Question

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Classify the following reaction as Arrhenius, Brønsted-Lowry, or Lewis acid-base. The reaction may fit all, two, one, or none of the categories:


N2 + 3 H2 ⇌ 2 NH3

Answer 1

The equation ${{\text{N}}_2} + 3{{\text{H}}_2} \to 2{\text{N}}{{\text{H}}_3}$  does not fit into none of the categories.

Further explanation:

Acids and bases can be defined in many ways based on different theories, which are as follows:

1.Arrhenius theory: According to this theory, acid is defined as the one which produces hydrogen or hydronium ions in a solution, while the base is defined as the one which produces hydroxide ions in a solution. Examples of Arrhenius acids include HBr, ${\text{HN}}{{\text{O}}_3}$ and ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$ while NaOH and KOH are examples of Arrhenius bases.

2.Bronsted-Lowry theory: According to this theory, the acid in the reaction donates a proton while a base is one that accepts a proton. For example, ${{\text{H}}_2}{\text{O}}$ acts as Bronsted acid while ${\text{N}}{{\text{H}}_3}$ is a Bronsted base.

Ammonia accepts a proton from the other species like water and water and therefore acts as Bronsted-Lowry acid as it donates a proton to other species like ${\text{N}}{{\text{H}}_3}$. This can be shown as in equation as follows:

${\text{N}}{{\text{H}}_3} + {{\text{H}}_{\text{2}}}{\text{O}}\to{\text{NH}}_4^ ++ {\text{O}}{{\text{H}}^ - }$  

3.Lewis theory: According to this theory, an acid accepts a pair of electrons to electron-rich species while a base donates electrons to electron-deficient species in the reaction. Examples of Lewis acids are ${\text{B}}{{\text{F}}_3}$, ${\text{S}}{{\text{O}}_3}$ while ${{\text{H}}_2}{\text{O}}$ and ROH are the examples of Lewis base.

 

The given reaction is as follows:

 ${{\text{N}}_2} + 3{{\text{H}}_2} \rightleftharpoons 2{\text{N}}{{\text{H}}_3}$

There is neither transfer of proton between ${{\text{N}}_{\text{2}}}$ and ${{\text{H}}_{\text{2}}}$ nor there is any acceptance or removal of electrons between them. So, the reaction does not fall under the category of Lewis acid-base reactions and Bronsted Lowry acid-base reactions.

${{\text{N}}_{\text{2}}}$ and ${{\text{H}}_{\text{2}}}$ don’t qualify as Arrhenius acid-base reaction as they do not produce hydronium ion or hydroxide ion too in aqueous solution.

So, it is not an acid-base reaction but just a simple combination reaction. ${{\text{N}}_{\text{2}}}$  combines with ${{\text{H}}_{\text{2}}}$ to form ${\text{N}}{{\text{H}}_3}$. Hence, the option will be none of these.

Learn more:

1. what is the structure of bromous acid? https://brainly.com/question/7273171

2. Reason for the acidic and basic nature of amino acid. https://brainly.com/question/5050077

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Acid, base and salts

Keywords: acid, base, electrons, protons, Arrhenius theory, Lewis theory, Bronsted-Lowry theory, hydrogen, hydronium ion, hydroxide ion, accept, donate, ammonia and nitric oxide.