The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25°C: CH3CO2H1soln2 + CH3CH2OH1soln2 ∆ Acetic acid Ethanol CH3CO2CH2CH31soln2 + H2O1soln2 Kc = 3.4 (a) How many moles of ethyl acetate are present in an equi- librium mixture that contains 4.0 mol of acetic acid, 6.0 mol of ethanol, and 12.0 mol of water at 25 °C?

검증된 단계별 안내

Identify the balanced chemical equation for the reaction: \( \text{CH}_3\text{CO}_2\text{H} + \text{CH}_3\text{CH}_2\text{OH} \rightleftharpoons \text{CH}_3\text{CO}_2\text{CH}_2\text{CH}_3 + \text{H}_2\text{O} \).

Write the expression for the equilibrium constant \( K_c \): \( K_c = \frac{[\text{CH}_3\text{CO}_2\text{CH}_2\text{CH}_3][\text{H}_2\text{O}]}{[\text{CH}_3\text{CO}_2\text{H}][\text{CH}_3\text{CH}_2\text{OH}]} \).

Substitute the known values into the \( K_c \) expression: \( 3.4 = \frac{x \cdot 12.0}{(4.0 - x)(6.0 - x)} \), where \( x \) is the moles of ethyl acetate at equilibrium.

Rearrange the equation to solve for \( x \), which represents the moles of ethyl acetate.

Use algebraic methods to solve the equation for \( x \), ensuring to check for any assumptions or approximations made during the process.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction provided, Kc = [ethyl acetate][water] / [acetic acid][ethanol]. Understanding Kc helps predict the extent of the reaction and the concentrations of species at equilibrium.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In this case, the stoichiometric coefficients from the balanced equation indicate the molar relationships between acetic acid, ethanol, ethyl acetate, and water, which are essential for determining the moles of ethyl acetate formed at equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance. This principle can be applied to predict how changes in concentration of reactants or products will affect the equilibrium position, which is relevant when analyzing the equilibrium mixture of acetic acid, ethanol, and ethyl acetate.