Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as :
`CH_(3)COOH(I)+C_(2)H_(5)OH(I) hArrCH_(3)COOC_(2)H_(5)(I)+H_(2)O(I)`
`(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 `293K`, 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 `293K`, `0.214` mol of ethyl acetate is found after sometime. Has equilibrium been reached ?