Final answer:
If 4.2 L of N₂ reacts completely with 6.3 L of O₂ under constant temperature and pressure to form dinitrogen trioxide, according to the stoichiometry of the balanced equation and Avogadro's law, the volume of N₂O₃ produced will be 4.2 L.
Step-by-step explanation:
Based on the chemical equation provided (2 N₂(g) + 3 O₂(g) → 2 N₂O₃(g)), we can analyze the reaction between nitrogen and oxygen to form dinitrogen trioxide. Using the stoichiometry of the reaction, we know that two volumes of nitrogen will react with three volumes of oxygen to produce two volumes of dinitrogen trioxide. Given that 4.2 L of N₂ reacts with 6.3 L of O₂, and taking into account the stoichiometry ratio from the balanced equation, we expect to produce an equal volume of dinitrogen trioxide as the volume of nitrogen that reacted, which is 4.2 L.
In chemical reactions at constant temperature and pressure, the volume of gasses consumed and produced aligns with the mole ratio presented in the balanced equation, according to Avogadro's law. Since 4.2 L of N₂ corresponds to 2 moles of nitrogen gas in the reaction, the produced volume of N₂O₃ will also correspond to 2 moles. Consequently, the volume of N₂O₃ gas produced will be 4.2 L, assuming complete consumption of both reactants and that the gases behave ideally.