Question

The elementary reaction: \(2 \mathrm{HI} \rightarrow \mathrm{H}_{2}+\mathrm{I}_{2}\), is an example of a reaction. a. Tetramolecular b. Termolecular c. Bimolecular d. Unimolecular

Short answer

The reaction is bimolecular.

Step-by-step solution

Understand Molecularity

Molecularity refers to the number of molecules that come together to react in an elementary reaction. It tells us about the number of reactant molecules involved in a single step of the reaction mechanism.

Analyze the Reaction Equation

Look at the given reaction equation: \( 2 \text{HI} \rightarrow \text{H}_2 + \text{I}_2 \). For this reaction, there are two molecules of \( \text{HI} \) (hydrogen iodide) reacting to form products.

Determine the Molecularity

Since the reaction involves two molecules of a single reactant (\(2 \text{HI}\)), this reaction is classified as bimolecular. Bimolecular reactions involve two reactant molecules coming together.

Key concepts

Elementary reactions

In chemistry, elementary reactions are single-step processes where reactants are directly converted into products. These reactions occur at the molecular level without the formation of intermediates. Understanding elementary reactions is crucial because they form the basis of complex reaction mechanisms.
Elementary reactions can help simplify the process of studying reaction pathways by breaking them down into smaller, manageable parts. The rate law for elementary reactions is directly derived from the stoichiometry of the reaction. This means the molecularity of the reaction dictates the components in the rate law, making it simpler to predict and understand the behavior of the reaction versus more complex, multi-step processes.
In analyzing elementary reactions, it's important to remember that they represent the smallest indivisible steps of a reaction, offering a clear picture of how reactants transform into products.

Bimolecular reactions

Bimolecular reactions are a type of elementary reaction where two reactant molecules collide and react to form products. These reactions are common and occur frequently in chemical processes. The term 'bimolecular' refers specifically to the number of molecules (two) involved in the collision event.
For example, consider the reaction: \[ 2 \text{HI} \rightarrow \text{H}_2 + \text{I}_2 \]This reaction involves two hydrogen iodide molecules coming together to produce hydrogen and iodine gases. Since two molecules are participating in the process, it is classified as bimolecular.
The rate of a bimolecular reaction typically depends on both the concentration and collision efficiency of the reactant molecules. As such, the rate law for bimolecular reactions commonly takes the form: \[ \text{Rate} = k[\text{A}][\text{B}] \]where \([\text{A}]\) and \([\text{B}]\) are the concentrations of the two reactants, and \(k\) is the rate constant. Understanding these dynamics allows chemists to predict how changes in conditions affect reaction rates.

Reaction mechanism

The reaction mechanism is the detailed step-by-step description of how an overall chemical reaction occurs. It breaks down a complex reaction into simpler, elementary steps that detail the transformation from reactants to products. By understanding the mechanism, scientists can gain insights into the molecular changes and possible intermediates formed during the course of the reaction.
Each step in the reaction mechanism corresponds to an elementary reaction, and these are characterized by their molecularity, such as unimolecular, bimolecular, or termolecular. Studying reaction mechanisms involves understanding both the energy changes that occur during each step and the factors affecting the speed or rate of these steps.
The knowledge of a reaction mechanism is essential for designing new reactions and control conditions for desired outcomes, like increasing yield or reducing unwanted by-products. In practical applications, understanding reaction mechanisms leads to better catalysts and more efficient chemical processes. Thus, delving into reaction mechanisms opens up pathways to innovate and optimize chemical reactions for various applications.