Textbook Question
Calculate the equilibrium concentrations at 25 °C for the reaction in Problem 15.84 if the initial concentrations are 3N2O44 = 0.0200 M and 3NO24 = 0.0300 M.
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 88
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.
Verified step by step guidance1
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.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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.
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Equilibrium Constant Expressions
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.
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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.
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Related Practice
Textbook Question
The industrial solvent ethyl acetate is produced by the reac-tion of acetic acid with ethanol:CH3CO2H1soln2 + CH3CH2OH1soln2 ∆CH3CO2CH2CH31soln2 + H2O1soln2Ethyl acetate (b) A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 mol of ethyl ace- tate at equilibrium. Calculate the value of Kc. Explain why you can calculate K without knowing the volume of the solution.
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Textbook Question
The following reaction, which has Kc = 0.145 at 298 K, takes place in carbon tetrachloride solution:2 BrCl1soln2 ∆ Br21soln2 + Cl21soln2 A measurement of the concentrations shows 3BrCl4 =0.050 M, 3Br24 = 0.035 M, and 3Cl24 = 0.030 M. (b) Determine the equilibrium concentrations of BrCl, Br1, and Cl2.
Textbook Question
An equilibrium mixture of N2, H2, and NH3 at 700 K con- tains 0.036 M N2 and 0.15 M H2. At this temperature, Kc for the reaction N21g2 + 3 H21g2 ∆ 2 NH31g2 is 0.29. What is the concentration of NH3?
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