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Grace [21]
3 years ago
7

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
Chemistry
1 answer:
kherson [118]3 years ago
4 0

Answer:

0.1832 moles of ethyl acetate (C_{4}H_{8}O_{2})

Explanation:

1. Find the balanced chemical equation:

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

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

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

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

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}

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