Final answer:
The equation 'O3 + NO → O2 + NO2' involves reacting ozone with nitrogen oxide to form oxygen and nitrogen dioxide. Initial concentrations can be used for calculating the reaction quotient, and knowledge of equilibrium constants helps predict reaction behavior.
Step-by-step explanation:
The chemical reaction described by the equation O3 + NO → O2 + NO2 involves ozone (O3) reacting with nitrogen oxide (NO) to form oxygen (O2) and nitrogen dioxide (NO2). The presented concentrations, 8.0x10⁻⁴ M for O3 and 3.0x10⁻⁵ M for NO are likely to be the initial concentrations of the reactants before the reaction reaches equilibrium. In the context of chemical kinetics and equilibrium, these concentrations can be used to calculate the reaction quotient (Q) and compare it to the equilibrium constant (K) to predict which direction the reaction will proceed to reach equilibrium. Additionally, providing the equilibrium constants for sequential reactions involving N2 and O2 to form NO, and subsequently, NO2, helps in understanding the overall reaction mechanism that contributes to the formation of smog. These constants are given for reactions occurring at 100°C, where the formation of NO from N2 and O2 has a very small K1 value of 2.0 × 10⁻‥, indicating little NO production, and the subsequent reaction of NO with O2 to form NO2 has a much larger K2 value of 6.4 × 10⁹. The equation 2NO(g) + O2(g) → 2NO2(g) with reaction rates could also be relevant if it involves kinetic studies or rate expressions based on stoichiometric coefficients from the balanced equation.