Question

The diethyl ester of cis-butenedioic acid can be prepared by heating the corresponding anhydride with ethanol and concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in benzene in a mole ratio of perhaps \(1: 2.5: 0.25 .\) Write the steps that occur in this reaction and explain how the use of benzene and more than a catalytic amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) makes the formation of the diethyl ester thermodynamically more favorable than with just a catalytic amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\).

Short answer

Benzene removes water, and excess sulfuric acid pushes equilibrium to favor ester formation.

Step-by-step solution

Identify the reactants and conditions

The reaction involves cis-butenedioic anhydride, ethanol, and concentrated sulfuric acid in the presence of benzene. The mole ratio provided is 1:2.5:0.25, which is important for determining the relative quantities of each reactant.

Mechanism overview: Acid-catalyzed esterification

The reaction is an esterification in which the anhydride reacts with ethanol in the presence of an acid catalyst (sulfuric acid) to form the diethyl ester of cis-butenedioic acid.

Protonation of the anhydride

The concentrated sulfuric acid donates a proton to the oxygen atom of the anhydride. This protonation increases the electrophilicity of the carbon atoms in the carbonyl groups, making them more susceptible to nucleophilic attack by ethanol.

Nucleophilic attack by ethanol

Ethanol, acting as a nucleophile, attacks the more electrophilic carbon atom in the protonated anhydride, leading to the formation of a tetrahedral intermediate.

Formation of the first ester group

The tetrahedral intermediate collapses, losing a molecule of water and forming an ester linkage. The first molecule of ethanol reacts to substitute one of the anhydride's acyl groups.

Formation of the second ester group

A second ethanol molecule attacks the remaining acyl carbon, repeating the process to form the second ester linkage. This generates the diethyl ester.

Role of benzene and excess sulfuric acid

Benzene acts as a solvent that can facilitate the reaction by helping to remove water formed during the reaction. More than a catalytic amount of sulfuric acid serves not only to catalyze the reaction but also to dehydrate the system by sequestering water, pushing the equilibrium towards ester formation.

Key concepts

Acid-Catalyzed Reaction

In an acid-catalyzed reaction, an acid is used to facilitate the transformation of reactants into products. Here, sulfuric acid (\(\text{H}_2\text{SO}_4\)) acts as a catalyst in the esterification process. Catalysts are essential because they lower the activation energy required for reactions, making it easier and faster for the chemical process to occur.
Protonation is a crucial first step in acid-catalyzed reactions. When sulfuric acid donates a proton to the anhydride, it increases the anhydride's reactivity by making the carbonyl carbons more electrophilic. This increased reactivity allows ethanol, as a nucleophile, to easily attack these carbon atoms, leading to the formation of the ester.
Remember, the role of the catalyst isn't to get consumed in the reaction, but to assist and speed up the reaction process.

Organic Chemistry Mechanism

Understanding the mechanism of this esterification is critical for grasping how the reaction unfolds. It starts with the protonation of the anhydride's oxygen, thanks to concentrated sulfuric acid. This modification makes the anhydride more reactive, priming it for attack.

• **Protonation:** Helps in making the carbonyl carbons more electrophilic.
• **Nucleophilic Attack:** Ethanol attacks the carbon of the protonated anhydride, causing the formation of a tetrahedral intermediate.
• **Formation of Tetrahedral Intermediate:** This intermediate is a transient structure where new bonds form, leading to the first ester linkage.

The mechanistic steps repeat as another ethanol molecule attacks the remaining acyl carbon, forming the second ester group. The described series of steps demonstrates how molecular transformations directly lead to the synthesis of an ester through meticulously orchestrated chemical pathways.

Reaction Thermodynamics

Reaction thermodynamics explores the energy changes occurring in a chemical reaction. For esterification, thermodynamic favorability is crucial. Using concentrated sulfuric acid more than just catalytically serves two purposes: catalysis and shifting the equilibrium.
The principle of Le Chatelier's plays a role; by sequestering water (a by-product of the reaction) using sulfuric acid, the equilibrium is pushed towards the ester side, enhancing yield. Benzene, used as a solvent, aids thermodynamically by facilitating the removal of water due to its ability to maintain a less polar environment that favors the formation of non-polar esters.
Thus, both the excess sulfuric acid and benzene ensure the reaction is more efficient and yields more product by tweaking the thermodynamic balance.

Ester Formation

Ester formation involves synthesizing esters from carboxylic acids or their derivatives, such as anhydrides. In our reaction, the anhydride derived from cis-butenedioic acid reacts with ethanol to create the diethyl ester.
Here's how it works:

• **Initial Attack**: Ethanol attacks the activated edifice of the anhydride.
• **Ester Link Formation**: Results from the collapse of the tetrahedral intermediate, releasing water, and forming the ester linkage.
• **Repeat of the Process**: Another ethanol molecule repeats the cycle, forming the second ester group, completing diethyl ester synthesis.

This conversion highlights the dynamic and often iterative nature of esterification, showcasing how precise molecular interactions produce versatile organic products with diverse applications, from food flavorings to pharmaceuticals.