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Determine the theoretical maximum moles of ethyl acetate, , that could be produced in this experiment. The reactant, acetic acid, is the limiting reagent. (To avoid introducing rounding errors on intermediate calculations, enter your answer to four significant figures.) Theoretical maximum moles of ethyl acetate = mol Reactant mass 11.0 g Product mass 10.8 g Reactant moles 0.1833 mol

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Answer:

0.1832 moles of ethyl acetate ([tex]C_{4}H_{8}O_{2}[/tex])

Explanation:

1. Find the balanced chemical equation:

In the production of ethyl acetate, the acetic acid [tex]CH_{3}COOH[/tex] reacts with ethanol to produce ethyl acetate [tex]C_{4}H_{8}O_{2}[/tex] and water, that is:

[tex]CH_{3}COOH+C_{2}H_{5}OH=C_{4}H_{8}O_{2}+H_{2}O[/tex]

2. Find the theoretical maximum moles of ethyl acetate [tex]C_{4}H_{8}O_{2}[/tex]:

As the problem says that the acetic acid [tex]CH_{3}COOH[/tex] is the limiting reagent, use stoichiometry to find the moles of ethyl acetate produced:

[tex]11gCH_{3}COOH*\frac{1molCH_{3}COOH}{60.05gCH_{3}COOH}*\frac{1molC_{4}H_{8}O_{2}}{1molCH_{3}COOH}=0.1832molesC_{4}H_{8}O_{2}[/tex]

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