A proposed mechanism for the oxidation of nitric oxide to nitrogen dioxide was described in Problem 14.29. Another possible mechanism for this reaction is
(a) Write a balanced equation for the overall reaction.

Verified step by step guidance

1. Identify the reactants and products from the mechanism provided. In this case, the reactants are nitric oxide (NO) and oxygen (O2), and the product is nitrogen dioxide (NO2).
2. Write the chemical formulas for each reactant and product: NO for nitric oxide, O2 for oxygen, and NO2 for nitrogen dioxide.
3. Combine the reactants in a chemical equation: NO + O2 → NO2.
4. Balance the number of atoms of each element on both sides of the equation to ensure the law of conservation of mass is obeyed. This involves adjusting the coefficients of the reactants and products.
5. Verify that the total number of atoms of each element is the same on both sides of the equation to confirm that the equation is balanced.

Key Concepts

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In the context of the oxidation of nitric oxide (NO) to nitrogen dioxide (NO2), NO is oxidized as it loses electrons, while another species must be reduced. Understanding the roles of oxidizing and reducing agents is crucial for identifying the overall reaction mechanism.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on the balanced equation. In the case of the oxidation of nitric oxide, stoichiometry helps determine the molar ratios of NO and O2 needed to produce NO2, facilitating accurate calculations in chemical processes.