The reaction for formation of nitric acid is more complex...

The reaction for formation of nitric acid is more complex than that shown in Figure $13.10 .$ In the first step, three molecules of nitrogen dioxide react with a water molecule to form nitric acid and nitrogen oxide. In the second step, the nitrogen oxide is oxidized by atmospheric oxygen to nitrogen dioxide, and then the cycle continues. Write balanced equations representing these two steps.

Key Concepts

Chemical Equation Balancing

This concept involves ensuring that the number of atoms for each element is the same on both the reactant and product sides of a chemical equation. Achieving balance adheres to the law of conservation of mass and is fundamental in predicting the quantitative relationships in chemical reactions, including the formation of acids and the oxidation reactions involved in atmospheric processes.

Reaction Mechanism

A reaction mechanism details the step-by-step sequence of elementary reactions through which overall chemical change occurs. Many processes, including the formation of nitric acid, proceed via multiple steps with distinct intermediate species, demonstrating that the overall reaction can be divided into several simpler reactions.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions are chemical processes in which electrons are transferred between species, leading to changes in oxidation states. In atmospheric chemistry, one common example is the oxidation of a gaseous intermediate, where a species like nitrogen oxide is oxidized by oxygen, highlighting the interplay between oxidation and reduction within reaction sequences.

Reaction Intermediates

Reaction intermediates are transient species formed during the multi-step process of a chemical reaction. These intermediates do not appear in the final overall equation but are crucial for understanding the stepwise transformation of reactants into products, as seen in the sequential formation and oxidation steps of nitric acid synthesis.

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