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Nitrogen oxides, commonly referred to as NO\(_x\), are a group of gases that includes nitrogen monoxide (NO) and nitrogen dioxide (NO\(_2\)). These gases are significant air pollutants due to their role in the formation of smog and acid rain. Understanding their chemical behavior is important for environmental science.
NO, a colorless gas, and NO\(_2\), a reddish-brown gas, are typically produced by combustion processes in vehicles and industries. These oxides of nitrogen contribute to air quality problems when they react with sunlight, water, and other compounds in the atmosphere.
Efforts to control NO\(_x\) emissions focus on reducing vehicle emissions, using technologies like catalytic converters, which chemically transform NO and NO\(_2\) into less harmful substances before they exit the vehicle's exhaust system.

Catalytic converters are crucial components in vehicle exhaust systems that help reduce harmful emissions. They are designed to convert toxic pollutants into less harmful emissions through catalyzed chemical reactions.
The converter contains a core of ceramic or metal coated with catalysts, typically platinum, palladium, and rhodium, which facilitate the conversion of gases without being consumed. When exhaust gases pass through the converter, reactions take place that change NO and NO\(_2\) into nitrogen gas (N\(_2\)) and oxygen gas (O\(_2\)). This process significantly reduces the emission of nitrogen oxides, contributing to cleaner air.
In addition to reducing nitrogen oxides, catalytic converters also work to lessen other harmful emissions such as carbon monoxide and hydrocarbons, promoting a cleaner environment.

Balanced chemical equations are fundamental in understanding and describing chemical reactions. A balanced equation ensures that there is an equal number of each type of atom on both sides of the reaction, adhering to the law of conservation of mass.
For the decomposition of NO into N\(_2\) and O\(_2\), the balanced chemical equation is:

• 2NO \(\rightarrow\) N\(_2\) + O\(_2\)

For NO\(_2\), the balanced equation is slightly different due to the additional oxygen relative to NO:

• 2NO\(_2\) \(\rightarrow\) N\(_2\) + 2O\(_2\)

In both equations, notice that the coefficients ensure the number of each atom is the same on both sides. Balancing these equations is an essential step in predicting the products of a reaction and in performing stoichiometric calculations.

Molar mass calculations are vital for translating between mass and moles in chemical reactions. The molar mass is the weight of one mole of a given substance and is measured in grams per mole (g/mol).
For nitrogen monoxide (NO), the molar mass is calculated by adding the atomic masses of nitrogen (14 g/mol) and oxygen (16 g/mol), resulting in a molar mass of 30 g/mol. Similarly, for nitrogen dioxide (NO\(_2\)), the molar mass is found by adding the atomic mass of nitrogen (14 g/mol) and twice the atomic mass of oxygen (32 g/mol), resulting in 46 g/mol.
Understanding how to calculate molar mass enables you to convert between grams and moles, which is crucial for determining the quantities of reactants and products involved in chemical equations. For example, in the exercise, knowing the molar masses is necessary to determine how many grams of each gas (NO and NO\(_2\)) are produced by the car.