How Do You Calculate Keq from a 66.6% Yield in Esterification?

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To calculate the equilibrium constant (Keq) for the esterification of isoamyl acetate with a yield of 66.6%, one must determine the concentrations of both products and reactants. Given that equimolar amounts of reactants were used, 33.4% of the reactants remain unreacted, which allows for the calculation of final concentrations based on an assumed volume. Using the reaction equation, the concentration of the product can be derived from the volume of the unreacted reactants. The equilibrium constant expression can then be formulated as Keq = [product] / [reactants], where stoichiometry is taken into account. This approach effectively utilizes the ICE table method and the relationship C=n/V to find the necessary values for the calculation.
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In the preparation of isoamyl acetate, a student reported a % yield of 66.6%.Assuming that he used equimolar amounts of the starting materials,what is the equilibirium constant of the esterification process?

I need conc of products & conc of reactants to get Keq but how do i get that? They only said that equimolar amounts were used & that means there is no limiting or excess reagent.

All I've managed to get so far is that i need to use the reaction:
CH3CO2H + HOCH2CH2CH(CH3)2 ---> CH3CO2CH2CH2CH(CH3)2 +H2O

Keq= [CH3CO2CH2CH2CH(CH3)2] / [CH3CO2H] [HOCH2CH2CH(CH3)2]

But how do i get these conc.?
 
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You have to assume that volume has not changed and use stoichiometry to calculate final amounts of unreacted rectants. That's in a way similar to using ICE table.

And don't forget C=n/V.

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33.4% of the reactants have not reacted. So if we assume V=100ml that means 33.4ml have not reacted and 66.6 ml is V for the product. Is this correct?
Incase it is, how do i get n? I only need n for one species because its equimolar & stoich is 1:1.
 
Start assuming initially n=1. Write expression for K. Check if volume doesn't cancel out.

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