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Question
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
\[\ce{CH3COOH (l) + C2H5OH (l) ⇌ CH3COOC2H5 (l) + H2O (l)}\]
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
Let the volume of the reaction mixture be V.
| CH3COOH(l) | + | C2H5OH(l) | ↔ | CH3COOC2H5(l) | + | H2O(l) | |
| Initial conc. | `1.0/"V"`M | `0.5/"V"`M | 0 | 0 | |||
| After some time | `(1.0 - 0.214)/"V"` | `(0.5 - 0.214)/"V"` | `0.214/"V"`M | `0.214/"V"`M | |||
| `= 0.786/"V"`M | `= 0.286/"V"`M |
Therefore, the reaction quotient is,
`"Q"_"C" = (["CH"_3"COOC"_2"H"_5]["H"_2"O"])/(["CH"_3"COOH"]["C"_2"H"_5"OH"])`
`= (0.214/"V" xx 0.214/"V")/(0.786/"V" xx 0.286/"V")`
= 0.2037
= 0.204 (approximatly)
Since `"Q"_"c" < "K"_"c"` equilibrium has not been reached.
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