A characteristic reaction of ethyl acetate is hydrolysis, the reverse of the reaction in Problem 15.87. Write the equilibrium equation for the hydrolysis of ethyl acetate, and use the data in Problem 15.87 to calculate Kc for the hydrolysis reaction.

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

검증된 단계별 안내

Step 1: Write the balanced chemical equation for the hydrolysis of ethyl acetate. The hydrolysis of ethyl acetate (CH3COOC2H5) in the presence of water (H2O) produces ethanol (C2H5OH) and acetic acid (CH3COOH). The equation is: CH3COOC2H5 + H2O \(\rightleftharpoons\) C2H5OH + CH3COOH.

Step 2: Identify the equilibrium expression for the reaction. The equilibrium constant expression (Kc) for the reaction is based on the concentrations of the products and reactants at equilibrium: Kc = \(\frac{[C2H5OH][CH3COOH]}{[CH3COOC2H5][H2O]}\).

Step 3: Use the data from Problem 15.87 to determine the concentrations of the reactants and products at equilibrium. This involves substituting the given equilibrium concentrations into the Kc expression.

Step 4: Calculate the equilibrium constant (Kc) using the equilibrium concentrations. Substitute the equilibrium concentrations into the Kc expression and solve for Kc.

Step 5: Interpret the value of Kc. A large Kc value indicates that the reaction favors the formation of products, while a small Kc value suggests that the reactants are favored at equilibrium.

주요 개념

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Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. Understanding Kc is essential for predicting the direction of a reaction and the extent to which reactants are converted into products.

Hydrolysis Reaction

Hydrolysis is a chemical reaction in which a compound reacts with water, leading to the breakdown of that compound. In the case of ethyl acetate, hydrolysis involves the reaction of ethyl acetate with water to form acetic acid and ethanol. This reaction is important in organic chemistry and is often reversible, meaning it can reach a state of equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle is crucial for understanding how changes in concentration, temperature, or pressure affect the position of equilibrium in reactions such as the hydrolysis of ethyl acetate.