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    Can someone explain how to do this question I just tried it and it's wrong.

    A second method by which ethanoic acid is synthesised involves the oxidative
    fermentation of ethanol in the presence of bacteria. The equation representing this
    reaction is given below.
    C2H5OH + O2 ----> CH3COOH + H2O
    In a small scale experiment using this second method it was found that 23.0 g of ethanol produced only 4.54 g of ethanoic acid. Calculate the percentage yield for this experiment.
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    I'll help get you started.

    percentage yield = (actual mass of product) ÷ (theoretical mass of product) × 100
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    I find it easier to work in terms of moles.

    Find the moles of the limiting reagent (do you understand what I mean by this?) - in this case it will be the ethanol, as it is assumed there is plenty of oxygen!
    Calculate the number of moles of the limiting reagent (ethanol).

    Calculate the number of moles of product.

    Work out the maximum possible number of moles of product, using the stoichiometery of the reaction. In this case it is 1:1.

    Express as a percentage.
 
 
 
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