Catalytic converters work to remove nitrogen oxides and carbon monoxide from exhaust. Balance the skeletal equation for one of the reactions that occurs in a catalytic converter. $$ \mathrm{NO}(g)+\mathrm{CO}(g) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{CO}_{2}(g) $$

Catalytic converters are essential components in modern vehicles that reduce harmful emissions from the exhaust system. These emissions, such as nitrogen oxides (NOx) and carbon monoxide (CO), are byproducts of combustion in the engine. The converter's main role is to facilitate a chemical reaction that transforms these toxic gases into less harmful substances like nitrogen (N₂) and carbon dioxide (CO₂).

Catalytic converters use catalysts, typically made of platinum, palladium, and rhodium, to accelerate the chemical reactions without being consumed in the process. When the exhaust gases pass over these catalysts, a redox reaction occurs, where reduction and oxidation happen simultaneously, effectively cleaning the exhaust before it exits the vehicle.

Balancing chemical equations is a fundamental skill in chemistry that ensures the law of conservation of mass is upheld. In a balanced equation, the number of atoms for each element must be the same on both the reactants and products sides. This balance is essential because it indicates that during a chemical reaction, atoms are neither created nor destroyed.

The process usually involves adjusting coefficients—whole numbers placed before chemical formulas—in the equation to achieve this balance. It's important to begin by balancing elements that appear in only one reactant and one product, and to leave diatomic molecules, such as O₂ or N₂, for last. Balancing becomes easier with practice and develops an understanding of the reaction's stoichiometry.

Stoichiometry is the area of chemistry that pertains to the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a given reaction. Stoichiometry is grounded in the mole concept, which provides a way to count atoms and molecules using Avogadro's number (6.022 x 10²³ particles per mole).

To solve stoichiometric problems, one must use a balanced chemical equation, which provides the mole ratios of reactants and products. This ratio is essential for converting between masses, volumes, and particles of substances. Understanding stoichiometry is crucial for many applications, including the formulation of reaction mechanisms in catalytic converters and determining the efficiency of nitrogen oxides reduction.

Nitrogen oxides, or NOx, are a group of gases that include nitric oxide (NO) and nitrogen dioxide (NO₂). These pollutants are notorious for their role in forming smog and acid rain and can have significant adverse effects on human health and the environment. Reducing NOx emissions is a key function of catalytic converters.

The reduction of nitrogen oxides involves converting them into nitrogen gas (N₂), which is inherently harmless as it makes up a significant portion of the Earth's atmosphere. This conversion typically occurs under high temperatures using a reducing agent such as CO. The balanced equation used in the exercise represents one such reaction where NO is reduced to N₂, and CO is oxidized to CO₂. Addressing NOx reduction is paramount to improving air quality and is part of a broader range of strategies aimed at minimizing the environmental footprint of vehicles and industrial processes.