In an esterification reaction How many moles of ester are produced
at equilibrium when 1 mole of acetic acid and 3 moles of ethanol are reacted together? (kc = 4.0]
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Let initially, 1 mole of ethanol and 1 mole of acetic acid is present.
Let x moles of ethanol reacts with x moles of acetic acid to reach equilibrium.
Ethanol
Acetic acid
Ethyl acetate
Water
Equilibrium number of moles
1−x 1−x
x
x
The total number of moles =1−x+1−x+x+x=2
The mole fraction of water at equilibrium is
2
x
=0.333
Hence, x=0.666 and 1−x=0.334
The equilibrium constant expression is
K=
[ethanol][acetic acid]
[Ethyl acetate[Water]]
K=
0.334×0.334
0.666×0.666
K=4
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