00 ; n C 2 H 5 O H = 0.180 and n C H 3 C O O C 2 H 5 = n h 2 O = 0
At equilibrium :
n C H 3 C O O H = (1.00 − 0.171) = 0.829, n C 2 H 5 O H = (0.180 − 0.171) = 0.009
n C H 3 C O O C 2 H 5 = n H 2 O = 0.171
K =
=
= 3.919
(iii)C H 3 C O O H + C 2 H 5 O H ⇌ C H 3 C O O C 2 H 5 + H 2 O
Initial
n C H 3 C O O H = 1.00 mol, n C 2 H 5 O H = 0.500 mol , n C H 3 C O O C 2 H 5 = n H 2 O = 0
At equilibrium,
n C H 3 C O O H = (1.00 - 0.214) = 0.786 mol,
n C 2 H 5 O H = (0.500 - 0.214) = 0.286 mol,
n C H 3 C O O C 2 H 5 = 0.214 and n H 2 O = 0.214
Q c =
=
= 0.2037
AsQ c < K, the equilibrium has not reached. The reaction tends to proceed right, towards products.
(ii)
Initially
At equilibrium :
K =
(iii)
Initial
At equilibrium,
As
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