Question

Ethyl acetate \(\left(\mathrm{CH}_{3} \mathrm{COOCH}_{2} \mathrm{CH}_{3}\right)\) is produced in the equilibrium system described by the following equation. \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH} \rightleftharpoons\) $$ \mathrm{CH}_{3} \mathrm{COOCH}_{2} \mathrm{CH}_{3}+\mathrm{H}_{2} \mathrm{O} $$ Why does the removal of water result in the production of more ethyl acetate?

Short answer

The removal of water from the equilibrium system causes the system to shift to the right, in order to restore the original equilibrium and replace the removed water. This shift results in an increased production of ethyl acetate, as more ethanoic acid and ethanol molecules react together to form ethyl acetate and water, according to Le Chatelier's principle.

Step-by-step solution

Understand the reaction and its equilibrium state

The given equilibrium reaction can be written as: \[ \mathrm{CH}_{3} \mathrm{COOH}(\mathrm{a})+\mathrm{CH}_{3}\mathrm{CH}_{2} \mathrm{OH}(\mathrm{b}) \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOCH}_{2} \mathrm{CH}_{3}(\mathrm{c})+\mathrm{H}_{2} \mathrm{O}(\mathrm{d}) \] Initially, the reactants (CH₃COOH and CH₃CH₂OH) and products (CH₃COOCH₂CH₃ and H₂O) are present in certain concentrations. After a while, the system achieves equilibrium, which means the rate of forward reaction (formation of products) equals the rate of reverse reaction (formation of reactants).

Apply Le Chatelier's Principle

Le Chatelier's principle states that if a disturbance is introduced to a system at equilibrium, the system will adjust itself to minimize the effect of the disturbance and restore the original equilibrium. In this case, the disturbance is the removal of water (product) from the system. According to Le Chatelier's principle, the system will react to counteract the disturbance by shifting the equilibrium in the direction that replaces/makes more of the removed species (water in this case).

Shift in Equilibrium and Formation of Ethyl Acetate

As water is removed from the system, the equilibrium shifts to the right to increase the concentration of water. As a result, more ethanoic acid and ethanol molecules react to form ethyl acetate and water, leading to an increased production of ethyl acetate. So, the removal of water leads to the production of more ethyl acetate, as the equilibrium shifts to the right to replace the removed water, according to Le Chatelier's principle.

Key concepts

Le Chatelier's Principle

Le Chatelier's principle is a key concept in understanding how chemical systems respond to changes in conditions. When an equilibrium system, like the production of ethyl acetate from acetic acid and ethanol, is disturbed, the system will adjust to oppose this change and attempt to reestablish balance.
For example, if water, a product in this reaction, is removed from the system, the equilibrium will shift to counterbalance the loss.
This results in the forward reaction being favored to produce more water, consequently generating more ethyl acetate in the process. This dynamic reaction adjustment prioritizes maintaining equilibrium despite external changes.
Understanding this principle is crucial because it provides insight into how equilibriums adapt under varying conditions, helping to optimize chemical processes and predict outcomes in industrial and laboratory settings.

Reaction Kinetics

Reaction kinetics involves the study of reaction rates and the steps by which reactions occur. In the context of ethyl acetate synthesis, understanding the kinetic factors can help determine the speed at which equilibrium is reached. Various factors like temperature, concentration of reactants, and catalysts influence reaction rates.
Increasing the concentration of reactants, like acetic acid and ethanol, can lead to higher rates of reaction towards forming ethyl acetate.
Similarly, temperature can play a significant role; higher temperatures often increase reaction rates by providing more energy to overcome activation barriers.
Catalysts, although not changing the equilibrium position, can ramp up the rate at which equilibrium is achieved by lowering the energy requirements for the reaction. Thus, reaction kinetics is pivotal in understanding the practical aspects of how and when equilibrium is reached during chemical synthesis.

Equilibrium Shift

An equilibrium shift occurs when a change in concentration, temperature, or pressure leads to the system adjusting to reestablish a new equilibrium position. In the reaction to produce ethyl acetate, if water is removed, this triggers an equilibrium shift.
The system, following Le Chatelier's principle, shifts to the right to produce more water and ethyl acetate. Such shifts can be manipulated deliberately to enhance product yields.
For example, continuously removing a reaction product can encourage the forward reaction, leading to greater amounts of desired substances.
Understanding equilibrium shifts allows chemists to design processes that maximize output and minimize resources, which is critical in both academic research and industrial applications.

Organic Synthesis

Organic synthesis is the science of constructing organic molecules through chemical reactions. Producing ethyl acetate demonstrates such a synthesis, where simpler organic molecules (acetic acid and ethanol) undergo a chemical reaction to yield a more complex compound.
This process embodies the principles of designing and executing chemical reactions to build novel molecular structures. Organic synthesis is fundamental in manufacturing a wide array of products including pharmaceuticals, agrochemicals, and polymers.
In the context of ethyl acetate production, understanding reaction conditions like equilibrium shifts and reaction kinetics is essential for optimizing the synthesis process.
Thus, knowledge of organic synthesis not only assists in theoretical understanding but is crucial for practical applications across various chemical industries.