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Question
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
Write the concentration ratio (reaction quotient), Qc, for this reaction (note: water is not in excess and is not a solvent in this reaction).
Solution
Reaction quotient,
`"Q"_"C" = (["CH"_3"COOC"_2"H"_5]["H"_2"O"])/(["CH"_3"COOH"]["C"_2"H"_5"OH"])`
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Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
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.
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
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?
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